Answer:
There are 1000 milliliters (ml) in one liter. Therefore, the teacher has a total of 6 x 1000 = 6000 ml of sodium nitrate solution.
Explanation:
To divide the solution evenly among the 24 students, we need to divide the total volume of the solution by the number of students:
6000 ml ÷ 24 students = 250 ml per student
Therefore, each student will receive 250 milliliters of sodium nitrate solution.
Answer:
Answer- 0.25ml
Explanation:
So there are 24 students and 6 liters of Solution.So to evenly distribute
Just divide 6 by 24(6÷24/)... So the answer will be 0.25
You react 0.017 mol of solid metal with HCl in a coffee cup calorimeter (reaction shown below). The calorimeter has 100 mL of water in it, and the temperature of the water increases by 3.81°C. The calorimeter has a heat capacity of 40.4 J/°C. What is the enthalpy of the reaction in terms of kJ per mol of the metal (your answer should be NEGATIVE, remember to convert from J to kJ, specific heat capacity of water is 4.184 J/g-°C)?
M(s) + 2 HCl (aq) MCl2 (aq) + H2 (g)
M = metal
A sample of an ideal gas has a volume of 3.75 L
at 10.60 ∘C
and 1.80 atm.
What is the volume of the gas at 23.20 ∘C
and 0.990 atm?
The volume of the gas at 23.20∘C and 0.990 atm is 7.12L.
How to calculate volume?The volume of a gas can be calculated using the combined gas law equation as follows;
PaVa/Ta = PbVb/Tb
Where;
Pa, Va and Ta = initial pressure, volume and temperature respectively Pb, Vb and Tb = final pressure, volume and temperature respectivelyAccording to this question, a sample of an ideal gas initially has a volume of 3.75 L at 10.60 ∘C and 1.80 atm. The resulting volume can be calculated as follows;
1.8 × 3.75/283.6 = 0.990 × Vb/296.2
0.0238 × 296.2 = 0.990Vb
Vb = 7.0498 ÷ 0.990
Vb = 7.12L
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WHEN SOME PEOPLE HAVE AN UPSET STOMACH, THEY TAKE A SODA TABLET LIKE
TUMS TO NEUTRALIZE THEIR STOMACH ACID.
THE REACTION IS HYDROCHLORIC ACID PLUS SODIUM BICARBONATE MAKES SALT,
CARBON DIOXIDE (THAT'S WHY SOME PEOPLE BURP) AND WATER.
HOW MUCH CARBON DIOXIDE AND SALT (IN GRAMS) ARE PRODUCED IF A 2 GRAM
TABLET OF SODIUM BICARBONATE IS TAKEN TO REACT WITH 18 GRAMS OF
HYDROCHLORIC ACID?
The balanced chemical equation for the reaction between hydrochloric acid (HCl) and sodium bicarbonate [tex](NaHCO_3)[/tex] is:
[tex]HCl + NaHCO_3\ - > NaCl + CO_2 + H_2O[/tex]
The coefficients in the balanced equation show that 1 mole of HCl reacts with 1 mole of [tex]NaHCO_3[/tex] to produce 1 mole of NaCl, 1 mole of [tex]CO_2[/tex], and 1 mole of [tex]H_2O[/tex]. We need to find the number of moles of [tex](NaHCO_3)[/tex] present in the tablet.
2 grams of [tex]NaHCO_3[/tex] is equivalent to 0.02 moles, and 18 grams of HCl is equivalent to 0.45 moles. Since [tex](NaHCO_3)[/tex] is limiting reagent, only 0.02 moles of NaCl and [tex]CO_2[/tex] will be produced. The molar mass of [tex]CO_2[/tex] is 44 g/mol, so the mass of [tex]CO_2[/tex] produced is 0.88 g. The molar mass of NaCl is 58.44 g/mol, mass of NaCl produced is 1.17 g.
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Mark needs to determine how much the temperature of a solution changes during a chemical reaction. Which tool does he need?
Mark would need a thermometer to determine the temperature change of a solution during a chemical reaction. A thermometer is a tool used to measure temperature and can be used to monitor and record changes in temperature during a chemical reaction. So the answer is thermometer .
There are different types of thermometers, such as liquid-in-glass thermometers, bimetallic strip thermometers, digital thermometers, and infrared thermometers, among others. The choice of thermometer depends on the specific requirements of the experiment or process being carried out.
By measuring the initial and final temperatures of the solution before and after the chemical reaction, Mark can determine the temperature change, which is an important parameter in many chemical reactions as it provides information about the heat energy involved in the reaction, and helps in understanding the thermodynamics and kinetics of the process. Therefore the answer is thermometer .
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Water can dissolve many substances because-
-
it has a partial charge on each side of its molecules
it has a linear molecular shape
it has a nonpolar molecular structure
it has the molecular formula H₂O
Answer:
Water can dissolve many substances because it has a partial charge on each side of its molecules.
Explanation:
Water is a polar molecule, meaning that it has an uneven distribution of electrons between its hydrogen and oxygen atoms. This creates a partial negative charge on the oxygen side of the molecule and a partial positive charge on the hydrogen side. These partial charges allow water molecules to attract and surround other charged or polar molecules, such as ions and polar compounds, and separate them from each other. This process of surrounding and separating other substances in a solution is known as hydration or dissolution, and it is what allows water to dissolve many substances. Therefore, the correct option is: "it has a partial charge on each side of its molecules."
Please help I appreciate it thanks!!!!!!!!!!!!!!!!!!!!!!
The correct molar mass for nickel chloride is 94.14 g/mol (option C).
How to calculate molar mass?Molar mass is the mass of a given substance divided by its amount, measured in moles. It is commonly expressed in grams (sometimes kilograms) per mole.
The molar mass of a substance can be calculated by summing up the atomic masses of the element components.
According to this question, the atomic mass of nickel is 58.693 amu while that of chlorine gas is 35.45 amu. The molar mass of nickel chloride can be calculated as follows;
molar mass = 35.45 amu + 58.693 amu = 94.14 g/mol
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One way to cool down your cup of coffee is to plunge an ice-cold piece of aluminum into it. Suppose you store an 18 g piece of aluminum in the refrigerator at 4.4°C, and drop it into your coffee. The coffee temperature drops from 90.0°C to 55.0°C. How much kJ of heat energy did the aluminum block absorb?
Note: The specific heat of aluminum is 0.89 J/g °C.
Do not round your answer in the middle of the problem, round at the very end.
Round your answer to the proper number of sig figs. Don't forget your units.
The aluminum block absorbed 0.875 kJ of heat energy when it was dropped into the coffee.
let's calculate the heat lost by the coffee when it is cooled from its initial temperature of 90.0°C to its final temperature of 55.0°C:
Q1 = m1 * C1 * (90.0°C - 55.0°C)
Q1 = 850 g * 4.184 J/g °C * (90.0°C - 55.0°C)
Q1 = 125660 J
where m1 is the mass of the coffee, C1 is the specific heat of water.
Next, let's calculate the heat gained by the aluminum block when it is heated from 4.4°C to the final temperature of the mixture, which is 55.0°C:
Q2 = m2 * C2 * (55.0°C - 4.4°C)
Q2 = 18 g * 0.89 J/g °C * (55.0°C - 4.4°C)
Q2 = 875.16 J
where m2 is the mass of the aluminum block, and C2 is the specific heat of aluminum.
Since the energy lost by the coffee is gained by the aluminum block, we can set Q1 equal to Q2:
Q1 = Q2
125660 J = 875.16 J + m2 * C2 * (55.0°C - 4.4°C)
Solving for m2, we get:
m2 = (125660 J - 875.16 J) / (0.89 J/g °C * (55.0°C - 4.4°C))
m2 = 152.2 g
Therefore, the mass of the aluminum block that was dropped into the coffee is 152.2 g. To calculate the heat energy absorbed by the aluminum block, we can use the heat gained by the aluminum block that we calculated earlier:
Q2 = 875.16 J
Converting this to kJ, we get:
Q2 = 0.875 kJ
Therefore, the aluminum block absorbed 0.875 kJ of heat energy when it was dropped into the coffee.
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PLEASE HELP!
Distilled vinegar contains a solution of acetic acid (CH3CO2H) in H2O. Using the formula M1V1=M2V2, solve for the concentration of the solution that results from diluting 0.50 L of 0.839 M vinegar solution to 2.5 L?
Question 4 options:
0.15 M
0.24 M
0.17 M
1.49 M
How many moles are in 28g of CO2?
Answer:
0.636 moles of CO2
Explanation:
The molar mass of CO2 is 44.01 g/mol (12.01 g/mol for one carbon atom and 2 x 16.00 g/mol for two oxygen atoms). To find the number of moles in 28g of CO2, you can divide the mass by the molar mass: 28g / 44.01 g/mol = 0.636 moles of CO2.
A sample of gas is contained in a 245 mL flask at a temperature of 23.5°C. The gas pressure is 37.8 mm Hg. The gas is moved to a new flask, which is then immersed in ice water, and which has a volume of 54 mL. What is the pressure of the gas in the smaller flask at the new temperature?
The pressure of the gas in the smaller flask at the new temperature is approximately 168.5 mm Hg.
To solve this problem, we can use the combined gas law equation, which relates the initial and final states of a gas sample undergoing changes in pressure, volume, and temperature. The equation is:
[tex]P_1V_1/T_1 = P_2V_2/T_2[/tex]
where [tex]P_1[/tex] and [tex]P_2[/tex] are the initial pressure and final pressure, [tex]V_1[/tex] and [tex]V_2[/tex] are the initial and final volumes, and [tex]T_1[/tex] and [tex]T_2[/tex] are the initial and final temperatures in Kelvin.
[tex]V_1[/tex] = 245 mL
[tex]T_1[/tex] = 23.5°C + 273.15 = 296.65 K
[tex]P_1[/tex] = 37.8 mm Hg
[tex]V_2[/tex] = 54 mL
[tex]T_2[/tex] = 0°C (ice water) + 273.15 = 273.15 K
We need to find [tex]P_2[/tex] . Plug the given values into the equation and solve for [tex]P_2[/tex] :
(37.8 mm Hg * 245 mL) / 296.65 K = (P2 * 54 mL) / 273.15 K
Rearrange the equation to isolate [tex]P_2[/tex] :
[tex]P_2[/tex] = (37.8 mm Hg * 245 mL * 273.15 K) / (296.65 K * 54 mL)
[tex]P_2[/tex] ≈ 168.5 mm Hg
So, the pressure of the gas is approximately 168.5 mm Hg in the smaller flask at the new temperature.
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How many grams of O are in 615g of N2O?
There are approximately 223.2 grams of oxygen in 615 grams of N2O.
To find the number of grams of O in 615g of N2O, we first need to understand the chemical formula of N2O. N2O is a compound made up of two nitrogen atoms (N) and one oxygen atom (O). Therefore, the molecular weight of N2O would be:
(2 x atomic weight of N) + (1 x atomic weight of O)
= (2 x 14.01 g/mol) + (1 x 16.00 g/mol)
= 44.01 g/mol
Now, to calculate the number of grams of O in 615g of N2O, we need to know the proportion of O in the compound. Since there is only one oxygen atom in each molecule of N2O, we can find the proportion of O by dividing the atomic weight of O by the molecular weight of N2O:
Atomic weight of O / Molecular weight of N2O
= 16.00 g/mol / 44.01 g/mol
= 0.363
This means that oxygen makes up 36.3% of the total weight of N2O. To find the number of grams of O in 615g of N2O, we can multiply the total weight by the proportion of O:
615g x 0.363
= 223.2g
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1. While doing a calorimetry experiment, you notice the temperature of 50.0 g of water changes by 7ºC. What is the energy of the chemical reaction? (Cwater= 4.18 J/g*°C)
2. Which of the following is an example of a kinetic energy change?
Hydrazine, N2H4
, reacts with oxygen to form nitrogen gas and water.
N2H4(aq)+O2(g)⟶N2(g)+2H2O(l)
If 3.55 g
of N2H4
reacts with excess oxygen and produces 0.850 L
of N2
, at 295 K
and 1.00 atm,
what is the percent yield of the reaction?
Hydrazine, reacts with the oxygen to form the nitrogen gas and the water. The percent yield of the reaction is 3.18 %.
The balanced reaction is :
N₂H₄ + O₂ ---> N₂ + 2H₂O
The mass of the N₂H₄ = 3.55 g
The moles of N₂H₄ = mass / molar mass
The moles of N₂H₄ = 3.55 / 32
The moles of N₂H₄ = 0.110 mol
The theoretical yield = 0.110 mol × 28 g/mol
The theoretical yield = 3.08 g
The gas equation is :
P V = n R T
n = P V / R T
n = (1 × 0.850 ) / ( 0.0823 ×295 )
n = 0.0035 mol
The actual yield = 0.0035 × 28
The actual yield = 0.098 g
The percent yield = ( 0.098 / 3.08 ) × 100 %
The percent yield = 3.18 %.
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If an atom loses an electron, what will its resulting charge be?
Answer:
If an atom loses or gains electrons, it will become a positively or negatively charged particle, called an ion. The loss of one or more electrons results in more protons than electrons and an overall positively charged ion, called a cation.
Hope it helped! :)
Here are some data from a similar experiment, to determine the empirical formula of on oxide of tin.
Calculate the empirical formula according to these data.
Mass of crucible, cover, and tin sample 21.76 g
Mass of empty crucible with cover 19.66 g
Mass of crucible and cover and sample,
after prolonged heating gives constant weight 22.29 g
The information given can be used to construct the empirical formula for a tin oxide. We must first determine the mass of tin in the sample. This may be achieved by deducting the mass of the crucible, cover, and sample (21.76 g) from the mass of the empty crucible and cover (19.66 g).
This gives us a mass of 2.10 g of tin in the sample. The mass of oxygen in the sample must then be determined. To achieve this, we must deduct the mass of the crucible, cover, and sample (21.76 g) from the mass of the same components (22.29 g) prior to protracted heating. This provides us with an oxygen mass of 0.53 g.
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What is the minimum concentration of fluoride ions necessary to precipitate CaF2 from a 5.25 x 10-3 M solution of Ca(NO3)2? Ksp of CaF2 = 3.9 x 10-11
The minimum concentration of fluoride ions necessary to precipitate [tex]CaF_2[/tex] from a [tex]5.25 * 10^{-3}[/tex] M solution of [tex]Ca(NO_3)_2[/tex] is [tex]6.09 * 10^{-5}[/tex] M.
The solubility product expression for [tex]CaF_2[/tex] is:
[tex]Ksp = [Ca_2^+}][F^-]^2[/tex]
We can use this expression to find the minimum concentration of fluoride ions necessary to precipitate [tex]CaF_2[/tex] from a [tex]5.25 * 10^{-3} M[/tex] solution of [tex]Ca(NO_3)_2[/tex].
First, we need to determine the initial concentration of [tex]Ca_2^+[/tex] ions in solution. Since [tex]Ca(NO_3)_2[/tex] dissociates into two [tex]Ca_2^+[/tex] ions and two [tex]NO_3^-[/tex]ions, the initial concentration of [tex]Ca_2^+[/tex] ions is:
[tex]Ca_2^+[/tex] = [tex]2 * 5.25 * 10^{-3} M = 1.05 * 10^{-2} M[/tex]
Next, we can use the solubility product expression to solve for the minimum concentration of fluoride ions required to precipitate [tex]CaF_2[/tex]:
Ksp = [[tex]Ca_2^+[/tex]][tex][F^-]^2[/tex]
[tex]3.9 * 10^{-11} = (1.05 * 10^{-2} M)([F^-]^2)[/tex]
[tex][F^-]^2 = (3.9 * 10^{-11})/(1.05 * 10^{-2} M) = 3.71 * 10^{-9}[/tex]
[tex][F^-] = \sqrt{(3.71 * 10^{-9}) } = 6.09 * 10^{-5} M[/tex]
Therefore, the minimum concentration of fluoride ions necessary to precipitate [tex]CaF_2[/tex] from a [tex]5.25 * 10^{-3}[/tex] M solution of [tex]Ca(NO_3)_2[/tex] is [tex]6.09 * 10^{-5}[/tex]M.
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What is the molar volume of CO2 at 39 C and 652 torr?
The molar volume of a gas can be calculated using the ideal gas law:
PV = nRT
where P is the pressure of the gas in atmospheres (atm), V is the volume of the gas in liters (L), n is the number of moles of gas, R is the ideal gas constant (0.08206 L·atm/mol·K), and T is the temperature of the gas in Kelvin (K).
To solve for the molar volume of CO2 at 39°C (312 K) and 652 torr (0.859 atm), we can rearrange the ideal gas law as follows:
V = (nRT) / P
First, we need to calculate the number of moles of CO2. We can use the following equation, which relates the pressure, volume, number of moles, and temperature of a gas:
PV = nRT
Solving for n, we get:
n = (PV) / (RT)
Substituting the given values, we get:
n = (0.859 atm * V) / (0.08206 L·atm/mol·K * 312 K)
Now we can substitute this expression for n into the equation for the molar volume:
V = (nRT) / P
V = [(0.859 atm * V) / (0.08206 L·atm/mol·K * 312 K)] * (0.08206 L·atm/mol·K * 312 K) / (0.859 atm)
Simplifying, we get:
V = 24.45 L/mol
Therefore, the molar volume of CO2 at 39°C and 652 torr is 24.45 L/mol.
Convert the following number
into correct scientific notation.
0.0602 x 10^25
[ ? ] × 10 [ ? ]
The number is converted to 60. 2 × 10²²
What are index forms?Index forms are simply described as mathematical forms that are used in the representation of numbers that are too small or too large in more convenient forms.
These index forms are also referred to as scientific notation or standard forms.
Some rules of index forms are;
Add the exponents when multiplying forms of the same basesSubtract the exponents when dividing forms of the same basesFrom the information given, we have that;
0. 0602 × 10 ²⁵
Subtract three from the exponent value and move three spaces right, we have;
60. 2 × 10²⁵⁻³
60. 2 × 10²²
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Please help thanks so much!!!!!!!!!!!!
The total mass of products obtained when 130 g of zinc react completely with HCl is 274 g (3rd option)
How do i determine the total mass of products obtained?First, we shall determine the mass of each product obtained. Details below:
For ZnCl₂
2HCl + Zn -> ZnCl₂ + H₂
Molar mass of Zn = 65 g/molMass of Zn from the balanced equation = 1 × 65 = 65 g Molar mass of ZnCl₂ = 135 g/molMass of ZnCl₂ from the balanced equation = 1 × 135 = 135 gFrom the balanced equation above,
65 g of Zn reacted to produce 135 g of ZnCl₂
Therefore,
130 g of Zn will react to produce = (130 × 135) / 65 = 270 g of ZnCl₂
Thus, the mass of ZnCl₂ obtained is 270 g
For H₂
2HCl + Zn -> ZnCl₂ + H₂
Molar mass of Zn = 65 g/molMass of Zn from the balanced equation = 1 × 65 = 65 g Molar mass of H₂ = 2 g/molMass of H₂ from the balanced equation = 1 × 2 = 2 gFrom the balanced equation above,
65 g of Zn reacted to produce 2 g of H₂
Therefore,
130 g of Zn will react to produce = (130 × 2) / 65 = 4 g of H₂
Thus, the mass of H₂ obtained is 4 g
Finally, we shall determine the total mass of the product produced. Details below:
Mass of ZnCl₂ = 270 gMass of H₂ = 4 gTotal mass of product =?Total mass of product = mass of ZnCl₂ + mass of H₂
Total mass of product = 270 + 4
Total mass of product = 274 g (3rd option)
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1. How many joules of heat is needed to heat 68.00 grams of aluminum foil from 55.00 °C to 93.00 °C if aluminum has a specific heat of 0.90 J/g °C?
2. Which of the following equations is an exothermic reaction?
Answer:
7. C. 2326 J
8. B
Explanation:
7. Use the equation q=m*c* change in temp, where m is mass, c is specific heat capacity.
q= 68 g* (0.9 J/g*c) * (93-55) C
q= 2326 J
8. An exothermic reaction is characterized by a negative delta H (change in enthalpy) since energy is released during the reaction. B is the only choice with a negative delta H.
Given Equation (Balance it) :
C2H4O2 + NaHCO3 —> NaC2H3O2 + H2O + CO2
Word Problem:
If you have 100 mg of Acetic Acid (C2H4O2) and 10 mg of NaHCO3 (Sodium Bicarbonate), how many grams of CO2 can be produced ?
also determine the theoretical yield of the chemical reaction.
C₂H₄O₂ + NaHCO₃ —> NaC₂H₃O₂ + H₂O + CO₂ the amount of Carbon dioxide produced is 5.28 mg.
Is the reaction between acetic acid and sodium bicarbonate exothermic or endothermic?Water, CO₂ , and C₂H₃NaO₂ were produced when acetic acid and NaHCO₃ were combined. The chemistry is as follows: The reaction between vinegar and baking soda was endothermic.
Acetic acid: 2(12.01 g/mol) + 4(1.01 g/mol) + 2(16.00 g/mol)
= 60.05 g/mol
NaHCO₃ 22.99 g/mol + 1.01 g/mol + 3(16.00 g/mol)
= 84.01 g/mol
100 mg of Acetic acid is equal to 0.1 g, and 10 mg of NaHCO₃ is equal to 0.01 g.
Number of moles of Acetic acid = 0.1 g / 60.05 g/mol
= 0.00167 mol
Number of moles of NaHCO₃ = 0.01 g / 84.01 g/mol
= 0.00012 mol
Since NaHCO₃ has fewer moles, it is the limiting reactant.
Therefore, 0.00012 mol of NaHCO₃ will produce 0.00012 mol of CO₂
The mass of CO₂ produced can be calculated as follows:
Mass of CO₂ = Number of moles of CO₂ x Molar mass of CO₂
Mass of CO₂ = 0.00012 mol x 44.01 g/mol
= 0.00528 g or 5.28 mg
Therefore, the amount of CO₂ produced is 5.28 mg.
The theoretical yield of CO₂ is 0.00012 mol x 44.01 g/mol
= 0.00528 g or 5.28 mg.
This is equal to the actual yield of CO₂ produced.
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The table below shows the vapor pressure of water at various temperatures.
Temp(degC) Vapor Pressure (mmHg)
17
14.5
18
15.5
19
16.5
20
17.5
21
18.7
22
19.8
During an experiment 675 mL of helium gas is collected over water at 22 degC. The air pressure in the lab is 0.926 atm. What is the partial pressure of the dry helium collected?
The partial pressure of the Helium gas is 0.9 atm.
What is the partial pressure of gas collected over water?The pressure that a gas exerts on its own when it is collected over water, independent of the pressure that the water vapor in the collecting vessel also produces, is known as its partial pressure.
When gas is collected over water, some of the water vapor will dissolve in it and change the overall pressure in the collecting vessel. Water vapor has its own partial pressure, which is affected by the relative humidity and temperature of the air around it. This is why it behaves in this way.
We have that;
Vapor pressure of the gas = 19.8 mmHg or 0.026 atm
Partial pressure of the Helium gas = 0.926 atm - 0.026 atm
= 0.9 atm
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The specific heat of gold is 0.129 J/g C. A king gets sold a gold crown but he's unsure if it's pure gold. He takes the crown which weighs 1,130 grams, heats it to 98.8 C, and then places it in 1.34 L of water with a starting point of 25.83 C. The final temperature of the water is 27.84 C. What is the specific heat of the crown and is it pure gold?
We can use the formula:
Q = mcΔT
where Q is the heat absorbed or released, m is the mass, c is the specific heat, and ΔT is the change in temperature.
First, let's calculate the heat absorbed by the crown:
Q1 = mcΔT
Q1 = (1130 g)(0.129 J/g C)(98.8 C - 25.83 C)
Q1 = 107,776.6 J
Next, let's calculate the heat released by the crown into the water:
Q2 = mcΔT
Q2 = (m)(c)(ΔT)
Q2 = (1340 g)(4.184 J/g C)(27.84 C - 25.83 C)
Q2 = 11096.64 J
Since Q1 = -Q2 (heat lost by the crown is equal to heat gained by the water),
mcΔT = -mcΔT
We can then solve for the specific heat of the crown:
c = -(Q2/mΔT)
c = -(11096.64 J)/(1130 g)(27.84 C - 25.83 C)
c = 0.131 J/g C
The specific heat of pure gold is 0.129 J/g C, and the specific heat of the crown is 0.131 J/g C. Since the specific heat of the crown is slightly higher than that of pure gold, it is possible that the crown is not pure gold. However, other factors such as impurities or alloying metals can also affect the specific heat, so further analysis would be necessary to confirm if the crown is pure gold.
Which
thermochemical
equation
corresponds to
the graph?
Answer: C
Explanation:
Answer: C
Explanation:
Does anyone have Personal Care services on E2020
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A client with a new ileostomy has been home for four days. The HHA is giving the client a bath and notices that the pouch is full. The HHA should say to the client: D. "I'll empty the pouch for you."A client is bedridden at home and has an infected draining sacral wound. The infection control supplies that should be kept in the home is: Gloves.What is infection?An infection is the entrance and growth of dangerous microorganisms in the body that harm the host, such as bacteria, viruses, fungus, or parasites.
Infections can be systemic (affecting the entire body) or localized (affecting a particular area of the body), and they can be moderate to severe.
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The hypochlorite ion, ClO-, is the active ingredient in bleach. The perchlorate ion, ClO4-, is a main component of rocket propellants. Draw Lewis structures for both ions.
(a) What is the formal charge of Cl in the hypochlorite ion?
(b) What is the formal charge of Cl in the perchlorate ion, assuming the ClㅡO bonds are all single bonds?
(c) What is the oxidation number of Cl in the hypochlorite ion?
(d) What is the oxidation number of Cl in the perchlorate ion, assuming the ClㅡO bonds are all single bonds?
(e) In a redox reaction, which ion would you expect to be more easily reduced?
(a) The formal charge of Cl in the hypochlorite ion (ClO-) is +1.
(b) The formal charge of Cl in the perchlorate ion (ClO4-) with single bonds is +3.
How to solveFor chlorine (Cl):
Valence electrons: 7
Non-bonding electrons: 6 (3 lone pairs)
Bonding electrons: 2 (1 single bond with oxygen)
Formal charge of Cl = 7 - 6 - (1/2 * 2) = 7 - 6 - 1 = +1
Hence, the formal charge of Cl in the hypochlorite ion is +1.
(c) The oxidation number of Cl in the hypochlorite ion is +1.
(d) The oxidation number of Cl in the perchlorate ion with single bonds is +7.
(e) In a redox reaction, the hypochlorite ion (ClO-) would be more easily reduced because it has a lower oxidation number (+1) compared to the perchlorate ion (+7).
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A 50.0-g sample of water at 25.0°C is mixed with 29.0 g of water at 65.0°C. The final temperature of the water is ________°C.
Answer:
39.7
Explanation:
Therefore, the final temperature of the water is 39.7°C.
How are models used in chemistry? How does evidence change these models?
Answer: As they develop theories, chemists use models to attempt to explain their findings. Chemists assess the model they are using as new evidence becomes available and, if required, continue to refine it by making modifications.
Explanation:
ichiometry in space
A typical space shuttle crew consists of six individuals and
each CCC contains 750 g of LIOH. Assuming that each crew
member expels 42.0 g of CO₂ per hour on average, and that
a mission is scheduled to last 18 days, how many CCCS must
be carried on board the space
shuttle?
- By knowing the recipe (balanced chemical equation), and
some molar masses, I can calculate this answer.
We need to carry at least 187 CCCs on board the space shuttle to absorb all the CO2 produced by the crew during the 18-day mission.
What is the amount of CO2 absorbed?To solve this problem, we need to use the following information:
Each crew member expels 42.0 g of CO2 per hour.The mission is scheduled to last 18 days.There are 6 crew members on board.Each CCC contains 750 g of LIOH.First, we need to calculate the total amount of CO2 that will be expelled during the mission:
Total CO2 = 6 crew members x 42.0 g CO2/hour x 24 hours/day x 18 days = 136,080 g CO2
Next, we need to calculate the amount of LIOH needed to absorb this CO2. The balanced chemical equation for the reaction between CO2 and LIOH is:
CO2 + 2 LIOH → Li2CO3 + H2O
The molar mass of CO2 is 44.01 g/mol, and the molar mass of LIOH is 23.95 g/mol.
This means that 2 moles of LIOH are needed to absorb 1 mole of CO2.
So, to absorb 136,080 g of CO2, we need:
136,080 g CO2 x (1 mol CO2/44.01 g) x (2 mol LIOH/1 mol CO2) x (23.95 g LIOH/1 mol) = 139,648 g LIOH
Since each CCC contains 750 g of LIOH, we need:
139,648 g LIOH / 750 g CCC = 186.2 CCCs
Therefore, we need to carry at least 187 CCCs on board the space shuttle to absorb all the CO2 produced by the crew during the 18-day mission.
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Balance:
2. K₂O + H₂O → KOH
3.F₂ +NaBr-NaF + Br₂
4.Ba(CIO3) → BaCl2 + O2
*
5.SrBr₂ + (NH4)2CO3 → SrCO3 + NH4Br
6. C8H18 + O₂ → CO₂ + H₂O
What is the reactions to these?
the balanced equation and there reactions are as follow:
K₂O + H₂O → 2KOH
The reaction between potassium oxide and water produces potassium hydroxide (KOH).
F₂ + 2NaBr → 2NaF + Br₂
The reaction between fluorine gas and sodium bromide produces sodium fluoride and bromine.
2Ba(CIO3)₂ → 2BaCl₂ + 3O₂
The decomposition of barium chlorate produces barium chloride and oxygen gas.
SrBr₂ + (NH₄)₂CO₃ → SrCO₃ + 2NH₄Br
The reaction between strontium bromide and ammonium carbonate produces strontium carbonate and ammonium bromide.
C₈H₁₈ + 12O₂ → 8CO₂ + 9H₂O
The combustion of octane with oxygen produces carbon dioxide and water.
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