the special proteins prevent

a or b

Answer:

a. welding torch fuel

Answer:

welding torch fuel

Explanation:

Answer:

D. delta H is positive, and delta S is positive

Answer:

1.2046x10²⁴ atoms

Explanation:

First we convert 60 grams of acetic acid into moles of acetic acid, using its molar mass:

Then we double the number of acetic acid moles, as there are two oxygen moles per acetic acid mole.

Finally we convert moles into number of atoms, using Avogadro's number:

Answer: The empirical formula and the molecular formula of the hydrocarbon is [tex]C_2H_3[/tex] and [tex]C_4H_6[/tex] respectivley.

Explanation:

The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:

[tex]C_xH_y+O_2\rightarrow CO_2+H_2O[/tex]

where, 'x', 'y'  are the subscripts of Carbon, hydrogen

We are given:

Mass of [tex]CO_2[/tex] = 12.74 g

Mass of [tex]H_2O[/tex]= 3.913 g

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44g of carbon dioxide, 12 g of carbon is contained.

So, in 12.74 g of carbon dioxide, =[tex]\frac{12}{44}\times 12.74=3.474g[/tex] of carbon will be contained.

For calculating the mass of hydrogen:

In 18g of water, 2 g of hydrogen is contained.

So, in 3.913 g of water, =[tex]\frac{2}{18}\times 3.913=0.435g[/tex] of hydrogen will be contained.  

Mass of C = 3.474 g

Mass of H = 0.435 g

Step 1 : convert given masses into moles.

Moles of C =[tex] \frac{\text{ given mass of C}}{\text{ molar mass of C}}= \frac{3.474g}{12g/mole}=0.289moles[/tex]

Moles of H=[tex]\frac{\text{ given mass of H}}{\text{ molar mass of H}}= \frac{0.435g}{1g/mole}=0.435moles[/tex]

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For C =[tex]\frac{0.289}{0.289}=1[/tex]

For H =[tex]\frac{0.435}{0.289}=1.5[/tex]

The ratio of C : H = 1: 1.5

The whole number ratio will be = 2: 3

Hence the empirical formula is [tex]C_2H_3[/tex].

The empirical weight of [tex]C_2H_3[/tex] = 2(12.01)+3(1.008)= 27.04 g.

The molecular weight = 54.09 g/mole

Now we have to calculate the molecular formula.

[tex]n=\frac{\text{Molecular weight }}{\text{Equivalent weight}}=\frac{54.09}{27.04}=2[/tex]

The molecular formula will be=[tex]2\times C_2H_3=C_4H_6[/tex]

Answer:

O4Br9

Explanation:

Tetra means 4 and nona means 9. Just use these prefixes to decide how many of each element you have.

Answer:

they cause animals home's to be destroyed

Explanation:

Answer:6.68

Explanation:

Answer:

The IUPAC name of the given compound is - Methyl - 4 - methylpentanoate

Explanation:

IUPAC name of the compound helps to determine the correct structure of the compound which can be used universally in order to avoid any confusion or misinterpretation.

[tex]CH_3CH_2COO(C_6H_5)[/tex]

The IUPAC name of the given compound is - phenyl propanoate.

[tex]CH_3OCOCH_2CH_2CH(CH_3)_2[/tex]

The IUPAC name of the given compound is - Methyl - 4 - methylpentanoate.

Answer:

1) Cl2   2 is missing

2) H     H is missing

Explanation:

Answer:

3-methyl-2-butanone.

Explanation:

Hello there!

In this case, for these types of oxidation of secondary alcohols, due to the 2-butanol, it is possible for us to remember that the product is a ketone exhibiting a carbonyl (C=O) group as the product of the oxidation. In such a way, the reaction would be:

CH3 - CH - CH - CH3      ------->       CH3 - C - CH - CH3

           |        |                                                ||     |  

          OH   CH3                                          O  CH3

Therefore, the product would be 3-methyl-2-butanone.

Best regards!

Answer:

False

Explanation:

Some substances don't have to be

Answer:

Because You never know when a meteor will hit you.

Answer:

A weak acid is one that does not dissociate completely in solution; this means that a weak acid does not donate all of its hydrogen ions (H+) in a solution. ... Therefore, the concentration of H+ ions in a weak acid solution is always less than the concentration of the undissociated species, HA.

Explanation:

Hope it helps

FOLLOW MY ACCOUNT PLS PLS

Answer:

An apple.

Explanation:

Hope this helps.

Answer:

2.03 x 10⁻² mol NaOH

Explanation:

First step for these questions is to ensure the reaction is balanced, then use the periodic table to determine the molar mass for the reactant you are given. Use the ratio from the balanced equation and dimensional analysis to solve. See attached image

Answer:

71820 J

Explanation:

From the question given above, the following data were obtained:

Mass (M) = 1.05 Kg

Initial Temperature (T₁) = 23 °C

Final temperature (T₂) = 99 °C

Heat (Q) required =?

Next, we shall determine the change in temperature. This can be obtained as follow:

Initial Temperature (T₁) = 23 °C

Final temperature (T₂) = 99 °C

Change in temperature (ΔT) =?

ΔT = T₂ – T₁

ΔT = 99 – 23

ΔT = 76 °C

Finally, we shall determine the heat required. This can be obtained as follow:

Mass (M) = 1.05 Kg

Change in temperature (ΔT) = 76 °C

Specific heat capacity (C) of aluminum = 900 J/KgºC

Heat (Q) required =?

Q = MCΔT

Q = 1.05 × 900 × 76

Q = 71820 J

Thus, 71820 J heat energy is required.

Answer:

Yes it does

Explanation:

Answer:

B. CO₂ and H₂O.

Explanation:

When any organic substance undergoes complete combustion, it produces carbon dioxide (CO₂) and water (H₂O).

In the case of methane, the balanced reaction is:

With the above information in mind the correct answer is option B. CO₂ and H₂O.

When the combustion is incomplete, carbon monoxide (CO) is produced as well.

Answer:

B. CO₂ and H₂O!

Answer:

Explanation:

S2Si

O2

C2H4

N2

CBr4

S2

I think these are correct

Answer:

5.51g

Explanation:

Using the following formula:

Q = m × c × ∆T

Where;

Q = amount of heat in Joules

m = mass/weight of Aluminum

c = specific heat of Aluminum (0.900 J/g°C)

∆T = change in temperature.

Based on the information given in this question, Q = 175.6 joules, ∆T = 35.4°C, c = 0.900 J/g°C.

Using, Q = m × c × ∆T

175.6 = m × 0.900 × 35.4

175.6 = 31.86m

m = 175.6/31.86

m = 5.51g

The weight of the aluminum sample is 5.51g.

Answer:

[tex]3.0molMg(OH)_2[/tex]

Explanation:

Hello there!

In this case, for these types of acid-base neutralizations, it is crucial to firstly set up the chemical reaction taking place between the acid and the base; in this case HCl and Mg(OH)2 respectively, whose products are obtained by switching around the anions and cations as shown below:

[tex]HCl(aq)+Mg(OH)_2(aq)\rightarrow MgCl_2(aq)+H_2O(l)[/tex]

Which must be balanced to accurately predict the mole ratio on the reactants side:

[tex]2HCl(aq)+Mg(OH)_2(aq)\rightarrow MgCl_2(aq)+2H_2O(l)[/tex]

Whereas we can see a 2:1 mole ratio of the acid to the base; thus, the moles of Mg(OH) required for the neutralization of 6.0 moles of HCl turn out to be:

[tex]6.0molHCl*\frac{1molMg(OH)_2}{2molHCl} \\\\=3.0molMg(OH)_2[/tex]

Best regards!

Answer:

hope that helps

Answer:

Explanation:

Answer:  The empirical formula and the molecular formula of the organic compound is [tex]CHO[/tex] and [tex]C_4H_4O_4[/tex] respectively.

Explanation:

The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:

[tex]C_xH_yO_z+O_2\rightarrow CO_2+H_2O[/tex]

where, 'x', 'y' and 'z' are the subscripts of Carbon, hydrogen and oxygen respectively.

We are given:

Mass of [tex]CO_2[/tex] = 21.71 g

Mass of [tex]H_2O[/tex]= 5.926 g

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44g of carbon dioxide, 12 g of carbon is contained.

So, in 21.71 g of carbon dioxide, =[tex]\frac{12}{44}\times 21.71=5.921g[/tex] of carbon will be contained.

For calculating the mass of hydrogen:

In 18g of water, 2 g of hydrogen is contained.

So, in 5.926 g of water, =[tex]\frac{2}{18}\times 5.926=0.658g[/tex] of hydrogen will be contained.

Mass of oxygen in the compound = (17.11) - (5.921+0.658) = 10.53  g

Mass of C = 5.921 g

Mass of H = 0.658 g

Mass of O = 10.53 g

Step 1 : convert given masses into moles.

Moles of C =[tex] \frac{\text{ given mass of C}}{\text{ molar mass of C}}= \frac{5.921g}{12g/mole}=0.493moles[/tex]

Moles of H=[tex]\frac{\text{ given mass of H}}{\text{ molar mass of H}}= \frac{0.658g}{1g/mole}=0.658moles[/tex]

Mass of O=[tex]\frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{10.53g}{16g/mole}=0.658moles[/tex]

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For C =[tex]\frac{0.493}{0.493}=1[/tex]

For H =[tex]\frac{0.658}{0.493}=1[/tex]

For O=[tex]\frac{0.658}{0.493}=1[/tex]

The ratio of C : H: O =  1: 1: 1

Hence the empirical formula is [tex]CHO[/tex].

empirical mass of CHO = 12(1) + 1(1) + 1 (16) = 29

Molecular mass = 104.1 g/mol

[tex]n=\frac{\text {Molecular mass}}{\text {Equivalent mass}}=\frac{104.1}{29}=4[/tex]

Thus molecular formula = [tex]n\times {\text {Empirical formula}}=4\times CHO=C_4H_4O_4[/tex]

Answer:

there is no d electron that can be promoted via the absorption of visible light

Explanation:

One of the properties of transition elements is the possession of incompletely filled d orbitals. This property accounts for their unique colours.

The colours of transition metal compounds stem from d-d transition of electrons due to the presence of vacant d orbitals of appropriate energy to which electrons could be promoted.

For elements whose atoms have a d10 configuration, such vacant orbitals does not exist hence their compounds are not colored.

Sometimes, the colour of transition metal compounds stem from ligand to metal charge transfer(LMCT) for instance in KMnO4.