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3 years ago

PLEASE HELP ASAP!

Chemistry

1 answer:

hoa [83]3 years ago

3 0

Answer:

A. 145.2 g NH3

B. 0.76 g H2

C. 1.41 x 10^22 molecules NH3

Explanation:

A. 1 mol N2 -> 2 mol NH3

4.27 mol N2 -> x

x= (4.27 mol N2 * 2 mol NH3)/1 mol N2 x= 8.54 mol NH3

1 mol N2 -> 17 g

8.54 mol N2 -> x x= 145.2 g NH3

2 g H2 -> 34 g NH3

x -> 13.01 g NH3

x= 0.76 g H2

2 g H2 -> 34 g NH3

0.0235 g H2 -> x

x= 0.39 g NH3

0.39 g NH3 (1 mol NH3/17 g NH3)(6.023 x 10^23 molecules/1 mol NH3) =

1.41 x 10^22 molecules NH3

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90.7 %

Explanation:

1) Chemical equation (given)

2NaHCO₃ → Na₂CO₃ + H₂CO₃

2) Theoretical yield

a) Convert mass of NaHCO₃ to moles:

n = mass in grams / molar mass
molar mass = 84.007 g/mol
n = 2.36 g / 84.007 g/mol = 0.02809 mol

b) Mole ratio:

2 mol NaHCO₃ : 1 mol H₂CO₃

c) Proportionality:

2 mol NaHCO₃ / mol H₂CO₃ = 0.02809 mol NaHCO₃ / x

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3) Actual yield

a) Mass balance: 2.36 g - 1.57 g = 0.79 g

b) Convert 0.79 g of carbonic acid to number of moles:

n = mass in grams / molar mass

molar mass = 62.03 g/mol

n = 0.79 g / 62.03 g/mol = 0.01274 mol

4) Percentage yield, y (%)

y (%) = actual yield / theoretical yield × 100

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Answer:

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Given the following data:

$V = 5 L$

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$n_{H_2} = 4 mol$

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According to the ideal gas law, we know that the product between pressure and volume of a gas is equal to the product between moles, the ideal gas law constant and the absolute temperature:

$pV = nRT$

Since the temperature and the ideal gas constant are constants, as well as the fixed container volume of 5 L, we may rearrange the equation as:

$\frac{p}{n}=\frac{RT}{V}=const$

This means for two conditions, we'd obtain:

$\frac{p_1}{n_1}=\frac{p_2}{n_2}$

Given:

$p_1 = 9 atm$

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Solve for the final pressure:

$p_2 = p_1\cdot \frac{n_2}{n_1}$

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