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Dafna1 [17]
3 years ago
13

Please help !!

Chemistry
1 answer:
ipn [44]3 years ago
5 0

<u>Answer:</u>

<u>For 2:</u> The % yield of the product is 92.34 %

<u>For 3:</u> 12.208 L of carbon dioxide will be formed.

<u>Explanation:</u>

  • <u>For 2:</u>

The percent yield of a reaction is calculated by using an equation:

\% \text{yield}=\frac{\text{Actual value}}{\text{Theoretical value}}\times 100              ......(1)

Given values:

Actual value of the product = 78.4 g

Theoretical value of the product = 84.9 g

Plugging values in equation 1:

\% \text{yield}=\frac{78.4 g}{84.9g}\times 100\\\\\% \text{yield}=92.34\%

Hence, the % yield of the product is 92.34 %

  • <u>For 3:</u>

The number of moles is defined as the ratio of the mass of a substance to its molar mass.

The equation used is:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}} ......(2)

Given mass of carbon dioxide = 24 g

Molar mass of carbon dioxide = 44 g/mol

Plugging values in equation 1:

\text{Moles of carbon dioxide}=\frac{24g}{44g/mol}=0.545 mol

<u>At STP conditions:</u>

1 mole of a gas occupies 22.4 L of volume

So, 0.545 moles of carbon dioxide will occupy = \frac{22.4L}{1mol}\times 0.545mol=12.208L of volume

Hence, 12.208 L of carbon dioxide will be formed.

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