Question

how many grams of carbon dioxide would be formed if 38.9 g of C2H2 reacted completely with oxygen

Answer 1

Answer:

131.7 grams of carbon dioxide would be formed

Explanation:

2C₂H₂ + 5O₂ = 4CO₂ + 2H₂O

m(CO₂)/{4M(CO₂)} = m(C₂H₂)/{2M(C₂H₂)}

m(CO₂)=2M(CO₂)m(C₂H₂)/M(C₂H₂)

m(CO₂)=2*44g/mol*38.9g/26g/mol = 131.7 g

131.7 grams of carbon dioxide would be formed

Answer 2

Answer: The mass of carbon dioxide produced in the given reaction is 132 grams.

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$      .....(1)

• For ethyne:

Given mass of ethyne = 38.9 g

Molar mass of ethyne = 26 g/mol

Putting values in equation 1, we get:

$\text{Moles of ethyne}=\frac{38.9g}{26g/mol}=1.5mol$

• The chemical reaction for the combustion of ethyne follows the equation:

$2C_2H_2+5O_2\rightarrow 4CO_2+2H_2O$

By Stoichiometry of the reaction:

2 moles of ethyne produces 4 moles of carbon dioxide.

So, 1.5 moles of ethyne will produce = $\frac{4}{2}\times 1.5=3mol$ of carbon dioxide.

• Now, calculating the mass of carbon dioxide from equation 1, we get:

Molar mass of carbon dioxide = 44 g/mol

Moles of carbon dioxide = 3 moles

Putting values in equation 1, we get:

$3mol=\frac{\text{Mass of carbon dioxide}}{44g/mol}\\\\\text{Mass of carbon dioxide}=132g$

Hence, the mass of carbon dioxide produced in the given reaction is 132 grams.