Question

In the acetylene torch, acetylene gas (C2H2) burns in oxygen to produce carbon dioxide water and energy. How many moles of CO2 are formed from the reaction with 1.20 moles of C2H2?

Given the following equation
2C2H2(g) + 502(g) = 4CO2(g) + 2H2O(g)

Answer 1

Answer: 2.40 moles of $CO_2$ will be formed in the reaction.

Explanation:

Given values:

Moles of $C_2H_2$ = 1.20 moles

The given chemical equation follows:

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

By the stoichioemetry of the reaction:

If 2 moles of $C_2H_2$ produces 4 moles of carbon dioxide

Then, 1.20 moles of $C_2H_2$ wil produce = $\frac{4}{2}\times 1.20=2.40mol$ of carbon dioxide

Hence, 2.40 moles of $CO_2$ will be formed in the reaction.