2. If 360g of CO2 gas was produced during the reaction of ethyne gas. Cal i.Write the balanced chemical equation ii.What is the mass of ethyne was used during the reaction iii.Mass of CO2 when 120g of ethyne reacts with excess oxygen iv. Actual yield v. Theoretical yield vi. Percentage yield

Question

2. If 360g of CO2 gas was produced during the reaction of ethyne gas. Cal i.Write the balanced chemical equation ii.What is the mass of ethyne was used during the reaction iii.Mass of CO2 when 120g of ethyne reacts with excess oxygen iv. Actual yield v. Theoretical yield vi. Percentage yield

Asked on April 10, 2026Chemistry

This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.

Accepted Answer · 2026-04-10T10:31:43.624Z

Here are the calculations for the reaction of ethyne gas: i. Write the balanced chemical equation The combustion of ethyne ($\text{C}_2\text{H}_2$) with oxygen ($\text{O}_2$) produces carbon dioxide ($\text{CO}_2$) and water ($\text{H}_2\text{O}$). $$2\text{C}_2\text{H}_2(g) + 5\text{O}_2(g) \longrightarrow 4\text{CO}_2(g) + 2\text{H}_2\text{O}(l)$$ ii. What is the mass of ethyne was used during the reaction This refers to the reaction that produced

2. If 360g of CO2 gas was produced during the reaction of ethyne gas. Cal i.Write the balanced chemical equation ii.What is the mass of ethyne was used during the reaction iii.Mass of CO2 when 120g of ethyne reacts with excess oxygen iv. Actual yield v. Theoretical yield vi. Percentage yield

2. If 360g of CO2 gas was produced during the reaction of ethyne gas. Cal i.Write the balanced chemical equation ii.What is the mass of ethyne was used during the reaction iii.Mass of CO2 when 120g of ethyne reacts with excess oxygen iv. Actual yield v. Theoretical yield vi. Percentage yield

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