Consider the following reaction:
4KO₂(s) + 2CO₂(g) $\rightarrow$ 2K₂CO₃(s) + 3O₂(g)
How many liters of oxygen are produced at STP if 10.5 moles of carbon dioxide are used at STP?

Question

Consider the following reaction:
4KO₂(s) + 2CO₂(g)

\rightarrow

2K₂CO₃(s) + 3O₂(g)
How many liters of oxygen are produced at STP if 10.5 moles of carbon dioxide are used at STP?

Quizplus · Accepted Answer

At STP, 1 mole of gas occupies 22.4 liters. The reaction shows that 2 moles of CO2 produce 3 moles of O2. Therefore, 10.5 moles of CO2 will produce (10.5 moles CO2 * 3/2) = 15.75 moles of O2. At STP, this is 15.75 moles * 22.4 L/mole = 353 liters of O2.

Consider the Following Reaction: 4KO2(s)+ 2CO2(g) →\rightarrow→ 2K2CO3(s)+ 3O2(g) How Many Liters of Oxygen Are Produced at Many

Consider the Following Reaction:
4KO₂(s)+ 2CO₂(g) $\rightarrow$ 2K₂CO₃(s)+ 3O₂(g)
How Many Liters of Oxygen Are Produced at Many