Consider the following reaction:
2K 2 CO 3(s) + 3O 2(g) $\rarr$ 4KO 2(s) + 2CO 2(g)
How many moles of K 2 CO 3 are needed to react with 35.0 L of oxygen at STP?
A) 22.4
B) 0.52
C) 1.04
D) 2.34
E) 33.6

Question

Consider the following reaction:
2K 2 CO 3(s) + 3O 2(g) $\rarr$ 4KO 2(s) + 2CO 2(g) 
How many moles of K 2 CO 3 are needed to react with 35.0 L of oxygen at STP?
A) 22.4
B) 0.52
C) 1.04
D) 2.34
E) 33.6

Quizplus · Accepted Answer

At STP, 1 mole of gas occupies 22.4 L. Therefore, 35.0 L of O2 is 35.0/22.4 = 1.5625 moles. According to the balanced equation, 2 moles of KCO3 react with 3 moles of O2. Thus, 1.5625 moles of O2 would require (2/3) * 1.5625 = 1.0417 moles of KCO3, which rounds to 1.04 moles.

Consider the Following Reaction: 2K2CO3(s) + 3O2(g) →\rarr→ 4KO2(s) + 2CO2(g) How Many Moles of K2CO3 Are Needed

Consider the Following Reaction:
2K₂CO_3(s) + 3O_2(g) $\rarr$ 4KO_2(s) + 2CO_2(g)
How Many Moles of K₂CO₃ Are Needed