Consider the reaction CO(g)+ 2 H₂(g)→ CH₃OH(g).If 15.0 L of hydrogen,measured at 22°C and 732 torr,reacts with excess carbon monoxide,what volume of methanol,measured at 345°C at 1.12 × 10³ torr,will be produced?

Question

Quizplus · Accepted Answer

First, we need to find the moles of hydrogen gas:

PV = nRT

(732 torr)(15.0 L) = n(0.0821 L·atm/K·mol)(295 K)

n = 0.905 mol H2

According to the balanced chemical equation, 1 mole of CO reacts with 2 moles of H2 to produce 1 mole of methanol. Therefore, we need to find the moles of methanol produced:

n(CH3OH) = (0.905 mol H2) / 2 = 0.4525 mol CH3OH

Now we can use the ideal gas law to find the volume of methanol produced:

PV = nRT

(V)(1.12 × 10^-13 torr) = (0.4525 mol)(0.0821 L·atm/K·mol)(618 K)

V = 10.3 L

Therefore, the volume of methanol produced is 10.3 L. The correct answer choice is C.

Consider the Reaction CO(g)+ 2 H2(g)→ CH3OH(g)

Consider the Reaction CO(g)+ 2 H₂(g)→ CH₃OH(g)