Problem: In the reaction shown here, 4.55 L of O2 was formed at P = 746 mmHg and T = 308 K .2Ag2O(s) → 4Ag(s)+O2(g)How many grams of Ag2O decomposed?

FREE Expert Solution

Calculate moles O2 produced using the ideal gas equation:

PV=nRT

P=746 mmHg×1 atm760 mmHg

P = 0.9815 atm
V = 4.55 L
T = 308 K

PVRT=nRTRTn=PVRTn=(0.9815 atm)(4.55 L)(0.08206L·atmmol·K)(308 K)

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Problem Details

In the reaction shown here, 4.55 L of O2 was formed at P = 746 mmHg and T = 308 K .

2Ag2O(s) → 4Ag(s)+O2(g)

How many grams of Ag2O decomposed?

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