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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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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Gas Stoichiometry concept. If you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.