The reaction forms 15.9g of Ag (s). 2Ag2O (s) →4Ag (s) + O2 (

g. What total volume of gas forms if it is collected over water at a temperature of 25 ∘C and a total pressure of 757mmHg?

You will use PV=nRT

First, water vapor pressure at 25°C is 23.8 mmHg. Subtract this from the total pressure to get 733.2 mmHg. Convert to atm to get 0.965 atm.

15.9g of Ag =.147 mole Ag

25°C + 273.15 = 298.15K

Plug in the values.

(.965atm) V = (.147mol) (.08206 L*atm/mol*K) (298.15K) = 3.7 L