Answered

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 ?

Verified Answer :

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 Latm/molK)(298.15K) = 3.7 L

The total volume of the reaction Ag(s). 2Ag2O(s)→4Ag(s)+O2(

g. will be 3.7L.

What is volume?

Each three-dimensional solid's volume consists only the sufficient space it takes up.

Given data:

Mass = 15.9g  

n= 0.147 mole

Temperature =25 ∘C

Pressure = 757mmHg = 0.965 atm

Volume = ?

Volume can be determined by the formula:

PV =nRT

where, P is pressure, V is volume, R is gas constant and T is temperature.

Put the value of given data in volume equation.

(0.965 atm) × V = (0.147 mole) ( 0.8206 Latm/molK)(298.15 K)

V = 3.7 L

Therefore, the volume will be 3.7 L.

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