The pressure exerted on a 240.0mL sample of hydrogen gas at constant temperature is increased from 4.28atm to 7.24atm. What will the final volume of the sample be?

141.88ml

Explanation:

From Boyles law, the pressure of a gas is inversely proportional to the volume at constant temperature, which can be expressed below

P1V1=P2V2

P1= initial pressure= 4.28atm

P2= final pressure=7.24atm

V1= initial volume= 240.0mL

V2= final volume=?

Making V2 subject of the formula we have, V2= (P1V1)/P2 then substitute those values we have

V2= (4.28atm× 240.0mL)/7.24atm

V2= 1027.2/7.24

V2=141.87mL

Therefore,the final volume of the sample is 141.87mL

explanation:

detials on each model with digrams

"standard molar enthalpy:

h2o ( liquid water ) : - 285.8 kj/mole

h2o ( water vapor ) : - 241.8 kj / mole.

δhrxn = - 241. 8 - ( - 285.8 )= -241.8 + 285.8 = 44.0

answer: 44.0 kj"