A 2.50L sample of nitrogen gas at a temperature of 308K has a pressure of 1.15atm. What is the new volume of the gas if the pressure is increased to 1.80atm and the temperature is decreased to 286K?

1.48L

Explanation:

From the question given, we obtained the following data:

V1 (initial volume) = 2.50L

T1 (initial temperature) = 308K

P1 (initial pressure) = 1.15atm

P2 (final pressure) = 1.80atm

T2 (final temperature) = 286K

V2 (final volume) =..?

Using the general gas equation P1V1/T1 = P2V2/T2, the final volume of the gas can obtain as follow:

P1V1/T1 = P2V2/T2

1.15 x 2.5/308 = 1.8 x V2/286

Cross multiply to express in linear form:

308 x 1.8 x V2 = 1.15 x 2.5 x 286

Divide both side by 308 x 1.8

V2 = (1.15 x 2.5 x 286)/(308 x 1.8)

V2 = 1.48L

Therefore, the new volume of the gas is 1.48L

your answer is a. the enthalpy of formation for a pure element in its standard state is always positive.