A bag of potato chips contains 585 mL of air at 25°C with a pressure of 765 mm HG. What will be its volume at the top of the mountain where the pressure is 442 MM Hg and the temperature is 5.0°C

944.55mL

Explanation:

Data obtained from the question include:

V1 (initial volume) = 585 mL

T1 (initial temperature) = 25°C = 25 + 273 = 298K

P1 (initial pressure) = 765 mmHg

V2 (final volume) =?

P2 (final pressure) = 442 mmHg

T2 (final temperature) = 5°C = 5 + 273 = 278K

Applying the general gas equation P1V1/T1 = P2V2/T2, the final volume at the top of the mountain can be obtained as follow:

P1V1/T1 = P2V2/T2

765 x 585/298 = 442 x V2/278

Cross multiply to express in linear form as shown below:

298 x 442 x V2 = 765 x 585 x 278

Divide both side by 298 x 442

V2 = (765 x 585 x 278)/(298 x 442)

V2 = 944.55mL

Therefore, the volume at the top of the mountain will be 944.55mL

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