Ask a New Question

We have 1 mol of N2 gas that is heated at constant pressure from 300K to 5770K on the surface of the sun.

i) Find H and S given that P for nitrogen is (25.7 + 0.0130T) J/mol-K.
ii) Now, redo your calculation assuming that the second T-dependent term in the P expression is negligible (i.e. P does not depend on T)
iii) What is the percent error if we assume that P is not temperature dependent?

Ask a New Question or answer this question.

Similar Questions

At constant volume, a container of gas at 1 atm is heated from 300K to 350K. What is the final pressure?a 0.35 atm b 0.86 atm c
1. 1 answer
a gas at 10atm pressure occupy a volume of 10L at 300k it is allowed to expand at the constant temperature of 300k under
1. 2 answers
one mole of ideal gas is slowly heated at a constant pressure of 2.0 atm from 200 to 300k.Calculateq,w,£GE,and£GH,allinjoules.
1. 0 answers
The Equilibrium Constant Kp for the following reaction is 4atm^2 at 300K.AB(s) -> A(g) + B(g) What is the equilibrium pressure
1. 1 answer

more similar questions