One mole of an ideal gas (Cv 2.5R) is reversibly changed from 400K, 5 atm to 600K, 2 atm. Calculate the change in enthalpy, entropy and Gibbs free energy if molar entropy at 400K is 5 J/(K.mol).
Answers
Answered by
4
ΔS=2.303 n Rlog(V1V2)
=2.303×10×8.314log(10100)=191.47 JK−1
Thus ΔS=191.47JK−1
Answered by
1
Answer:
(25/8)÷____=-10
25/8 ÷ (-5 /16) = -10
sᴏʟᴠɪɴɢ ʟʜs :-
25 /8 × - 16 /5
-(5 × 2)
= - 10
ʜᴇɴᴄᴇ, ᴛʜᴇ ᴀɴsᴡᴇʀ ɪs -5/16
Similar questions
Social Sciences,
19 days ago
Math,
1 month ago
Environmental Sciences,
1 month ago
Physics,
9 months ago
Geography,
9 months ago