Derive the relationship `C_(P) - C_(v) = R`.

(a) Derive a relationship between K_(p) " and " K_(c) (b) What is a buffer solution? (C) Define acid according to Lewis concept. (d) Calculate pH value of 0.01 m HCI.

C_(P) - C_(V) = R . This R is

The ratio C_(p) // C_(v) for H_(2) is

The value of C_(P) - C_(v) = 1.00 R for a gas in state A and C_(P) - C_(v) = 1.06 R in another state. If P_(A) and P_(B) denote the pressure and T_(A) and T_(B) denote the temperature in the two states, then

If P((A)/(C))>P((B)/(C)) and P((A)/(bar(C)))>P((B)/(bar(C))), then the relationship between P(A) and P(B) is (A)P(A)=P(B) (B) P(A) P(B)(D)P(A)>=P(B)

The relationship between P_(C), V_(C) and T_(C) is

In Mayer's relation: C_(P)-C_(V)=R 'R' stands for:

In a real gas the internal energy depends on temperature and also on volume. The energy increases when the gas expands isothermally. Looking into the derivation of (C_p - C_v = R_1) find whether (C_p - C_v) will be more than R, less than R, or equal to R for a real gas.