Cv and Cp denote the molar specific heat capacities of a gas at constant volume and constant pressure, respectively. Then

Question

Cv and Cp denote the molar specific heat capacities of a gas at constant volume and constant pressure, respectively. Then (A) Cp-Cv is larger for a diatomic ideal gas than for a monoatomic ideal gas (B) Cp+Cv is larger for a diatomic ideal gas than for a monoatomic ideal gas (C) (Cp/Cv) is larger for a diatomic ideal gas than for a monoatomic ideal gas (D) Cp.Cv is smaller for a diatomic ideal gas than for a monoatomic ideal gas

Tardigrade Admin · Accepted Answer

For monoatomic gas, CP=(5/2)R And CV=(3/2)R For diatomic gas, CP=(7/2)R and CV=(5/2)R

Q. $C_{v}$ and $C_{p}$ denote the molar specific heat capacities of a gas at constant volume and constant pressure, respectively. Then

$C_{p} - C_{v}$ is larger for a diatomic ideal gas than for a monoatomic ideal gas

$C_{p} + C_{v}$ is larger for a diatomic ideal gas than for a monoatomic ideal gas

$\frac{C _{p}}{C _{v}}$ is larger for a diatomic ideal gas than for a monoatomic ideal gas

$C_{p} . C_{v}$ is smaller for a diatomic ideal gas than for a monoatomic ideal gas

For monoatomic gas,
$C_{P} = \frac{5}{2} R$
And $C_{V} = \frac{3}{2} R$
For diatomic gas,
$C_{P} = \frac{7}{2} R$
and $C_{V} = \frac{5}{2} R$

Q. Cv​ and Cp​ denote the molar specific heat capacities of a gas at constant volume and constant pressure, respectively. Then

Cp​−Cv​ is larger for a diatomic ideal gas than for a monoatomic ideal gas

Cp​+Cv​ is larger for a diatomic ideal gas than for a monoatomic ideal gas

Cv​Cp​​ is larger for a diatomic ideal gas than for a monoatomic ideal gas

Cp​.Cv​ is smaller for a diatomic ideal gas than for a monoatomic ideal gas