The heat capacity of a diatomic gas is higher than that of a monatomic gas.
Text Solution
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To determine whether the statement "The heat capacity of a diatomic gas is higher than that of a monatomic gas" is true or false, we can analyze the heat capacities of both types of gases based on their degrees of freedom.
### Step-by-Step Solution:
1. **Understanding Heat Capacity**:
- Heat capacity is the amount of heat required to raise the temperature of a substance by one degree Celsius (or one Kelvin). It is dependent on the number of degrees of freedom of the gas molecules.
2. **Degrees of Freedom**:
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Heat capacity of a diatomic gas is higher than that of a monoatomic gas.
Assertion : The ratio C_(P)// C_(upsilon) for a diatomic gas is more than that for a monoatomic gas. Reason : The moleculess of a monoatomic gas have more degrees of freedom than those of a diatomic gas.
The molar heat capacity for an ideal gas
The ratio of the molar heat capacities of a diatomic gas at constant pressure to that at constant volume is
The ratio of the specific heat at constant pressure to that at constant volume is larger for a diatomic gas than for a monoatomic gas.
One moles of a monatomic gas is mixed with three moles of a diatomic gas. The molar specific heat of the mixture at constant volume is
For a certain gas the heat capcity at constant pressure is greater than that at constant volume by 29.1 J//K . (a) How many moles of the gas are there ? (b) if the gas is monatomic, what are heat capacities at constant volume and pressure ? ( c) If the gas molecules are diatomic which rotate but do nit vibrate, what are heat capacities at constant volume and at constant pressure.
The molar heat capacity in a process of a diatomic gas if it does a work of Q/4 when a heat of Q is supplied to it is
For an ideal gas, the heat capacity at constant pressure is larger than than that at constant volume because
