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The heat capacity is the quantity of heat required to raise the temperature of 1 mole of a monoatomic gas to 1.0K.

The amount of heat absorbed and the temperature increased is related by $Q=n{C}_v鈭�T$

where Q is the heat intake, $n$is the number of moles, $C_v$is the heat capacity at constant volume, $鈭�T$is the change in temperature.

Expression for change in temperature from the above equation is $鈭�T=\frac{Q}{n{C}_v}$.

Even if the value of heat capacity, is constant, still change in temperature depends on the heat intake, and the number of moles as well.

For different gases, the number of moles contained in 1g will be different. Thus, the amount of heat required will be more for more number of moles (as $Q鈭�n$), and the corresponding rise in temperature will be less, as $鈭�T鈭�\frac{1}{n}$.

Hence, it takes different amount of heat to raise the temperature of 1.0g of each sample of monoatomic gas by1.0K .