The amount of heat energy required to raise t | vedclass

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(D) For an ideal gas,the heat required to change the temperature at constant volume is given by $\Delta Q = \mu C_V \Delta T$.Helium is a monoatomic g

Vedclass · Accepted Answer

$\frac{3}{8} N_A k_B (T_2 - T_1)$

Vedclass · Answer

(D) For an ideal gas,the heat required to change the temperature at constant volume is given by $\Delta Q = \mu C_V \Delta T$.Helium is a monoatomic gas,so its degrees of freedom $f = 3$.The molar specific heat at constant volume is $C_V = \frac{fR}{2} = \frac{3R}{2}$.The number of moles $\mu = \frac{	ext{mass}}{	ext{molar mass}} = \frac{1 \ g}{4 \ g/mol} = \frac{1}{4} \ mol$.Substituting these values into the formula:$\Delta Q = \left( \frac{1}{4} ight) \left( \frac{3R}{2} ight) (T_2 - T_1) = \frac{3R}{8} (T_2 - T_1)$.Since the universal gas constant $R = N_A k_B$,we substitute $R$ to get:$\Delta Q = \frac{3}{8} N_A k_B (T_2 - T_1)$.

The amount of heat energy required to raise the temperature of $1 \ g$ of helium from $T_1 \ K$ to $T_2 \ K$ at $NTP$ is ........

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