Specific Heat Capacity of a Gas

The specific heat of a substance i.e at constant pressure is defined as the rate of change of _____ with respect to ______

Specific heat of a substance at constant volume is a property of the system.

Heat transferred at constant ________ increases the ______ of a system.

The specific heat of a substance at constant volume is defined as the rate of change of _______ with respect to ______

If ${\mathrm{S}}_{\mathrm{P}}$ and ${\mathrm{S}}_{\mathrm{V}}$ denote the specific heats of nitrogen gas per unit mass at constant pressure and constant volume respectively, then

One gram mole of an ideal gas $A$ with the ratio of constant pressure and constant volume specific heats ${\gamma }_A=\frac{5}{3}$ is mixed with $n$ gram moles of another ideal gas $B$ with ${\gamma }_B=\frac{7}{5}$. If the $\gamma$ for the mixture is $\frac{19}{13}$, then what will be the value of $n$?

A thermally insulated piece of metal is heated under atmosphere by an electric current so that it receives electric energy at a constant power P. This leads to an increase of the absolute temperature T of the metal with time t as follows

$\mathrm{T}=\mathrm{a}{\mathrm{t}}^{\frac{1}{4}}$

Then the heat capacity ${\mathrm{C}}_{\mathrm{p}}$ is

Heat required to raise the temperature of 1 mole of a substance by $1°$ is called

The value of molar specific heat at constant pressure for one mole of triatomic gas (triangular arrangement) at temperature $T \mathrm{K} \text{is} (R$ is the universal gas constant)

70 cal of heat is required to raise the temperature of 2 moles of an ideal gas from 30$℃$ to 35$℃$ while the pressure of the gas is kept constant. The amount of the heat required to raise the temperature of the same gas through the same temperature range at constant volume is (gas constant $R=2 \mathrm{c}\mathrm{a}\mathrm{l}\mathrm{ }\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}-{\mathrm{K}}^{-1})$

A vessel contains helium, which expands at constant pressure when$15 \mathrm{kJ}$of heat is supplied to it. What is the work performed in the expansion?

Four moles of hydrogen, 2 moles of helium and 1 mole of water vapour form an ideal gas mixture. What is the molar specific heat at constant pressure of mixture?

310 J of heat is required to raise the temperature of 2 moles of an ideal gas at constant pressure from $25℃$to$35℃.$ The amount of heat required to raise the temperature of the gas through the same range at constant volume is

$10$ mole of an ideal gas is heated at a constant pressure of one atmosphere from $27°\mathrm{C}$ to $127°\mathrm{C}$. If ${\mathrm{C}}_{\mathrm{v}, \mathrm{m}}=21.686+{10}^{-3} \mathrm{T}$, then what will be $\Delta \text{H}$ for the process?

For three gases (assume ideal); oxygen, nitrogen and carbon dioxide, (C_p - C_v) will be

The molar heat capacity of oxygen gas at STP is nearly 2.5R. As the temperature is increased, it gradually increases and approaches 3.5 R. The most appropriate reason for this behaviour is that at high temperature 

${\mathrm{\Delta C}}_{\mathrm{p}}$ for a reaction is $2.0+0.2 \mathrm{T} \mathrm{cal} {\mathrm{g}}^{-1}$. Its enthalpy of reaction at $10 \mathrm{K}$ is $-14.2 \mathrm{kcal} {\mathrm{mol}}^{-1}$. Its enthalpy of reaction at $100 \mathrm{K} \mathrm{in} \mathrm{kcal} {\mathrm{mol}}^{-1}$ will be

$70 \mathrm{cal}$ of heat is required to raise the temperature of  $2 \mathrm{moles}$ of an ideal diatomic gas at constant pressure from $30°\mathrm{C}$ to $35°\mathrm{C}$. The amount of heat required (in calorie) to raise the temperature of the same gas through the same range $(30°\mathrm{C} \mathrm{to} 35°\mathrm{C})$ at constant volume is

$25.0 \mathrm{mL}$ of $1.0 \mathrm{M} \mathrm{HCl}$ is combined with $35.0 \mathrm{mL}$ of $0.5 \mathrm{M} \mathrm{NaOH}$. The initial temperatures of the solutions is $25^{\circ }\text{C}$, the density of the solution is $1.0 \mathrm{g}/\mathrm{mL}$, the specific heat capacity of the solution is $4.184 \text{J}/{\text{g}}^{\circ }\text{C}$, the reaction is completed in an insulated coffee cup, and the standard enthalpy of reaction for ${\text{H}}^{+}\left(\text{aq}\right)+{\text{OH}}^{-}\left(\text{aq}\right)⟶{\text{H}}_{2}O \left(\mathrm{l}\right)$ is $-56 \mathrm{kJ}/\mathrm{mol}$. What is the final temperature of the solution?