The molar constant-pressure heat capacity of a certain solid at 4.2K is `0.3J/(molK)` If the molar entropy at that temperature is `zj/(molK)` what is the value of10Z(Hint- when the temperature is so low, we can assume that the heat capacity varies with temperature as a `T^(3)` where a is a constant and T is absolute scale of temperature)

Find the relatio between volume and temperature of a gas in a process, in which the molar heat capacity C varies with temperature T as C=C_(V)+alphaT . [ alpha is a constant] .

When a certain amount of heat is supplied to a diatomic gas at constant volume, rise in temperature is T_(0) . When same heat is supplied to the gas at constant pressure, find the rise in temperature

For an ideal gas the molar heat capacity varies as C=C_V+3aT^2 . Find the equation of the process in the variables (T,V) where a is a constant.

The pressure P of an ideal diatomic gas varies with its absolute temperature T as shown in figure . The molar heat capacity of gas during this process is [R is gas constant]

The molar heat capacity of a certain substance varies with temperature according to the given equation C=27.2+(4xx10^-3)T The heat necessary to change the temperature of 2 mol of the substance from 300 K to 700 K is

The molar heat capacity of a certain substance varies with temperature "T" as c = a + bT where a = 27.2 J mol-1 K-2. Then the heat necessary to change the temperature of 2 moles of this substance from 27°C to 427°C is

The molar heat capacity at constant pressure of nitrogen gas at STP is nearly 3.5 R . Now when the temperature is increased, it gradually increases and approaches 4.5 R . The most approprite reason for this behaviour is that at high temperatures

The molar heat capacity of water at constant pressure, C, is 75 JK^(-1) mol^(-1) . When 1.0 kJ of heat is supplied to 100 g water which is free to expand, the increase in temperature of water is :

An ideal gas expands from 100 cm^(3) to 200 cm^(3) at a constant pressure of 2.0 xx 10^(5) when 50 J of heat is supplied to it. Calculate (a) the change in internal energy of the gas , (b) the number of moles in the gas if the initial temperature is 300K , (C ) the molar heat capacity C_P at constant pressure and (d) the molar heat capacity C_v at constant volume

One mole of an ideal monoatomic gas requires 207 J heat to raise the temperature by 10 K when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by the same 10 K, the heat required is [Given the gas constant R = 8.3 J/ mol. K]