What amount of heat must be supplied to `2.0 × 10^(–2) kg` of nitrogen (at room temperature) to raise its temperature by `45 °C` at constant pressure ? (Molecular mass of `N_(2) = 28, R = 8.3 J mol^(–1) K^(–1)`.)

What amount of heat must be supplied to 2.0 xx 10^(-2) kg of nitrogen (at room temperature) to raise its temperature by 45^(@)C at constant pressure? (Molecular mass of N_(2) = 28, R = 8.3 J cdot mol^(-1) cdot K^(-1))

What amount of heat is to be supplied to 14 g of nitrogen in order to increase the temperature by 40^(@)C at constant pressure? Molecular weight of nitrogen =28 and R = 8.3 J cdot mol^(-1) cdot K^(-1) .

Amount of heat required to raise the temperature of 1 kg of water by 1^@C is

Calculate heat of combustion of benzene at constant pressure at 27^@C . (R=8.3 J mol^-1 K^-1)

What is the entropy change in 2 mol N_(2) , when its temperature is taken from 400 K to 800 K, at constant pressure-

In which temperature 14 gm N_2 at 1.642 atm pressure occupies 10 lt? [R = 0.0821 L atm//mol^(-K) ]

At a temperature of 273K and 1 atm pressure 1L of a gas weighs 2.054g. Calculate its molecular mass.

For 0.5 mol of an ideal gas, 15 cal of heat is required to raise its temperature by 10K at constant volume. The molar heat capacity for the gas at constant pressure is-

The specific heat of oxygen gas at constant volume is 0.155 cal cdot g^(-1) cdot^(@)C^(-1) . What is its specific heat at constant pressure? Given, the molecular mass of oxygen = 32 and R = 2 cal cdot mol^(-1) cdot^(@)C^(-1) .

70 cal of heat is required to increase the temperature of 2 mol of an ideal diatomic gas at constant pressure from 40^(@)C to 45^(@)C . How much heat will be required to increase the temperature of that gas by the same amount at constant volume? R = 2 cal cdot mol^(-1) cdot K^(-1) .