Question

what amount of heat must be supplied to 2.0 into 10 power minus 2 kg of Nitrogen to rise its temperature by 25 degree Celsius at constant pressure ​

Answer 1

given mass of Nitrogen= 2.0×10^-2 kg

increasing temperature = 45°C

molecular mass of N2 = 28g = 28×10^-3 kg

number of moles = m/M = 2×10^-2/28×10^-3 = 5/7

molar specific heat at constant pressure = 7/2R

heat supplied = 933.75 J

Answer 2

Answer:

Here,

Mass of nitrogen ( m) = 2 × 10^-2 Kg

Increase in temperature (∆T) = 45°C

molecular mass of N2 (M) = 28 g

= 28 × 10^-3 Kg

R = 8.3 J/mol.K

Number of moles (n) = m/M = 2 × 10^-2/28 × 10^-3 = 5/7

molar specific heat at constant pressure ( Cp) = YR/(Y-1) where Y is atomicity of gases . Y = 1.4

Cp = 1.4R/(1.4-1) = 7R/2

So, heat supplied = nCp∆T

= 5/7 × 7/2 × 45 × 8.3

= 933.75 J