What amount of heat must be supplied to `2xx10^(-2)Kg` of nitrogen at room temperature to rise its temperature by `45^(@)C` at constant pressure? Given molecular mass of nitrogen is 28 and `R=8.3J mol e^(-1)K^(-1)`

Explanation

Here, mass of gas,
` m = 2 xx 10^(-2) kg = 20 g `, rise in temp.,
`Delta T = 45^(@)C`, Heat required ,`Delta Q = ?`
Moleculer mass, `M=28`
Number of moles, `n=m/M = 20/28 = 0.714`
As, nitrogen is a diamic gas, molar specific heat at consant pressure is
`C_(p) = 7/2 R = 7/2 xx 8.3 J mol e^(-1) K^(-1)`
As, `Delta Q = n C_(p) Delta T`
`:. Delta Q = 0.714 xx 7/2 xx 8.3 xx 45 J =933.4 J`.