Question

What amount of heat must be supplied to 2.0 x 10⁻² kg of nitrogen (at room temperature) to raise its temperature by 45 oc at constant pressure? (Molecular mass of N₂ = 28; R = 8.3 J mol⁻¹ K⁻¹)

Answer 1

heya...

Here is your answer..

Mass of nitrogen, m = 2.0 × 10–2 kg = 20 g
Rise in temperature, ΔT = 45°C
Molecular mass of N2, M = 28
Universal gas constant, R = 8.3 J mol–1 K–1
Number of moles, n = m/M
= (2 × 10-2 × 103) / 28
= 0.714
Molar specific heat at constant pressure for nitrogen, Cp = (7/2)R
= (7/2) × 8.3
= 29.05 J mol-1 K-1
The total amount of heat to be supplied is given by the relation:
ΔQ = nCP ΔT
= 0.714 × 29.05 × 45
= 933.38 J
Therefore, the amount of heat to be supplied is 933.38 J.

It may help you...☺☺

Answer 2

Hey mate ^_^

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Answer:
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Increase in temperature = 45°C 

Mass of nitrogen = 2 × 10^-2 Kg

Molecular mass of N2 = 28 × 10^-3 Kg

R = 8.3 J/mol.K

Number of moles

=> m/M
=> 2 × 10^-2/28 × 10^-3
=> 5/7

Molar specific heat at constant pressure = 7R/2

Heat supplied = nCp∆T

=> 5/7 × 7/2 × 45 × 8.3
=> 933.75 J

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Final answer: 933.75 J
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