Question

What amount of heat must be supplied to 2×10^-2kg of room temperature to raise its temperature by 45°C at constant pressure ! Given molecular mass of N = 28 and R = 8.3 ​

Answer 1

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 N2 = 28; R = 8.3 J mol–1 K–1.) Therefore, the amount of heat to be supplied is 933.38 J.

Answer 2

Hey!
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Ques.→ What amount of heat must be supplied to 2×10^-2kg of room temperature to raise its temperature by 45°C at constant pressure ! Given molecular mass of N = 28 and R = 8.3 J / mol k

Solution → We have ,

➖◾Mass of gas m = 2 × 10^-2 kg = 20 g ✔

◾➖Change in Temprature i,e ∆T = 45°C

We need to find the change in heat i,e ∆Q

•°• Use the formula for n ( Number of moles)

=> n = m/M

→ n = 20/28 { as molecular mass of nitrogen is 28 }

→ n = 0.71 ✔

◼We know that nitrogen is a diatomic gas.

=> Cp = 7/2 R

=> Cp = 7/2 × 8.3 ( putting the value of R )

For ∆Q we know that ,

°•° ∆Q = n Cp ∆T

✔put the values we get :

=> ∆Q = 0.714 × 7/2 × 8.3 × 45

•°• ∆Q = 933.4 J approx.!

$....$

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