Question

At constant volume, a container of gas at atmospheric pressure is heated from 27 degrees Celsius to 77 degrees Celsius. What is the final pressure?
1.2 atm
2.8 atm
0.35 atm
0.86 atm

Answer 1

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We know, (V1/T1)=(V2/T2)

Here, V1 = V (say), Then V2 = 3V

Putting in the formula we get T2 = 900K = 6270C

Answer 2

Answer:

The final pressure will be 1.17 atm. i.e.none of the options is correct.

Explanation:

We will use Gay-Lussac's law in this question. Which is given as,

$\frac{P_1}{T_1} =\frac{P_2}{T_2}$         (1)

Where,

P₁=initial pressure

T₁=initial temperature

P₂=final pressure

T₂=final temperature

From the question we have,

P₁=1 atm          (as gas is at atmospheric pressure)

T₁=27°C+273=300K

T₂=77°C+273=350K

By substituting the value of P₁, T₁, and T₂ in equation (1) we get;

$\frac{1}{300} =\frac{P_2}{350}$

$P_2=\frac{350}{300}\approx 1.17atm$

Hence, the final pressure will be 1.17 atm. i.e.none of the options are correct.