To solve this problem, we can use the combined gas law formula:
(P1)(V1)/(T1) = (P2)(V2)/(T2)
Where:
P1 = initial pressure = 76 cmHg
V1 = initial volume = 500 cm^3
T1 = initial temperature = 400°C + 273 = 673 K
P2 = final pressure (unknown)
V2 = final volume = 600 cm^3
T2 = final temperature = 120°C + 273 = 393 K
Plugging in the values:
(76)(500)/(673) = (P2)(600)/(393)
Solving for P2:
38000/673 = 600P2/393
56.45 = 1.525P2
P2 = 56.45/1.525
P2 ≈ 37 cmHg
Therefore, the pressure of the gas at the temperature of 120°C is approximately 37 cmHg.
Some quantity of dry air has volume of 500cm cube at 400degree Celsius and under pressure of 76cmhg at a temperature of 120 degree Celsius it's volume become 600cm cube calculate the pressure of the gas at the temperature
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