hydrogen gas is collected in a bottle, and the pressure of the gas is 892 torr at 24 °C. what is the pressure of hydrogen gas when the temperature decreases to 20 °C?
chemistry - DrBob222, Tuesday, November 30, 2010 at 1:25pm
(P1/T1) = (P2/T2)
Dear Dr Bob:
is this a right answer.
892/293 = P2/297
P2= 880 torr
Please reply for me this urgent.
Thanks
I get 879.9865 torr which rounds to 880 torr. We are allowed 3 significant figures from 892. Good work.
Yes, your answer is correct. To solve this problem, you can use the ideal gas law equation: (P1/T1) = (P2/T2), where P1 is the initial pressure, T1 is the initial temperature, P2 is the final pressure, and T2 is the final temperature.
In this case, the initial pressure is 892 torr and the initial temperature is 24 °C, which needs to be converted to Kelvin by adding 273 to it (24 + 273 = 297 K). The final temperature is 20 °C, which also needs to be converted to Kelvin (20 + 273 = 293 K).
By plugging these values into the equation, you get:
(892 torr / 297 K) = (P2 / 293 K)
Simplifying this equation, you can cross multiply and solve for P2:
892 torr x 293 K = P2 x 297 K
(892 torr x 293 K) / 297 K = P2
After performing the calculations, you find that P2 is equal to 880 torr. Therefore, the pressure of the hydrogen gas when the temperature decreases to 20 °C is 880 torr.