Ok ive been working on this problem for hours now, can you please tell me if i am correct? Thank You!
A gas occupies 340mL at 273 K and 610 torr. What final temperature would be required to increase the pressure to 1 atm, the volume being held constant?
P1/T1 = P2/T2
T2 = (T1*P2)/ P1
1 atm = 760 torr
So,
T2 = (273 K * 760 torr)/610 torr
T2 = 340 K
340 K is correct.
To solve this problem, you can use the combined gas law equation P1/T1 = P2/T2, which relates the pressure and temperature of a gas when the volume is held constant.
Given:
P1 = 610 torr
T1 = 273 K
P2 = 1 atm = 760 torr
To find T2, we need to rearrange the equation as follows:
T2 = (T1 * P2) / P1
Substituting the given values:
T2 = (273 K * 760 torr) / 610 torr
T2 ≈ 340 K (rounded to the nearest whole number)
Therefore, the final temperature required to increase the pressure to 1 atm, with the volume held constant, is approximately 340 K.