A gas occupies a volume of 200 ml at a pressure of 4 atm .If temperature remains constant what volume will it occupy at 1 atm URGENT
Answers
Explanation:
gas x occupies a volume of 200ml at a pressure of 4 ... If the temperature remains constant what volume will it occupy at 1atmospheric pressure ... 200 ml. P1 =4 atm.
Answer:
A gas occupies a volume of 200....
This problem can be solved using the combined gas law,
(P_1V_1)/(T_1) = (P_2V_2)/(T_2)
where P is pressure, V is volume, T is Kelvin temperature and the subscripts 1 and 2 denote initial and final conditions.
Rearranging, we get
T_2 = (P_2V_2T_1)/(P_1V_1)
T2 = (760 torr)(250 ml)(298K)/(380 torr)(200 ml) = 745 K
The combined gas law comes from the Ideal Gas Law, PV=nRT.
PV/nT = a constant (R), so P1V1/n1T1 = P2V2/n2T2. We can leave out n, the number moles, if it's constant. This leaves us with the combined gas law, a combination of Boyle's and Charles' laws.
Boyle's law says that at constant temperature the pressure and volume of a gas are inversely proportional: P1V1 = P2V2
Charles' law says that at constant pressure the temperature and volume of a gas are directly proportional: V1/T1 = V2/T2