First, let's convert the initial pressure from torr to atm:
1 atm = 760 torr
Initial pressure = 759 torr / 760 torr/atm = 0.9987 atm
Now, we can use the combined gas law equation:
P1V1 = P2V2
Where:
P1 = initial pressure = 0.9987 atm
V1 = initial volume = 5.52 L
P2 = final pressure = 1.89 atm
V2 = final volume (unknown)
Plugging in the values:
0.9987 atm * 5.52 L = 1.89 atm * V2
5.5116 = 1.89 * V2
V2 = 5.5116 / 1.89
V2 = 2.9145 L
Therefore, the gas will occupy a volume of 2.9145 L when the pressure is increased to 1.89 atm and the temperature is held constant.
A fixed quantity of gas at 23 ∘C
exhibits a pressure of 759 torr
and occupies a volume of 5.52 L
.Calculate the volume the gas will occupy if the pressure is increased to 1.89 atm
while the temperature is held constant.
1 answer
1 answer