Ammonia gas occupies a volume of 5.00L at 4.00 degrees celcius and 760 torr. what is the volume at 77degrees celcius and 800 torr?
Use PV = nRT
P in atm and T in kelvin
To find the volume of ammonia gas at a different temperature and pressure, we can use the combined gas law equation:
(P1 x V1) / (T1) = (P2 x V2) / (T2)
Where:
P1 = initial pressure = 760 torr
V1 = initial volume = 5.00 L
T1 = initial temperature = 4.00 degrees Celsius + 273.15 = 277.15 Kelvin
P2 = final pressure = 800 torr
V2 = final volume (what we're trying to find)
T2 = final temperature = 77 degrees Celsius + 273.15 = 350.15 Kelvin
Now we can rearrange the equation to solve for V2:
V2 = (P1 x V1 x T2) / (P2 x T1)
Plugging in the given values:
V2 = (760 torr x 5.00 L x 350.15 K) / (800 torr x 277.15 K)
Now we can solve for V2:
V2 = (1330380 torr*K*L) / (221720 torr*K)
V2 = 5.99 L (rounded to two decimal places)
Therefore, the volume of the ammonia gas at 77 degrees Celsius and 800 torr is approximately 5.99 L.