Hello,
i need some help solving. not sure if i did this correctly or not. Please show steps so i may correct and check accordingly. thanks so much for your help and assistance!
A group of students has added a 12.5 g sample of a gas to an evacuated, constant volume container at 22° C. The pressure of the gas is greater than atmospheric pressure. Now the students will heat the gas at constant pressure. The easiest way to do this is to allow some of the gas to escape during heating. what mass of gas must be released if the temperature is raised to 202°C?
thanks again!
i need some help solving. not sure if i did this correctly or not. Please show steps so i may correct and check accordingly. thanks so much for your help and assistance!
A group of students has added a 12.5 g sample of a gas to an evacuated, constant volume container at 22° C. The pressure of the gas is greater than atmospheric pressure. Now the students will heat the gas at constant pressure. The easiest way to do this is to allow some of the gas to escape during heating. what mass of gas must be released if the temperature is raised to 202°C?
thanks again!
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Let T1 = the initial temperature = 22° C = 295° K
Let T2 = the final temperature = 202° C = 475° K
Let P = the constant pressure
Let V = the constant volume
Let k = molar mass of the gas
Let m = the final mass of the gas
Let n1 = the initial number of moles of the gas = 12 g/k
Let n2 = the final number of moles of the gas = m/k
PV =(12 g/k)(R)(T1) = (m/k)(R)(T2)
m = (12 g)(295)/475
m = 7.45 g
The mass released is the difference, 4.55 g.
Let T2 = the final temperature = 202° C = 475° K
Let P = the constant pressure
Let V = the constant volume
Let k = molar mass of the gas
Let m = the final mass of the gas
Let n1 = the initial number of moles of the gas = 12 g/k
Let n2 = the final number of moles of the gas = m/k
PV =(12 g/k)(R)(T1) = (m/k)(R)(T2)
m = (12 g)(295)/475
m = 7.45 g
The mass released is the difference, 4.55 g.