How many moles of H2 would be contained in 4.0 L of the gas at 202.6 kPa and 127°C?

A. 89.6 mol

B. 6.38 mol

C. 0.24 mol

D. 0.77 mol

Question

How many moles of H2 would be contained in 4.0 L of the gas at 202.6 kPa and 127°C?



 
A. 89.6 mol 
 
 
B. 6.38 mol 
 
 
C. 0.24 mol 
 
 
D. 0.77 mol

taramgrant0543664 · Answer

You're going to have to use the formula PV=nRT
P is the pressure 
V is your volume 
n is the number of moles
R is the ideal gas constant 
T is your temperature

taramgrant0543664 · Answer

The Pressure would have to be in atmospheres in order to use 0.0821 as your R value and your temperature has to be in Kelvin instead of celcius

taramgrant0543664 · Answer

202.6kPa is equal to 2.0atm so thats your pressure that you can use in the formula
127+273=400K so you can use 400K as your temperature

taramgrant0543664 · Answer

P=2.0atm
V=4.0L
n=unknown
R=0.0821L-atm/mole-K
T=400K
Put them into the formula to solve for n

photon336 · Answer

$$\frac{ pV }{ RT } = n $$