The ideal gas law is presented
by the equation PV = nRT. n, the number of moles, is equal to mass over molar
mass. And density is M/V.
PV = nRT
PV = (M/molar mass)RT
P/RT = (1/molar mass)(M/V)
M/V = D = (molar mass)(P/RT)
Molar mass of CO2 = 44 g/mol
D = (molar mass)(P/RT)
D = (44 g/mol)(1 atm)/(0.08206
L-atm/mol-K)(273K)
D = 1.964 g/L
Which is not a pure substance?
(C) antifreeze
Answer:
17.27 atm
Explanation:
Use the ideal gas law or PV = nRT
We are solving for pressure here so lets isolate for P before we plug in values:
So first to get n or the number of moles we need to convert the grams of N2O to moles of N2O. We can do this by multiplying by the inverse of the molar mass like so:
Our grams of N2O would cancel and give us 11.813 mol of N2O
Now all thats left is to plug in and solve with the correct value for R which in this case for all of our units to cancel is 0.08206
P = 17.27 atm
(I would double check the calculator work if it is for correctness just be sure)