4. A 75.0-g sample of dinitrogen monoxide is confined in 3.1-L vessel. What is the pressure (in atm) at 115 ºC? show work please
dinitrogen monoxide = N2O
the molar mass is 2(N) + O = 2(14) + (16) = 44 g
So, there are n = (75.0 g)*(1 mol / 44 g) = 1.70 mol of N2O
Also, T = 115 C = 388.15 K
Using PV = nRT
P(3.1L) = (1.70 mol)(0.08205746 (L*atm)/(K*mol))(388.15 K)
Solving gives P = 17.51 atm (round appropriately.)
Dinitrogen Monoxide
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Verified answer
dinitrogen monoxide = N2O
the molar mass is 2(N) + O = 2(14) + (16) = 44 g
So, there are n = (75.0 g)*(1 mol / 44 g) = 1.70 mol of N2O
Also, T = 115 C = 388.15 K
Using PV = nRT
P(3.1L) = (1.70 mol)(0.08205746 (L*atm)/(K*mol))(388.15 K)
Solving gives P = 17.51 atm (round appropriately.)
Dinitrogen Monoxide