a gaseous mixture containing 7.0 gram nitrogen and 11.0 carbon dioxide at 290 Kelvin exerts a pressure of 1.0 atm find the density of the mixture resuming them to be ideal
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Assuming the mixture to behave as an ideal gas.
molecular weight of CO2 = 12+16+16 = 44
molecular weight of SO2 = 32+16+16 = 64
moles of CO2 = 7.5/44 = 0.17045
moles of SO2 = 10/64 = 0.15625
n= moles of CO2 + moles of SO2 = 0.15625 + 0.17045 = 0.3267
V= 2.5L = 2.5*10^-3 m^3
T= 25C = 298K
PV = nRT
P = nRT/V = 0.3267*8.314*298/(2.5*10^-3) = 323769.10896 Pa
= 3.1953atm
molecular weight of CO2 = 12+16+16 = 44
molecular weight of SO2 = 32+16+16 = 64
moles of CO2 = 7.5/44 = 0.17045
moles of SO2 = 10/64 = 0.15625
n= moles of CO2 + moles of SO2 = 0.15625 + 0.17045 = 0.3267
V= 2.5L = 2.5*10^-3 m^3
T= 25C = 298K
PV = nRT
P = nRT/V = 0.3267*8.314*298/(2.5*10^-3) = 323769.10896 Pa
= 3.1953atm
Answered by
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your answer is 3.19 of the numerical
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