Could someone check my answer.
"If a sample of CO2 gas has a mass of 1.5 grams when the atmospheric pressure is 202 kPa and the temperature is 25 degrees C, what would the density of the gas be at STP?"
Solve for initial volume under conditions 202kpa (1.99 atm), 1.5g CO2, and 25C (298K)
PV = N * R * T is modified to PV = (mass/molar mass) * R * T
(1.99 atm) (V) = (1.5 g /44 g/mol) (0.0821 L*atm/mol*K) (298K)
V = 0.419 L
At STP, conditions are always 1 atm, 273K, and 1 mole gas = 22.4 L
(P1) * (V1)/ (T1) = (P2) * (V2)/ (T2) is modified to V2 = V1 * (P1/P2) * (T2/T1)
V2 = (0.419 L) * (1 atm/ 1.99 atm) * (273K/ 298K) = 0.193 L
Density is (moles/L).
0.034 moles/ 0.193 L = 0.18 moles/L
"If a sample of CO2 gas has a mass of 1.5 grams when the atmospheric pressure is 202 kPa and the temperature is 25 degrees C, what would the density of the gas be at STP?"
Solve for initial volume under conditions 202kpa (1.99 atm), 1.5g CO2, and 25C (298K)
PV = N * R * T is modified to PV = (mass/molar mass) * R * T
(1.99 atm) (V) = (1.5 g /44 g/mol) (0.0821 L*atm/mol*K) (298K)
V = 0.419 L
At STP, conditions are always 1 atm, 273K, and 1 mole gas = 22.4 L
(P1) * (V1)/ (T1) = (P2) * (V2)/ (T2) is modified to V2 = V1 * (P1/P2) * (T2/T1)
V2 = (0.419 L) * (1 atm/ 1.99 atm) * (273K/ 298K) = 0.193 L
Density is (moles/L).
0.034 moles/ 0.193 L = 0.18 moles/L