This experiment was performed using 1.00 atm of gas at 294.6 K. However, STP con

Question

This experiment was performed using 1.00 atm of gas at 294.6 K. However, STP conditions are 1.00 atm 273.15 K. Use the Ideal Gas Law to calculate the volume that the same number of moles of gas will occupy at STP. Calculate the molar volume at STP. How does your STP molar volume to the known value of 22.4 L? R is 0.0820 L atm mon^-1 K^-1. Record your data in the table below. Suppose 0.274 mol of a gas occupy 6.62 L at a given temperature and pressure. What volume will 0.878 mol occupy at the same temperature and pressure? Use Avogadro's Law to explain why a flat tire takes up less space than an inflated tire. The tire has air in it, the law states that gas is directionally proportional to the number of moles of gas. What mass of propane will occupy the same volume as 0.057 mol of butane at 1.00 atm and 298 K?

Explanation / Answer

According to Ideal gas law : PV = nRT

P = 1 atm, V = 150mL = 0.15 L, T = 294.6 K

n = ?

For STP conditions :

P = 1 atm, V = ?, n = 6.21*10^-3 , T = 273.15 K

V = nRT/P

To calculate molar volume :

Volume at STP /number of moles

propane Butane Methane No of moles in 150mL 6.21*10^-3 6.21*10^-3 6.21*10^-3 volume at STP 0.139 L 0.139L 0.139L Molar volume at STP 22.38 L 22.38 L 22.38 L

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