molar mass of unknown gas = 58.0 g/mol
Explanation
According to Graham's effusion law
t2 / t1 = (M2 / M1)1/2
where t1 = 34.4 s
M1 = molar mass O2 = 32.0 g/mol
t2 = 46.3 s
Substituting the values,
46.3 / 34.4 = (M2 / 32.0 g/mol)1/2
(M2 / 32.0 g/mol)1/2 = 1.346
M2 / 32.0 g/mol = (1.346)2
M2 / 32.0 g/mol = 1.81
M2 = (1.81) * (32.0 g/mol)
M2 = 58.0 g/mol
A gas effusion cellis loaded with O2 gas at STP it take 344 seconds 0.010% of the gas to effuse through the hole. U...
A gas effusion cell is loaded with O2 gas at STP it take 35.7 seconds 0.010% of the gas to effuse through the hole. Under the same conditions, an unknown gas takes 56.3 seconds for 0.010% of gas to effuse through the hole. Based on these data, what is the molar mass of the unknown gas (in g/mol)? QUESTION 2 A sample of gas is contained in a cylinder with a movable piston. The initial conditions of the gas are...
Please help! QUESTION 1 A gas effusion cell is loaded with O2 gas at STP it take 34 seconds 0.010% of the gas to effuse through the hole. Under the same conditions, an unknown gas takes 59.4 seconds for 0.010% of gas to effuse through the hole. Based on these data, what is the molar mass of the unknown gas (in g/mol)? QUESTION 2 A sample of gas is contained in a cylinder with a movable piston. The initial conditions...
A gas of unknown molecular mass was allowed to effuse through a small opening under constant pressure conditions. It required 67 s for 1.0 L of the gas to effuse. Under identical experimental conditions it required 31 s for 1.0 L of O2 gas to effuse. Calculate the molar mass of the unknown gas. (Remember that the faster the rate of effusion, the shorter the time required for effusion of 1.0 L; that is, rate and time are inversely proportional.)
A gas of unknown molecular mass was allowed to effuse through a small opening under constant pressure conditions. It required 52 s for 1.0 L of the gas to effuse. Under identical experimental conditions it required 27 s for 1.0 L of O2 gas to effuse. Calculate the molar mass of the unknown gas. (Remember that the faster the rate of effusion, the shorter the time required for effusion of 1.0 L; that is, rate and time are inversely proportional.)...
1. The rate of effusion of CH4 gas through a porous barrier is observed to be 9.17*10^-4 mol/h. Under the same conditions, the rate of effusion of gas would be _____________ mol/h. 2. A sample of N2 gas is observed to effuse through a pourous barrier in 1.93 minutes. Under the same conditions, the same number of moles of an unknown gas requires 2.97 minutes to effuse through the same barrier. The molar mass of the unknown gas is _______________
A sample of O2 gas is observed to effuse through a pourous barner in 5.93 minutes. Under the sa,e number of moles of an unknown gas requires 3.92 minutes to effuse through the same barrier. The molar mass the unknown gas is g/mol.
under identical conditions separate samples of O2 and an unknown gas were allowed to effuse through identical membranes simultaneously. after a certain amount of time it was found that 5.39 mL of O2 had passed through the membrane but only 3.33 mL of the unknown gas had passed through, what is the molar mass of the unknown gas?
Under identical conditions, separate samples of O2 and an unknown gas were allowed to effuse through identical membranes simultaneously. After a certain amount of time, it was found that 7.83 mL of O2 had passed through the membrane, but only 3.87 mL of of the unknown gas had passed through. What is the molar mass of the unknown gas?
Under identical conditions, separate samples of O2 and an unknown gas were allowed to effuse through identical membranes simultaneously. After a certain amount of time, it was found that 6.71 mL of O2 had passed through the membrane, but only 3.14 mL of of the unknown gas had passed through. What is the molar mass of the unknown gas? Number g/mol
4. 1.10 mol of ozone (O3) in a container took 28.4 seconds to effuse through a pinhole into a vacuum. Under the exact same conditions, 1.10 mol of an unknown gas took 70.1 seconds to effuse. a) What is the molar mass of the unknown gas (in g/mol)? Do not try to identify the gas. (2 marks) b) What is Urms of the ozone gas at a temperature of 37"C? Express your answer in m/s. (2 marks)