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If 1.00 L of an unknown gas at STP has a mass of 5.40 g, what is its molar mass?

Answer 1

Serenity Allen

Approx, #121*g*mol^-1#

The molar volume at #"STP"# is #22.4*L*mol^-1#.

Given this, if we divide the mass by the molar quantity of the gas we get an answer in #g*mol^-1# as required:

#(1.00*L)/(22.4*L*mol^-1)# #=# #0.0446*mol#

#"Molar mass"# #=# #(5.40*g)/(0.0446*mol)# #=# #121*g*mol^-1#

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Answer 2

Henry Antrim

To find the molar mass of the unknown gas, you can use the ideal gas law equation:

Molar mass (M) = (mass of gas / volume of gas) × (molar volume of gas at STP)

Given: Mass of gas = 5.40 g Volume of gas = 1.00 L Molar volume of gas at STP = 22.4 L/mol

Molar mass (M) = (5.40 g / 1.00 L) × (22.4 L/mol) M = 120.96 g/mol

So, the molar mass of the unknown gas is approximately 120.96 g/mol.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.