# A 2.00 L tank contains an unknown gas that is 53.31% carbon, 11.18% hydrogen, and 35.51% oxygen by mass. At 35.0 °C and 0.470 bar, the gas in the tank has a mass of 3.30 g.What is the empirical formula of the gas?empirical formula:__________________________How many moles of gas are in the tank?moles of gas: _____________________ molWhat is the molecular formula of the gas?molecular formula: _________________

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A 2.00 L tank contains an unknown gas that is 53.31% carbon, 11.18% hydrogen, and 35.51% oxygen by mass. At 35.0 °C and 0.470 bar, the gas in the tank has a mass of 3.30 g.

What is the empirical formula of the gas?

empirical formula:__________________________

How many moles of gas are in the tank?

moles of gas: _____________________ mol

What is the molecular formula of the gas?

molecular formula: _________________

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Step 1

Given,

An unknown gas that is 53.31% carbon, 11.18% hydrogen, and 35.51% oxygen by mass. this means that 100 g of the gas contains:

Mass of carbon = 53.31 g

Mass of hydrogen = 11.18 g

Mass of oxygen = 35.51 g

Moles of C, H and O can be calculated as:

Step 2

The empirical formula of the gas can be written by finding the simplest whole molar ratio as:

Step 3

Given,

Pressure, P = 0.470 bar = 0.464 atm      ( 1 bar = 1/1.013 atm)

Volume, V = 2.00 L

Temperature, T = 35.0 °C = (...

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