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How many grams of a gas with a molar mass 36.02 g/mol would be required to occupy a 3979 mL flask at 1.07 atm and 81.7 degrees Celcius? Record your answer in scientific notation to 2 decimal spaces.

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A 3979 mL flask is occupied by 5.26 g of a gas with a molar mass of 36.02 g/mol at 1.07 atm and 81.7 °C.

What is an ideal gas?

An ideal gas is that whose behavior can be explained using the ideal gas laws.

  • Step 1. Convert 81.7 °C to Kelvin.

We will use the following expression.

K = °C + 273.15 = 81.7 + 273.15 = 354.9 K

  • Step 2. Calculate the moles of the gas.

We will use the ideal gas equation.

P × V = n × R × T

n = P × V / R × T

n = 1.07 atm × 3.979 L / (0.08206 atm.L/mol.K) × 354.9 K = 0.146 mol

  • Step 3. Calculate the mass of the gas.

The molar mass of the gas is 36.02 g/mol.

0.146 mol × 36.02 g/mol = 5.26 g

A 3979 mL flask is occupied by 5.26 g of a gas with a molar mass of 36.02 g/mol at 1.07 atm and 81.7 °C.

Learn more about ideal gases here: https://brainly.com/question/15634266