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78.5 g of Carbon dioxide gas fills a container that is 1.2 L. What is the
pressure of the gas in this container if the temperature of the gas is 45.1
degrees Celsius? Remember, you can't use temp. in degrees Celsius and
you need moles, not mass in grams so convert!!!

Respuesta :

nuhulawal20

Given the mass of the gas, temperature and volume of the cylinder, the pressure of the Carbon dioxide gas is 38.7atm.

What is Ideal Gas Law?

The Ideal gas law or general gas equation emphasizes on the state or behavior of a hypothetical ideal gas. It states that "the pressure multiplied by volume is equal to moles multiply by the universal gas constant multiply by temperature.

It is expressed as;

PV = nRT

Where P is pressure, V is volume, n is the amount of substance, T is temperature and R is the ideal gas constant ( 0.08206 Latm/molK )

Given that;

  • Mass of Carbon dioxide = 78.5g
  • Molar mass of Carbon dioxide 44.01 g/mol
  • Amount of gas n = 78.5g ÷ 44.01 g/mol = 1.78mol
  • Volume L = 1.2L
  • Temperature T = 45.1°C = 318.25K
  • Pressure P = ?

PV = nRT

P = nRT / V

P = ( 1.78mol × 0.08206 Latm/molK × 318.25K ) /  1.2L

P = 46.4857591Latm / 1.2L

P = 38.7atm

Therefore, given the mass of the gas, temperature and volume of the cylinder, the pressure of the Carbon dioxide gas is 38.7atm.

Learn more about Ideal Gas Law here: brainly.com/question/4147359

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