Given the mass of the gas, temperature and volume of the cylinder, the pressure of the Carbon dioxide gas is 38.7atm.
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What is Ideal Gas Law?</h3>
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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