Question

A sample of hydrogen gas at a pressure of 1.14 atm and a temperature of 27.1 °C, occupies a volume of 13.6 liters. If the gas is allowed to expand at constant temperature to a volume of 19.1 liters, the pressure of the gas sample will be atm. 

          A sample of hydrogen gas at a pressure of 1.14 atm and a temperature of 27.1 °C, occupies a volume of 13.6 liters. If the gas is allowed to expand at constant temperature to a volume of 19.1 liters, the pressure of the gas sample will be 
 atm.
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Chemistry: Structure and Properties
Chemistry: Structure and Properties
Nivaldo Tro 2nd Edition
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A sample of hydrogen gas at a pressure of 1.14 atm and a temperature of 27.1 °C, occupies a volume of 13.6 liters. If the gas is allowed to expand at constant temperature to a volume of 19.1 liters, the pressure of the gas sample will be atm.
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Transcript

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00:01 Hello there so for this question we're checking on a sample of hydrogen gas okay so gas where it's at a pressure of 1 .14 atm and has a temperature of 27 .1 degrees celsius that occupies a volume of 13 .6 liters so if the gas is allowed to expand at a constant temperature of let's say 19 .1 liters the pressure of the gas samples would be at atm so we're seeing they're questioning like what will the change be if the temperature if it expands and increase how it's going to have an effect on the pressure so for this question we're going to do our ideal gas and the way we're going to set up that we're going to solve for the for the pressure so we're going to times the volume which oops which will be p equals to nrt over phi so how we're going to do the equation that we're missing our n for our mold so how we're going to solve for the mold is we're going to solve our hydrogen gas so for our hydrogen gas our hydrogen gas is 2 .01568 and how i solve it i just times um its molar mass um by two let me fix that g okay and oops we're gonna times that by one mole of the hydrogen gas over our 1 .00784 grams so when we work on our calculation we should get we should get h equals two moles all right so now we got that part down and also what we have to change oh i'm…
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