Consider two identical 1-L containers, both at room temperature (300 K). One of them contains 1.0 g

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Consider two identical 1-L containers, both at room temperature (300 K). One of them contains 1.0 g of helium gas, and the other contains 1.0 g of hydrogen gas. Is the pressure higher in the helium container, higher in the hydrogen container, or the same in the two containers?

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To determine the pressure in the two containers we need to use the ideal gas law equation PV nRT Volume V 1 L Temperature T 300 K Number of moles n mass m molar mass M 1 For helium gas Mass of helium gas m 10 g Molar mass of helium M 40026 gmol The number of moles of helium n is calculated as n helium 10 g 40026 gmol 02498 mol 2 For hydrogen gas Mass of hydrogen gas m 10 g Molar mass of hydrogen M 20159 gmol The number of moles of hydrogen n is calculated as n hydrogen 10 g 20159 gmol 04961 mol Next we can calculate the pressure P using the ideal gas law equation P ...View the full answer

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