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In order to solve for the pressure of a gas when given its volume and amount in grams and the temperature, we need to use the ideal gas law.
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Pv equals nrt.
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Remember, when using the ideal gas law, these variables have very specific units.
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For pressure, we must be in atmospheres.
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For the volume, we must be in liters.
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The amount of the gas, n, must be in moles.
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And the temperature must be in kelvin's.
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This r value is a constant called the universal gas law constant, and it has a value of 0 .0821.
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And the units on this are atmospheres times liters per mole kelvin.
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If we need to solve the ideal gas law for pressure, we would rearrange the equation to say pressure equals n times.
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R times t divided by v then we can start plugging in values for the different variables let's say for example for the amount of gas we have 24 grams of oxygen so for the n here we cannot put in grams we have to switch these grams over to moles so if we had 24 grams of o2 gas we would do a mole conversion and basically we would multiply by one mole of oxygen over its molar mass from the periodic table...