If 91.5 mol of an ideal gas occupies 69.5 L at 31.00°C, what is the pressure of the gas?

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If 91.5 mol of an ideal gas occupies 69.5 L at 31.00°C, what is the pressure of the gas?

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Answer 1 · 2016-04-26T05:44:47

You will need to use the Ideal Gas Law to solve this problem:

$P V = n R T$ $PV = nRT$

Explanation:

To find pressure $(P)$ $(P)$ , derive from the Ideal Gas Law:

$P = \frac{n R T}{V}$ $P = (nRT)/V$

Gather up your known values, and plug them into the equation.

There are a few points to make here, Temperature $(T)$ $(T)$ must be converted to Kelvin.

$R$ $R$ = Ideal Gas Constant. This can have many forms. The one I used below is the one that I am most familiar with. Be aware of this though, and check which value you should be using per your curriculum.

$n = 91.5 m o l$ $n = 91.5 mol$
$V = 69.5 L$ $V = 69.5L$
$T = 31.0°C + (273.15K) = 304.15K$
$R = 8.314J/(mol*K)$

Finally,

$P = ((91.5mol)(8.314J/(mol*K))(304.15K))/(69.5L)$

$P = (x)atm$

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If 91.5 mol of an ideal gas occupies 69.5 L at 31.00°C, what is the pressure of the gas?

1 Answer

Explanation:

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