What is the pressure in atmospheres of a 2.50 mol gas in a 2.00 L bottle at 25.0ºC? The ideal gas constant is 0.0821 L·atm/mol·K

30.58 atm

Explanation:

Now recall that the ideal gas equation is given as ;

PV=nRT

Where;

P= pressure of the gas (the unknown)

V= volume of the gas= 2.00L

n= number of moles of the gas= 2.50 mol

T= temperature of the gas= 25.0° + 273 = 298K

R= ideal gas constant = 0.0821 L·atm/mol·K

Given all these parameters, we can now substitute into PV= nRT

Making P the subject of the formula;

P= nRT/V

substituting the given values into the equation;

P= 2.50 × 0.0821 × 298/2.00

P= 30.58 atm

Therefore, the pressure of the gas is 30.58 atm

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