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