A 3.25 liter container of ammonia gas exerts a pressure of 652 mm Hg at a temperature of 243 Kelvin. Calculate the pressure of this same amount of gas in a 2.50 Liter container at a temperature of 221 Kelvin

1.01atm

Explanation:

First, we need to calculate the numbers of mol of ammonia. This can be achieved by doing the following:

V = 3.25L

P = 652mmHg we must convert this to atm by:

760mmHg = 1atm

652mmHg = 652/760 = 0.858atm

T = 243K

R = 0.082atm.L/K /mol

n =?

PV = nRT

n = PV /RT

n = (0.858 x 3.25)/(0.082x243)

n = 0.14mol

From the question, we were to that the other gas had the same amount(0.14mol) as ammonia. We can calculate for the pressure of the gas as illustrated below:

P =?

V = 2.5L

T = 221K

R = 0.082atm.L/k/mol

n = 0.14mol

PV = nRT

P = nRT /V

P = (0.14x0.082x221) / 2.5

P= 1.01atm

your answer is a. the enthalpy of formation for a pure element in its standard state is always positive.