Question

A chemical reaction with an initial quantity of 1.35 moles of gas is performed in a 4.50-L flask at 24.7°C and under 1.07 atm of pressure. After the reaction is complete the final temperature is 55.2°C with a pressure of 2.92 atm. If the volume is limited by the size of the flask, how many moles of gas are present in the container after the reaction is complete?

Answer 1

0.488 mol

Step-by-step explanation:

By the ideal gas law:

PV = nRT

Where P is the pressure, V is the volume, n is the number of moles, R is the gas constant (0.082 atm.L/mol.K), and T is the temperature in K. Thus, after the reaction:

P = 2.92 atm

V = 4.50 L

T = 55.2°C + 273 = 328.2 K

PV = nRT

n = PV/RT

n = (2.92*4.50)/(0.082*328.2)

n = 0.488 mol