How many litres of O2 will be produced at a temperature of 37 degrees Celsius and 1520 torr if 2 moles of KCIO3 decompose according to the following balanced equation?

Question

How many litres of O2 will be produced at a temperature of 37 degrees Celsius and 1520 torr if 2 moles of KCIO3 decompose according to the following balanced equation?

2KCIO3 -> 2KCI + 3O2

Answer 1

2KCIO₃ -> 2KCI + 3O₂ .. balanced equation

First, find the moles of O2 produced, and then use the ideal gas law to calculate the volume in liters.

moles O2 produced = 2 moles KClO3 x 3 moles O2 /2 moles KClO3 = 3 moles O2 produced

Ideal gas law: PV = nRT

P = pressure in atm = 1520 torr x 1 atm / 760 torr = 2 atm

V = volume in liters = ?

n = moles of O2 = 3 moles

R = gas constant = 0.0821 Latm / Kmole

T = temperature in Kelvin = 37ºC + 273 = 310K

Solve for V (volume):

V = nRT / P = (3)(0.0821)(310) / 2

V = 38.2 liters (not corrected for sig. figs.)