Question

A sample of carbon monoxide and oxygen gasses are

allowed to combust in a small flask. They reaction is
described by the following equation.
2CO (g) + O₂ (g) → 2CO2 (g)
After the reaction is complete, the pressure of CO₂ is 0.868
atm and the temperature is 35.0 °C in a 500.0 mL flask. How
many moles of CO2 were produced assuming that the
reaction went to completion?

Answer 1

.0172 mole of CO2

Step-by-step explanation:

PV = nR T n = number of moles V = .5 liter

R = gas constant = .082057 L atm/(k mole)

T needs to be in Kelvin = C + 273.15

.868 * .5 = n * .082057 * ( 35 + 273.15)

n = .0172 moles