A mixture of CS2 (g) and excess O2 (g) is contained in a 20.0 liter reaction ves

Question

A mixture of CS2 (g) and excess O2 (g) is contained in a 20.0 liter reaction vessel at 130 degrees celsius; the total pressure of the mixture is 3.0 atm. A spark causes the CS2 to ignite, and it burns completely according to a the following equation.

CS2 (g) + 3O2 (g) ----> CO2 (g) + 2SO2 (g).

The vessel and contents are returned to 130 degree celsius and the mixture of product gases (CO2, SO2, and unreacted O2) has a total pressure of 2.4 atm. Determine the partial pressure of each of these gases in the final product mixture

Explanation / Answer

O2 is in excess

4 moles of reactants give 3 moles of product, difference is 1mole

0.6 x 4 atm of reactants give 0.6 x 3 atm, so amount of CS2 is 0.6 atm

amount of CO2 is equal to amount of CS2 =0.6 atm

amount of SO2 is 1.2

amount of O2 is 2.4 -(1.2+0.6) = 0.6

so partial pressures of O2 is 0.6, CO2 is 0.6 and CS2 is 1.2

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.