avogadros law in gas reduction

Question

A sample of gas contains 0.1500 mol of NH₃(g) and 0.1875 mol of O₂(g) and occupies a volume of 10.9 L. The following reaction takes place:

4NH₃(g) + 5O₂(g)4NO(g) + 6H₂O(g)

1.Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.

 _________L

A sample of gas contains 0.1200 mol of C₂H₄(g) and 0.1200 mol of H₂O₂(g) and occupies a volume of 8.80 L. The following reaction takes place:

C₂H₄(g) + H₂O₂(g)CH₂OHCH₂OH(g)

2.Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.

____________ L

Answer 1

Temperature and Pressure are constant, so moles (n) and volume (V) change.

V1/n1 = V2/n2

n1 = 0.1500 moles + 0.1875 moles = 0.3375 moles

V1 = 10.9 L

n2 = 0.3375 moles x 10/9 = 0.375 (there are 10 moles of gas on product side and 9 moles on reactant side)

V2 = ?

10.9/0.3375 = V2/0.375

V2 = 12.1 L

V1/n1 = V2/n2

V1 = 8.80 L

n1 = 0.1200 + 0.100 = 0.2400

V2 = ?

n2 = 0.2400 x 1/2 = 0.1200 (there is 1 mole of gas on product side and 2 moles on reactant side)

8.80/0.2400 = V2/0.1200

solve for V2