Metal oxides react with carbon and are reduced to the metal. The metal in the reaction above is copper.
The equation of the reaction is;
2MO(s) + C(s) -> 2M(s) + CO2(g)
We are told in the question that carbon is in excess so the metal oxide is the limiting reactant.
Number of moles of metal oxide = 34.49 g/M + 16
From PV = nRT
P = 1.50 atm
V = 4.42 L
T = 100°C + 273 = 373 K
n =?
R = 0.082 atmLK-1mol-1
n = PV/RT
n = 1.50 atm × 4.42 L/0.082 atmLK-1mol-1 × 373 K
n = 6.63/30.58
=0.217 moles
If 2 moles of metal oxide yields 1 mole of CO2
34.49 g/M + 16 yields 0.217 moles of CO2
34.49 g/M + 16 = 2 × 0.217
34.49 /M + 16 = 0.434
34.49 = 0.434(M + 16)
34.49 = 0.434M + 6.944
M = 34.49 - 6.944/0.434
M = 63.5
The metal is copper.
Learn more: brainly.com/question/22824409
