Question #55675
How many moles of PCl5 can be produced from 59.0 g of Cl2 (and excess P4)?
Express your answer to three significant figures and include the appropriate units.
Express your answer to three significant figures and include the appropriate units.
Expert's answer
The balanced chemical eqiation is
P4 + 10Cl2 = 4PCl5[sub]
The mass of clorine is m(Cl[sub]2) = 59.0 g
The amount of clorine is n(Cl2) = m(Cl2)/M(Cl2) = 59/70.906 = 0.832 mol
The reacion stoichiometry shows that
10 moles of Cl2 yield 4 moles of PCl5;
0.832 of Cl2 yield x moles of PCl5
n(PCl5) = 4*0.832/10 = 0.333 mol
Answer: 0.333 mol
P4 + 10Cl2 = 4PCl5[sub]
The mass of clorine is m(Cl[sub]2) = 59.0 g
The amount of clorine is n(Cl2) = m(Cl2)/M(Cl2) = 59/70.906 = 0.832 mol
The reacion stoichiometry shows that
10 moles of Cl2 yield 4 moles of PCl5;
0.832 of Cl2 yield x moles of PCl5
n(PCl5) = 4*0.832/10 = 0.333 mol
Answer: 0.333 mol
