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# Answer to Question #55699 in General Chemistry for sue

Question #55699
Now consider a situation in which 26.0 g of P4 is added to 59.0 g of Cl2, and a chemical reaction occurs. To identify the limiting reactant, you will need to perform two separate calculations:
1.Calculate the number of moles of PCl5 that can be produced from 26.0 g of P4 (and excess Cl2).
2.Calculate the number of moles of PCl5 that can be produced from 59.0 g of Cl2 (and excess P4).
Then, compare the two values. The reactant that produces the smaller amount of product is the limiting reactant.**answer to #1 is 0.839 moles...answer to #2 is 0.333 moles
Info needed:What mass of PCl5 will be produced from the given masses of both reactants?
Express your answer to three significant figures and include the appropriate units.
P4 + 10Cl2 = 4PCl5
1.
n(PCl5) = 4*n(P4) = 4*m(P4)/M(P4) = 4*26/124 = 0.839 mol
m(PCl5) = M(PCl5)*n(PCl5) = M(PCl5)*4*n(P4) = M(PCl5)*4*m(P4)/M(P4) = 208.5*4*26/124 = 174.9 g
2.
n(PCl5) = 0.4*n(Cl2) = 0.4*m(Cl2)/M(Cl2) = 0.4*59/71 = 0.332 mol
m(PCl5) = M(PCl5)*n(PCl5) = M(PCl5)*0.4*n(Cl2) = M(PCl5)*0.4*m(P4)/M(P4) = 208.5*0.4*59/71 = 69.3 g

1. m(PCl5) = 174.9 (g)
2. m(PCl5) = 69.3 (g)

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