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1.Calculate the number of moles of PCl5 that can be produced from30.0 of P4 (and excess Cl2 ).
2.Calculate the number of moles of PCl5 that can be produced from53.0 of Cl2 (and excess P4 ).
Then, compare the two values. The reactant that produces thesmaller amount of product is the limiting reactant

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4 Jul 2019
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Related questions

In the gaseous state, chlorine exists as a diatomic molecule Cl2 (Molar mass = 70.9 g/mol). Calculate the number of moles of chlorine present in 100 g of chlorine gas.

2 PART QUESTION! How many moles of PCl5 can be produced from 55.0 g of Cl2 (and excess P4)? 0.310 mole Actual Question: 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.

The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water.

4NH3(g)+5O2(g)ҟ¢4NO(g)+6H2O(g)

What is the maximum mass of H2O that can be produced by combining 21.6 g of each reactant?

STRATEGY:

Convert 21.6 g NH3 to moles, then find the corresponding amount of H2O.

Convert 21.6 g O2 to moles, then find the corresponding amount of H2O.

Identify the limiting reactant and calculate the mass of H2O produced.

Step 1: 21.6 g NH3 and excess O2 produce 1.90 mol H2O.

Step 2: 21.6 g O2 and excess NH3 produce 0.810 mol H2O.

Step 3: When 21.6 g NH3 and 21.6 g O2 are mixed, how many moles of H2O form?

(1) 1.90 + 0.810 mol H2O

(2) 0.810 mol H2O

(3) 1.90 mol H2O

Calculate the mass of H2O produced from the number of moles of H2O.

mass: [???] g H2O

3.20 g of H2 is ignited in a vessel containing 22.50 g O2 to produce H2O as the only product.

A. Write a balanced equation for this reaction.

2H2 + O2 ---> 2H2O --- not sure if that's right/balanced correctly.

B. Calulate the number of moles of H2O produced by 3.20 g of H2.

C. Calculate the number of moles of H2O produced by 22.50 g of O2,

D. Identify the limiting reactant.

E. Calculate the total mass of H2O produced in this reaction.

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