Elemental phosphorus reacts with chlorine gas according to the equation: P 4 (s) + 6 Cl 2 ( g) → 4 PCl 3 (l) A reaction mixture initially contains 45.69 g P 4 and 131.3 g Cl 2 . Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

Hi everyone today, we have a question asking us at the beginning of the reaction, there are 34.67g of copper oxide and 9.87 g of carbon monoxide. And we want to calculate the amount in grams of excess reactant that remains after the reaction has come to the completion and our reaction is copper copper oxide solid plus three carbon monoxide gashes forms to copper solid plus three carbon carbon dioxide gashes. So let's start out with our three 34 0.67 grams of copper oxide times one mole of copper oxide, divided by 175. g of copper oxide. And our grams here are canceling out, Leaving us with 0. moles of copper oxide. Next we have 9.17 g of carbon monoxide. And we're going to multiply that by one mole of carbon monoxide over .01g of carbon monoxide and our grams of carbon monoxide are going to cancel out. And that's going to leave us with 0.35- moles of carbon monoxide. And for our next step, we want to take our lowest number of moles, which is our 0.1980 and see how many moles of carbon monoxide we get. So we're going to have 0. moles of copper Times 1. 3 moles of carbon monoxide over two moles of copper Times are molar mass of carbon monoxide. So 28.01 g of carbon monoxide over one mole. So our moles of copper are canceling out, and our moles of carbon monoxide are canceling out, and that gives us 8. 1897 grams of carbon monoxide. And our last step is to take our 9.87 g -R 8. 1897, And that equals 1.55 g of carbon monoxide. So our answer here is B. Thank you for watching. Bye.

Ch.4 - Chemical Quantities & Aqueous Reactions

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Tro 4th Edition

Ch.4 - Chemical Quantities & Aqueous Reactions

Problem 48

Chapter 4, Problem 48

Elemental phosphorus reacts with chlorine gas according to the equation: P₄(s) + 6 Cl₂( g) → 4 PCl₃(l) A reaction mixture initially contains 45.69 g P₄ and 131.3 g Cl₂. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

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Determine the molar mass of P_4 and Cl_2 using the periodic table.

Convert the given masses of P_4 and Cl_2 to moles by dividing by their respective molar masses.

Use the balanced chemical equation to find the mole ratio between P_4 and Cl_2, which is 1:6.

Calculate the theoretical moles of Cl_2 needed to completely react with the available moles of P_4.

Compare the available moles of Cl_2 to the theoretical moles needed to identify the limiting reactant and calculate the remaining moles of the excess reactant.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the proportions of substances consumed and produced, which is essential for identifying limiting and excess reactants in a reaction.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is crucial for calculating how much of the excess reactant remains after the reaction.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is used to convert between the mass of a substance and the number of moles, which is necessary for stoichiometric calculations in chemical reactions.

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Iron(III) oxide reacts with carbon monoxide according to the equation: Fe₂O₃(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g) A reaction mixture initially contains 22.55 g Fe₂O₃ and 14.78 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

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Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is: 2 Mg(s) + O₂(g) → 2 MgO(s) When 10.1 g of Mg reacts with 10.5 g O₂, 11.9 g MgO is collected. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.

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Urea (CH₄N₂O) is a common fertilizer that is synthesized by the reaction of ammonia (NH₃) with carbon dioxide: 2 NH₃(aq) + CO₂(aq) → CH₄N₂O(aq) + H₂O(l) In an industrial synthesis of urea, a chemist combines 136.4 kg of ammonia with 211.4 kg of carbon dioxide and obtains 168.4 kg of urea. Determine the limiting reactant, theoretical yield of urea, and percent yield for the reaction.

Elemental phosphorus reacts with chlorine gas according to the equation: P4(s) + 6 Cl2( g) → 4 PCl3(l) A reaction mixture initially contains 45.69 g P4 and 131.3 g Cl2. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

Verified video answer for a similar problem:

Key Concepts

Stoichiometry

Limiting Reactant

Molar Mass

Elemental phosphorus reacts with chlorine gas according to the equation: P₄(s) + 6 Cl₂( g) → 4 PCl₃(l) A reaction mixture initially contains 45.69 g P₄ and 131.3 g Cl₂. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?