2. A reaction container holds 5.45 g of P, and 5.45 g of Oz. The following reaction occurs: P, +50,- P,010 a. What is the limiting reagent? b. What is the theoretical yield in grams? c. What mass of reactant is left in the reaction container? d. What is the percent yield if 7.41 g of P,O1p are formed in the reaction?

2. A reaction container holds 5.45 g of P, and 5.45 g of Oz. The following reaction occurs: P, +50,- P,010 a. What is the limiting reagent? b. What is the theoretical yield in grams? c. What mass of reactant is left in the reaction container? d. What is the percent yield if 7.41 g of P,O1p are formed in the reaction?

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 71AP: When elemental copper is strongly heated with sulfur, a mixture of CuS and Cu2Sis produced. with CuS...

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What is meant by a limiting reactant in a particular reaction? In what way is the reaction “limited”? What does it mean to say that one or more of the reactants are present in excess? What happens to a reaction when the limiting reactant is used up?
Consider the equation: 2A+B5C. If 10.0 g of A reacts with 5.00 g of B. how is the limiting reactant determined? Choose the best answer and explain. l type='a'> Choose the reactant with the smallest coefficient in the balanced chemical equation. So in this case, the limiting reactant is B. Choose the reactant with the smallest mass given. So in this case, the limiting reactant is The mass of each reactant must be converted to moles and then compared to the ratios in the balanced chemical equation. So in this case, the limiting reactant cannot be determined without the molar masses of A and B. The mass of each reactant must he converted to moles first. The reactant with the fewest moles present is the limiting reactant. So in this case, the limiting reactant cannot be determined without the molar masses of A and B. The mass of each reactant must be divided by their coefficients in the balanced chemical equation, and the smallest number present is the limiting reactant. So in this case, there is no limiting reactant because A and B arc used up perfectly.
Consider the hypothetical reaction between A2 and AB pictured below. What is the balanced equation? lf 2.50 moles of A2 are reacted with excess AB, what amount (moles) of product will form? If the mass of AB is 30.0 u and the mass of A2 are 40.0 u, what is the mass of the product? If 15.0 g of AB is reacted, what mass of A2 is required to react with all of the AB, and what mass of product is formed?
4.33 Silicon carbide, an abrasive, is made by the reaction of silicon dioxide with graphite (solid carbon): SiO2+CSiC+CO(balanced?) We mix 150.0 g of SiO2 and 101.5 g of C. If the reaction proceeds as far as possible, which reactant is left over? How much of this reactant remains?
One mol of ammonia reacts with 1.00 mol of oxygen to form nitrogen oxide and water according to the reaction 4NH3(g)+5O2(g)4NO(g)+6H2O(l)State which statements are true about the reaction and make the false statements true. (a) All the oxygen is consumed. (b) 4.00 mol NO are produced. (c) 1.50 mol H2O are produced. (d) The description of the experiment does not provide enough information to determine percent yield. (e) Three moles of water are produced for every two moles of NO obtained.
When elemental copper is strongly heated with sulfur, a mixture of CuS and Cu2Sis produced. with CuS predominating. :math>Cu(s)+S(s)CuS(s)2Cu(s)+S(s)Cu2S(s) at is the theoretical yield of CuS when 31.8 g of Cu(s) is heated with 50.0 g of S? (Assume only CuS is produced in the reaction.) What is the percent yield of CuS if only 40.0 g of CuS can be isolated from the mixture?
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Freon-12, CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is HCl. Outline the steps needed to determine the percent yield of a reaction that produces 12.5 g of CCl2F2 from 32.9 g of Cd4. Freon-12 has been banned and is no longer used as a refrigerant because it catalyzes the decomposition of ozone and has a very long lifetime in the atmosphere. Determine the percent yield.
The following pictures show a molecular-scale view of a chemical reaction between the compounds AB2 and B2. (A at-oms are shown in blue and B atoms in white). The box on the left represents the box on the right shows what is left once the reaction has gone to completion. Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
When small quantities of elemental hydrogen gas are needed for laboratory work, the hydrogen is often generated by chemical reaction of a metal with acid. For example, tine reacts with hydrochloric acid, releasing gaseous elemental hydrogen: :math>Zn(s)+2HCI(aq)ZnCl2(aq)+H2(g) at mass of hydrogen gas is produced when 2.50 g of zinc is reacted with excess aqueous hydrochloride acid?
The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. D Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.