according to balanced reaction
12 g C reacts with 143.1 g Cu2O
11.5 g C reacts with 11.5 x 143.1 / 12 = 137.14 g Cu2O
but we have 114.5 g Cu2O
so Cu2O is limiting reagent.
143.1 gCu2O forms 2 x 63.55 g
114.5 g Cu2O forms 114.5 x 2 x 63.55 / 143.1 = 101.7 g Cu
therotical yield = 101.7 g
actual yield = 87.4 g
% yield = (87.4 / 101.7) x 100
% yield = 85.94
Part 4 Consider the reaction: Cu_2O(s) + C(s) rightarrow 2 Cu (s) + CO(g) When 11.5...
How was 23 chosen as the actual value for the percentage
yield?
2. For the reaction: Cu2O(s) + C(s) 2 Cu(s) + CO(g) When 11.5 mol of Care allowed to react with 145 mol of Cu20 10.0 mol of Cu are obtained. Determine (a) the limiting reactant and the theoretical yield of copper, and then (b) the percent yield. Show the equation for percent yield first and then include the values in this equation and solve. Xtremting Reactant - amal...
Consider the reaction between HCl and O2: 4HCl(g)+O2(g)→2H2O(l)+2Cl2(g) When 63.1 gof HCl are allowed to react with 17.2 g of O2, 56.3 g of Cl2are collected. Part A: Determine the limiting reactant for the reaction. Express your answer as a chemical formula. Part B: Determine the theoretical yield of Cl2 for the reaction. Part C: Determine the percent yield for the reaction.
Consider the following redox reaction: Al(s) + Fe_2O_3 rightarrow Al_2O_3(s) + Fe(l) a. Determine the mass of Fe(l) that is produced when 500.0 g of aluminum reacts with an excess of iron (III) oxide b. Determine the mass of Fe(l) that is produced when 500.0 g of iron (III) oxide reacts with an excess of aluminum c. If 500.0 g Fe_2O_3 is allowed to react with 500.0 g Al, what is the limiting reactant? d. What is the theoretical yield...
need a-g
LAB VII. PRACTICE PROBLEMS NAME: SECTION: PART D. CHAPTER 4 PROBLEMS I) Reaction Stoichiometry, Limiting Reactant, Theoretical and Percent Yields a) For the equation Cu + C → Cu + Co, if 2.73 moles of C are reacted with an excess of Cu20, how many moles of CO would be produced? moles b) For the equation Co(NO3)3 + (NH4)2S → Co2S3 + NH4NO3, if 79.2 g of Co(NO3)3 are reacted with an excess of (NH4)2S, how many moles...
LAB VIL PRACTICE PROBLEMS NAME: SECTION: PART D. CHAPTER 4 PROBLEMS 1) Reaction Stoichiometry, Limiting Reactant, Theoretical and Percent Yields For the equation Cu + C > Cu + CO, if 2.73 moles of Care reacted with an excess of Cuzo, how many moles of CO would be produced? moles b) For the equation Co(NO) + (NH),S COS; + NH.NO, if 79.2 of CNO are reacted with an excess of (NH),S, how many moles of NH.NO, would be produced moles...
1. Consider the reaction: MnO2 (s) + 4 HCl (g)MnCl2 (s) + Cl2 (g) + 2 H20 (g) If 10.00 g of MnO2 and 10.00 g of HCl are reacted, how many grams of MnCl2 can be produced? Show all calculations 2. Consider the following unbalanced equation: NH4NOs(aq) + Na PO4(aq)(NH4)3PO4(aq NaNOs(aq) Assuming you start with 50.0 g of NHNOs and 50.0 g of NasPO4, which is the limiting reagent? What is the theoretical yield (g) of ammonium phosphate? a....
1. Consider the following reaction: 1.00 g 20.0 mL 6.00 M 14.0 g a) Which substance is the limiting reactant? b) What is the theoretical yield of the complex formed in the reaction? c) If 10.0 g of the complex was obtained from the reaction, what is the percent yield? 2. Draw the structures for the Al(C204)3 ion and the Cu(C204) ion
24 3 points Consider the reaction: Pa(s) + 6 H2() + 4 PH3(g) If 88.6 L of H2, measured at STP, is allowed to react with 158.3 g of P, which of the following are true? (select all that apply) Pe is the limiting reagent The theoretical yield is 48.3 L Hy is the limiting reagent The theoretical yield is 114L The theoretical yield is 59.1L The actual yield is 114 L
13. Consider 28 g O2 mixed with 4.8 g H2 according to this reaction: H2 + O2 = H2O a.) Balance the reaction? b.) Find the limiting reactant? c.) What is the theoretical yield (in grams)? d.) What is the percent yield if 3.4 g H2O are obtained?
4. Penny and Benedict used 0.510 g of Cu(s) in the initial reaction of this experiment. At the end of the experiment, they had obtained 0.384 g of Cu. a. What is their theoretical yield? b. What is their actual yield? c. What is their percent yield? Classifying Reactions in the Copper Cycle