A chemist attempted the reaction below using 35.5 grams of Zn and more than enough HCl. What was...
Question:
A chemist attempted the reaction below using 35.5 grams of {eq}Zn {/eq} and more than enough {eq}HCl {/eq}. What was their percent yield if they only recovered 6.50 grams of {eq}ZnCl_2 {/eq}?
{eq}Zn + HCl \to ZnCl_2 + H_2 {/eq}
Percent Yield:
The percent yield or reaction yield of a chemical reaction is calculated based on the relationship of the quantity of the products of the reaction as compared to the theoretical yield. Understanding the output of a reaction is important in commercially important reactions so that they can be optimized for maximum output and efficiency of the reaction.
Answer and Explanation:
Become a Study.com member to unlock this answer! Create your account
View this answerBalancing the equation:
Zn + 2HCl -> ZnCl2 + H2
There should be a ratio of 1:1 for Zn metal being converted to ZnCl2 if the reaction goes to...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
How to Calculate Percent Yield: Definition, Formula & Example
from
Chapter 10 / Lesson 15
330K
What is percent yield? Learn the definition and formula of percent yield. Learn about actual and theoretical yields. See examples of percent yield calculations.
Related to this Question
- If 2.5 moles of zinc react with 6.0 moles of hydrochloric acid in the equation Zn + 2HCl = ZnCl2 + H2, what is the limiting reactant?
- Calculate the mass of Ag produced when 3.22 g of Zn reacts with 4.35 g of AgNO3 according to the following equation. Zn (s) + 2 AgNO3 (aq) arrow 2 Ag (s) + Zn(NO3)2 (aq).
- If 32 grams of MgCl2 react. How many grams of HCl will be formed in the reaction? H2SO4 + MgCl2 -> 2 HCl + MgSO4
- Consider the reaction: Pb(SO4)2 + 2Zn arrow 2ZnSO4 + Pb. If 0.542 moles of zinc reacts with excess lead(IV) sulfate, how many grams of zinc sulfate will be produced in the reaction?
- If you start with 16 grams of N_2 and 8 grams of H_2, what will be the limiting reagent and the theoretical yield? If 12 grams of the product were formed what would be the percent yield? The reaction is: N_2 + 3H_ 2 to 2NH_3
- How many grams of Zinc would be required to synthesize 5.0 grams of Zinc sulfate in the following reaction? Zn(s) + CuSO4(s) rightarrow Cu(s) + ZnSO4(s)
- Consider the following reaction: 2Li (s) + ZnCl_2 (aq) \to Zn (s) + 2LiCl (aq) a. How many grams of lithium are needed to completely react with 22.45 grams of zinc chloride? b. How many grams of zinc can be made if we have 82.3 grams of lithium
- Hydrochloric acid can be prepared using the reaction described by the chemical equation: 2NaCl(s) + H2SO4(l) 2HCl(g) + Na2SO4(s). How many grams of HCl can be prepared from 393 g of H2SO4 and 4.00 moles of NaCl? a) 4.00 g b) 2.49 g c) 146 g d) 284 g e) No
- In a reaction to produce sulfuric acid, the theoretical yield is 300g. What is the percent yield if the actual yield is 280g?
- What is the percent yield for a reaction in which 342g of a product is actually produced when the theoretical yield is 400g?
- Given the equation HCL + NaOH = NaCl + H2O what is the percent yield if you measured 12 gams of H20? You started with 108 grams of HCL and 80 grams of NaOH.
- Zn + Cl_{2} \rightarrow ZnCl_{2} Identify the reactant that is oxidized and the reactant that is reduced.
- Consider the following reaction: Zn(s) + 2HCl(aq) arrow ZnCl2(aq) + H2(g). If 15.00 g of solid zinc reacts with 100.0 mL of 4.00 M hydrochloric acid, what volume of hydrogen gas will be produced at 25 degrees Celsius and 1.00 atm?
- A reaction is known to have a percent yield of 65.3%. If stoichiometric calculations indicate that a chemist should receive 45.0 g of a product, how much will the reaction actually produce?
- What mass of HCl is consumed by the reaction of 2.50 moles of magnesium? Mg + HCl arrow MgCl2 + H2
- In a particular reaction between copper metal and silver nitrate, 12.7g Cu produced 3.81g Ag. What is the percent yield of silver in this reaction? Cu+2AgNO3 yields Cu(NO3)2+2Ag
- 3H_2+N_2 \rightarrow NH_3 1.09 g of H_2 reacts with 10.3 g N2 to produce 1.29 g NH_3 What is the theoretical yield in grams. What is the percent yield.
- Suppose 9.0 grams of aluminum were reacted with an excess of chlorine according to the following reaction, and 20.0 grams of Al2Cl6 were actually formed. What was the percentage yield for this experiment? 2Al + 3Cl2 arrow Al2Cl6
- Consider the reaction between HCl and O_2: 4HCl_{(g)} + O_{2(g)} \to 2H_2O_{(l)} + 2Cl_{2 (g)} When 63.1 g of HCl are allowed to react with 17.2 g of O_2, 42.0 g of Cl_2 are collected. Determine the theoretical yield of Cl_2 for this reaction.
- Zinc and sulfur react to form zinc sulfide. If 8.00 grams of zinc and 8.00 grams of sulfur are available for this reaction, calculate the mass of zinc sulfide that will be produced.
- If 2.0 grams of CuCl2 reacts with excess NaNO3, what mass of NaCl is formed? CuCl2 + 2NaNO3 arrow Cu(NO3)2 + 2NaCl
- How do you find the theoretical yield and percent yield for a reaction?
- Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: \\ Zn(s) + 2HCl(aq) \rightarrow ZnCl_2(aq) + H_2(g) \\ The product gas, H_2 is collected over water at a temperature of 20^\circ C and a pressure
- When 1.34 g Zn (s) reacts with 60.0 mL of 0.750 M HCl (aq), 3.14 kJ of heat are produced. Determine the enthalpy change per mole of zinc reacting for the reaction: Zn (s) + 2 HCl (aq) \rightarrow ZnCl_{2} (aq) + H_{2} (g)
- Which of the following displacement reactions does not occur? a. Cl2 + 2KBr arrow 2KCl + Br2 b. TiCl4 + 2Mg arrow Ti + 2MgCl2 c. Pb + 2H2O arrow Pb(OH)2 + H2 d. Zn + 2HCl arrow ZnCl2 + H2
- In the following reaction, 80.0 mL of 2.0 M HCl would react with how many grams of aluminum? 2Al(s) + 6HCl(aq) arrow 2AlCl3(aq) + 3H2(g)
- Determine whether or not the following reaction is a single displacement reaction. Br2 + ZnCl2 arrow Cl2 + ZnBr2
- When 48.2 g of KClO_3 is completely decomposed, 1) what is the theoretical yield, in grams, of O_2? Show your calculation process and express the answer with the appropriate units. 2) If 11.9 g of O_2 is produced, what is the percent yield of O_2? Express
- How many moles of HCl are produced when 75.1 grams of AlCl3 reacts with excess H2SO4? 2AlCl3 + 3H2SO4 arrow Al2(SO4)3 + 6HCl
- Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: Zn(s) + 2HCl(aq) to ZnCl2(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 20 deg C and a pressure of 755 mm Hg. If th
- What is the percent yield of a chemical reaction?
- If 0.315 g of Al (26.982 g/mol) is reacted in the synthesis of Alum reaction and 3.265 g of Alum (474.39 g/mol) is produced, determine the percent yield. a. 60% b. 58% c. 57% d. 55% e. 59% f. 56%
- Suppose a 7.95 g sample of AgNO3(s) is reacted with a solution of BaCl2(aq), and 5.25 g of precipitate is collected. Calculate the percentage yield for this reaction.
- If the mass % of ZnCl2 is 25% in a solution, find the mole fraction of ZnCl2 in the solution.
- A student performs the following lead extraction to test the stoichiometric method and to determine the efficiency of the reaction. In the reaction 49.5 g of lead(II) nitrate is reacted with excess zinc in a single displacement reaction. Calculate the the
- Using the equation C_6H_6+Cl_2 \to C_6H_5Cl+HCl, what is the theoretical yield of C_6H_5Cl if 91.2 g of C_6H_6 react?
- 5g of CaO react with excess H2O. 6.11g of Ca(OH)2 is recovered. The theoretical yield is 0.089 mole of Ca(OH)2. What is the percent yield?
- C6H6 + Br2 rightarrow C6H5Br + HBr If the actual yield of bromobenzene is 63.25 g, what is the percent yield of bromobenzene?
- If 15.00 mL of a 1.00 M HCl solution is mixed with 25.00 mL of a 0.250 M NaOH solution in a process that produces 273 mg of NaCl, what is the percentage yield of NaCl?
- Zinc and sulfur react to form zinc sulfide, as shown in the following balanced chemical equation: Zn + S arrow ZnS If 8.00 g of zinc and 8.00 g of sulfur are available for this reaction, the limiting reagent will be: a. zinc b. sulfur c. zinc sulfide d. b
- Calculate the percent yield for the following reaction. If 233g of NO_{2} reacted and 175g of HNO_{3} were produced. 3NO_{2} + H_{2}O \rightarrow 2HNO_{3} + NO
- Consider the following: SCl4 + H2O \rightarrow SO2 + HCl a) Balance this reaction. b) How many grams of water is needed to react if 5.00 g of SCl4 is present?
- Calculate the percent composition of ZnCl2.
- Zinc (Zn) is a silvery metal that is used in making brass (with copper) and in plating iron to prevent corrosion. How many grams of Zn are in 0.356 moles of Zn?
- 8.7X10^24 H2 molecules are produced by the reaction of zinc and 30%W/W H_2SO_4 solution of density 1.25g/ cm3. For the reaction: Zn(s) +H_2SO_4(aq) H_2(g) + ZnSO_4(s) Calculate the volume of sulphuric acid solution used. (Zn = 65, O = 16, S = 3
- How many grams of chromium are needed to react with an excess of CuSO4 to produce 127.0g Cu? 2Cr(s)+3CuSO4(aq) yields Cr2(SO4)3(aq)+3Cu(s)
- What mass of HCl is produced when 3.00 mol of H_2 reacts completely in the following equation? H_2 + Cl_2 rightarrow 2 HCl
- Consider the reaction of 18.0 g of zinc with excess silver nitrite to produce silver metal and zinc nitrite. The reaction is stopped before all the zinc metal has reacted and 33.0 g of solid metal is present. Calculate the mass of each metal in the 33.0-
- Calculate the percent yield for the reaction below if 75.0 g of phosphorous reacts with 345 g of chlorine to produce 111.0 g of phosphorous trichloride. P4(s) + 6Cl2(g) arrow 4PCl3(l)
- In a lab, you reacted 3.0 g of sodium carbonate with 0.03 mol of hydrochloric acid. a) Write a balanced equation for the reaction. b) Calculate the mass of the gas that should be produced (the theoretical yield).
- What is the maximum percent yield in any reaction?
- 2Na + Cl2 \rightarrow 2NaCl If 15 mol of Na reacts with 15 mol Cl2, what is the theoretical yield of NaCl that could be formed?
- How many grams of Cl_2 can be prepared from the reaction of 16.0 g of MnO_2 and 30.0 g of HCl according to the following balanced chemical equation? MnO_2 + 4HCl to MnCl_2 + Cl_2 + 2H_2O a) 6.52 g b) 7.29 g c) 13.0 g d) 14.6 g e) 58.4 g
- For the following balanced equation, indicate how many moles and grams of each reactant and product are needed/produced in the reaction if 10.0 grams of FeS2 reacts. 4FeS2 + 11O2 arrow 2Fe2O3 + 8SO2
- Calculate the theoretical yield of AlCl3 when 15.0 g of Al reacts with 55.0 g of Cl2 in the reaction below. 2 Al (s) + 3 Cl2 (g) arrow 2 AlCl3 (s).
- For the reaction, CaCO3(s)+2HCl(aq) yields CaCl2(aq)+CO2(g)+H2O(l). Calculate the mass of CaCl2 that can be obtained if 115g of CaCO3 and 80.36g of HCl resulted in a 100% yield of CaCl2. Molar mass: CaCO3=100.09g mol-1; HCl=36.46g mol-1; CaCl2=110.98g mol
- If you start with 50.3 grams of Al(OH)3 and you isolate 39.5 grams of AlCl3, what is the percent yield? Al(OH)3(s) + 3HCl(aq) arrow AlCl3(aq) + 3H2O(l)
- The reaction listed below can be used to prepare small quantities of Cl2 gas. If a 85.2 g sample that is 86.5% K2Cr2O7(aq) by mass is allowed to react with 153 mL HCl(aq) with a density of 1.15 g/mL and 28.4% HCl by mass, how many grams of Cl2 will be pr
- Given the following balanced equation for the reaction of zinc with nitric acid, 4Zn(s)+10HNO3(aq) yields 4Zn(NO3)2(aq)+NH4NO3(aq)+3H2O(l). How many moles of nitric acid would be required to react with 87g of zinc? What mass of ammonium nitrate would be p
- How do you calculate percentage yield of a chemical reaction?
- If 12g of P react with 35g of Cl2, what is the limiting reactant, what is the theoretical yield of PCl3, if only 42.4 g of PCl3 are formed what is the percent yield, and how much excess of the reactant is left?
- For the following reaction refer to the activity series. Determine whether the following equation can occur. If the reaction occurs, write the complete, balanced equation. If the reaction does not occur, explain why. Reaction: Zinc plus sulfuric acid
- What is the limiting reactant in the reaction between 0.86 g copper and 1.5 g silver nitrate, and how many grams would be left over?
- What is the percent yield if 5.5 g Mg are recovered after burning 4.9 g Mg in sufficient O?
- Suppose 7 grams of aluminum metal is reacted with 11 grams of hydrogen sulfate and produces 3.4 grams of aluminum sulfate and hydrogen gas. Calculate the percent yield of this reaction.
- How many moles of Zn are present in 3.52 L of a 6.20 molal (m) solution of ZnCl2 with a density of 1.12 g/mL?
- In the following chemical reaction between H_2 and Cl_2 to produce HCl, what is the sum of the mass of HCl produced plus the mass of left over reactants when 3.21E - 1 g of H_2 completely reacts with 1.247E + 1 g of Cl_2?
- 150 g of C_7H_6O_3 reacts with 11.20 g of methanol (CH_3OH). The yield of C_8H_8O_3 is 1.31 g. What is the percentage yield?
- How many moles of silver chloride are produced when 8.50 g of MgCl2 reacts with silver nitrate?
- The equation for the decomposition of potassium chlorate is written as: 2KClO3(s) to 2KCl(s) + 3O2(g) When 48.2 g of KClO3 is completely decomposed, what is the theoretical yield, in grams, of O2?
- Reaction: Aluminum chloride is mixed with Hydrogen gas to produce Hydrochloric acid and Aluminum metal. If you are given 5 grams of Hydrogen and 50 grams of Aluminum chloride, how many grams of Aluminum can be produced if the reaction is 35% efficient? a.
- How many grams of K2S2O3 are needed to react with 2.0 moles of chlorine gas in the following reaction? K2S2O3 + 4Cl2 + 5H2O arrow 2KHSO4 + 8HCl
- If 1.0 gram of Nb_2O_5 is reacted with 10.0 grams of NbC, what mass of niobium is formed in the following reaction? Nb_2O_5(s) + 5NbC(s) \to 7Nb(s) + 5CO(g)
- For the balanced equation shown below, what would be the limiting reagent if 51.9 grams of Cu reacted with 17.6 grams of S? 2Cu + S arrow Cu2S
- Combining 0.251 moles of Fe2O3 with excess carbon produced 181 grams of Fe. Fe2O3 + 3C arrow 2Fe + 3CO a. What is the actual yield of iron in moles? b. What is the theoretical yield of iron in moles? c. What is the percent yield?
- How many grams of copper are required to completely react 200 \ g of sliver nitrate, and how many grams of sliver is produced then? 2AgNO_3 + Cu \to Cu(NO_3)_2 + Ag
- Calculate the mass of hydrogen produced in the following reaction when 5 grams of calcium reacts with an excess of dilute sulfuric acid. Ca + H2SO4 arrow CaSO4 + H2
- A sample of 8.5g NH3 on oxidation produces 4.5g of NO. Calculate the percent yield. Reaction: 4NH3 + 5O2 = 4NO + 6H2O
- For the following reaction, 13.1 grams of chlorine gas are allowed to react with 8.10 grams of water to produce hydrochloric acid and chloric acid. What is the maximum amount of hydrochloric acid that
- Metallic copper is formed when aluminum reacts with copper (II) sulfate. What is the theoretical yield of copper if 54.0 g of Al react with excess CuSO_4? Given the equation for reaction is 2Al + 3CuSO_4 \to Al_2(SO_4)_3+ 3Cu.
- 2HCl + Ca(OH)_2 rightarrow CaCl_2 + 2H_2O How many grams of calcium hydroxide, Ca(OH)_2, are needed to react completely with 82.9 g of hydrochloric acid, HCl?
- You generate hydrogen gas by reacting zinc with HCl to produce hydrogen gas and zinc dichloride. You collect the hydrogen gas in an evacuated container with a volume of 3.0 L. If you start with 6.0 gr
- What is the total number of grams of O2(g) needed to react completely with 0.50 moles of C2H2(g) for the balanced equation below? 2C2H2(g) + 5O2(g) arrow 4CO2(g) + 2H2O(g)
- How many grams of the excess reactant remain assuming the reaction goes to completion and started with 15.5 g of Na2S and 12.1 g of CuSO4?
- What is the calculated yield of ammonia in the following reaction if 0.0500 grams of hydrogen reacts completely? N2(g) + 3H2(g) arrow 2NH3(g)
- Use the equation: Zn + H2SO4 to ZnSO4 + H2S + H2, to find out which element is oxidized, which element is reduced and give the number of electrons gained or lost by each atom.
- How many mL of a 0.75 M HCl solution would just react with 4 grams of Ba(OH)2? 2HCl + Ba(OH)2 arrow BaCl2 + 2H2O
- The reaction below shows how silver chloride can be synthesized. AgNO3 + NaCl \rightarrow NaNO3 + AgCl How many moles of silver chloride are produced from 15.0 mol of silver nitrate?
- Silver chloride is one of the products of the double displacement reaction between magnesium chloride and silver nitrate. How many moles of silver chloride are produced when 8.50 g of MgCl2 reacts with silver nitrate?
- MgCl2(aq)+2HCl(aq) yields MgCl2(aq)+H2(g) a. How many mL of a 6.00M HCl solution are required to react with 15.0g magnesium? a. How many grams of hydrogen gas can form when 0.500L of 2.00M HCl reacts with excess magnesium?
- How many grams would 0.567 moles of zinc weigh?
- Magnesium and hydrochloric acid react according to the equation below : Mg(s)+2HCl(aq)\rightarrow MgCl_2(aq)+H_2(g) If 1.0g of Mg is reacted with 10.0 mL of 6.0 M HCl, what volume of hydrogen has will
- How many mL of 2.83 M HCl will be needed to completely neutralize 12.737 grams of Ca(OH)_{2(s)}?
- Consider the reaction between hydrochloric acid and zinc. How will increasing the temperature affect the rate of the reaction? Explain in detail.
- What is the chemical equation for the reaction between zinc carbonate and sulfuric acid?
- If 12.8 \ mL of NO_2 is measured at STP, is allowed to react with 14.9 \ g water, find the limiting reagent and the theoretical yield of HNO_3 in grams.
- How many grams of Cl_2 were used in the following reaction, if 10.0 grams of KCl were produced? (2K + Cl_2 \to 2KCl)
- How much of the excess reactant (in grams) remains after the reaction has gone to completion?
- Calculate the percent yield for the reaction if 75.0 g of phosphorus reacts with excess chlorine gas to produce 111.0 g of phosphorus trichloride.
Explore our homework questions and answers library
Browse
by subject