Part AWhen ethane (C2H6) reacts with chlorine (Cl2).the main product is C,H;Cl; but other productscontaining Cl, such as C,H4C12, are alsoobtained in small quantities. The formation of theseother products reduces the yield of C,H;Cl.Calculate the theoretical yield of C2H;Cl when 140 g of C2H6 reacts with 228 g of Cl2, assumingthat C2 H6 and Cl, react only to form C2H;Cl and HCI.ΑΣφ?m =gSubmitPrevious Answers Request AnswerX Incorrect; Try Again; 5 attempts remainingReview your calculations and make sure you round to 3 significant figures in the last step.Part BCalculate the percent yield of C2 H;Cl if the reaction produces 179 g of C2H;Cl.Πνα ΑΣφ?percent yield =%SubmitRequest Answer< Return to AssignmentProvide FeedbackP Pearson

Answered: Image /qna-images/answer/5c9c33a4-5b0c-4ba9-933e-c3719d073bfe.jpg

Part A Calculate the theoretical yield of C,H;Cl when 140 g of C,Hs reacts with 228 g of Cl2, assuming that C, H6 and Cl2 react only to form C2H;Cl and HCI. ? m= g Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining Review your calculations and make sure you round to 3 significant figures in the last step. Part B Calculate the percent yield of C,H;Cl if the reaction produces 179 g of C,H;CI. ? percent yield = % Submit Request Answer

Part A Calculate the theoretical yield of C,H;Cl when 140 g of C,Hs reacts with 228 g of Cl2, assuming that C, H6 and Cl2 react only to form C2H;Cl and HCI. ? m= g Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining Review your calculations and make sure you round to 3 significant figures in the last step. Part B Calculate the percent yield of C,H;Cl if the reaction produces 179 g of C,H;CI. ? percent yield = % Submit Request Answer

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

If the theoretical yield of H20 in the reaction is 49.3 grams, and 16 grams are actually produced, what is the % yield of H2O? 2 H2 + O2 --> 2 H2O Round your answer to 2 decimal places.
Mercury can be isolated from its ore by the reaction: 4 HgS + CaO --> 4 Hg + 3 CaS + CaSO4 a- How many Kilograms of Hg are produced along with 9.75 mol of CaSO4? b- How many Kilograms of CaS are produced along with 9.25 kg of Hg?
Iron reacts with oxygen at high temperatures to form iron(III) oxide. 4 Fe(s) + 30,(g) 2 Fe,0,(s) Suppose 17.2 g of iron (Fe) is reacted with 16.6 g of oxygen (0,). Select the limiting reagent. O2 Fe O Fe,O, Calculate the theoretical yield of iron(II) oxide (Fe, O,). 3 ald
(b) When 20.0 g of Fe and 40.0 g of CUSO4 are reacted, what is the limiting reactant and how many grams of each species will be present? limiting reactant: O Fe O CUSO4 O no limiting reactant i ! g Cu !g FeSO4 i !g excess reactant
Q.1: If 42.1 g of C4H10 0 react with 73.0 g of 02 according to the reaction Equation : C4H10 0 + 02 CO2 + H20 a) Write the balanced equation for the reaction. b) Determine the moles of given reactants b) Find the limiting reagent, c) calculate the mass of CO2 formed, d) If the actual yield of CO2 is 55.8 g, what is the percent yield? Given that: C= 12 g/ mol. , 0 = 16 g/ mol., : H = 1 g/ mol.
Please refer to the image i need this done asap pleaseeee show the work
aqueous sulfuric acid (H_{2}*S*O_{4}) reacts with solid sodium hydroxide ( ) to produce aqueous sodium sulfate (N*a_{2}*S*O_{4}) and liquid water (H_{2}*O). If 0.384 g of sodium sulfate is produced from the reaction of 0.98 g of sulfuric acid and 0.36 g of sodium hydroxide , calculate the percent yield of sodium sulfate Round your answer to 2 significant figures.
Using the following reaction, complete the following questions. Show all your work. NaCl + Ba3(PO4)2 ---> Na3PO4 + BaCl2 At the start of this reaction, 5 g of sodium chloride reacts with 2.7 g of barium phosphate. a) Which reactant is the limiting reagent? b) How many grams of barium chloride will be produced? c) At the end of the experiment, 0.20 g of barium chloride was collected. What was the percent yield?
Q.1: If 42.1 g of C4H10 0 react with 73.0 g of 02 according to the reaction Equation : C4H10 0 + 02 CO2 + H20 a) Write the balanced equation for the reaction. b) Determine the moles of given reactants b) Find the limiting reagent, c) calculate the mass of C02 formed, d) If the actual yield of CO2 is 55.8 g, what is the percent yield? Given that: C= 12 g/ mol. , O = 16 g/ mol., : H = 1 g/ mol.