A student performed the five step reaction to produce copper (I) chloride as outlined in the CHM 125 lab manual. The following reactions were performed: Cu(s) + 4 HNO3(aq) → Cu(NO3)2 (aq) + 2NO2 (g) + 2 H2O (l) 2 HNO3(aq) + Na2CO3 (s) → H2O (l) + CO2 (g) + 2 NaNO3 (aq) Cu(NO3)2(aq) + Na2CO3 (s) → CuCO3 (s) + 2NaNO3 (aq) CuCO3(s) + 2 HCl (aq) → CuCl2 (aq) + H2O(l ) + CO2 (g) CuCl2(aq) + Cu (s) → 2 CuCl (s) The student weighed out 1.245 g of Cu (s) and added 5.3 mL of 15.8 M nitric acid. The student then added 3.911 g of Na2CO3 (s) to the mixture to carry out reactions 2 and 3 at the same time. Based on this information and the reactions 1-5 answer the following questions: a.Using equation 1 calculate the total number of moles of HNO3 added. Next calculate how many moles of HNO3 were added in excess Based on the moles of HNO3 calculated in the previous step and also the number of moles of Cu(NO3)2 produced in reaction 1 calculate the total mass of Na2CO3 needed for steps 2 and 3. Was the amount of Na2CO3 added in excess or was it inadequate? By how much was it in excess or limited?

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...

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A student performed the five step reaction to produce copper (I) chloride as outlined in the CHM 125 lab manual. The following reactions were performed:

Cu(s) + 4 HNO₃(aq) → Cu(NO₃)₂ (aq) + 2NO₂ (g) + 2 H₂O (l)
2 HNO₃(aq) + Na₂CO₃ (s) → H₂O (l) + CO₂ (g) + 2 NaNO₃ (aq)
Cu(NO₃)₂(aq) + Na₂CO₃ (s) → CuCO₃ (s) + 2NaNO₃ (aq)
CuCO₃(s) + 2 HCl (aq) → CuCl₂ (aq) + H₂O(l ) + CO₂ (g)
CuCl₂(aq) + Cu (s) → 2 CuCl (s)

The student weighed out 1.245 g of Cu (s) and added 5.3 mL of 15.8 M nitric acid. The student then added 3.911 g of Na₂CO₃ (s) to the mixture to carry out reactions 2 and 3 at the same time. Based on this information and the reactions 1-5 answer the following questions:

a.Using equation 1 calculate the total number of moles of HNO₃ added. Next calculate how many moles of HNO₃ were added in excess

Based on the moles of HNO₃ calculated in the previous step and also the number of moles of Cu(NO₃)₂ produced in reaction 1 calculate the total mass of Na₂CO₃ needed for steps 2 and 3. Was the amount of Na₂CO₃ added in excess or was it inadequate? By how much was it in excess or limited?

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