1. ts) Balance all of the chemical reactions performed in this lab. a. Cu (s) + HNO, (aq) → Cu(NO) (aq) + NO₂ (g)+ H₂O (1) b. Cu(NO₂)2 (aq) + NaOH (og) → Cu(OH), (s) NaNO, (aq) c. Cu(OH): (s) → CuO (s) + H₂O (1) d. CuO (s) + H₂SO. (aq) → CuSO. (aq) + H₂O (1) e. CuSO₂ (aq) + Zn (s) Cu (s) + ZnSO₂ (aq)
1. ts) Balance all of the chemical reactions performed in this lab. a. Cu (s) + HNO, (aq) → Cu(NO) (aq) + NO₂ (g)+ H₂O (1) b. Cu(NO₂)2 (aq) + NaOH (og) → Cu(OH), (s) NaNO, (aq) c. Cu(OH): (s) → CuO (s) + H₂O (1) d. CuO (s) + H₂SO. (aq) → CuSO. (aq) + H₂O (1) e. CuSO₂ (aq) + Zn (s) Cu (s) + ZnSO₂ (aq)
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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Question
![1.
2.
3.
Chemical Transformations of Copper
PRESTUDY
ts) Balance all of the chemical reactions performed in this lab.
a. Cu (s) + HNO₂ (aq) → Cu(NO₂)2 (aq) + NO₂ (g) + H₂O (1)
b. Cu(NO₂)2 (aq) + NaOH (aq) → Cu(OH), (s) + NaNO, (aq)
c. Cu(OH)₂ (s) → CuO (s) + H₂O (1)
d. CuO (s) + H₂SO4 (aq) → CuSO. (aq) + H₂O (1)
e. CuSO. (aq) + Zn (s) → Cu (s) + ZnSO₂ (aq)
) Classify the reactions b, c, and e from above.
A student performs the experiment detailed in this lab. The student starts with 0.085 g of
copper wire. Referring to the balanced chemical equations in question one and applying
stoichiometric princples, answer the following questions. For full credit show a clear, concise set-
up and calculation.
a. How many moles of copper wire does the student have?
b. How many moles of copper(II) nitrate will the student produce?
c. How many moles of copper(II) hydroxide will the student produce?
d. How many moles of copper(II)oxide will the student produce?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F54779e31-9f51-4ea7-b33e-96294f7c4cb4%2F01049259-b417-4323-87ef-713a89733a79%2Fq578dja_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1.
2.
3.
Chemical Transformations of Copper
PRESTUDY
ts) Balance all of the chemical reactions performed in this lab.
a. Cu (s) + HNO₂ (aq) → Cu(NO₂)2 (aq) + NO₂ (g) + H₂O (1)
b. Cu(NO₂)2 (aq) + NaOH (aq) → Cu(OH), (s) + NaNO, (aq)
c. Cu(OH)₂ (s) → CuO (s) + H₂O (1)
d. CuO (s) + H₂SO4 (aq) → CuSO. (aq) + H₂O (1)
e. CuSO. (aq) + Zn (s) → Cu (s) + ZnSO₂ (aq)
) Classify the reactions b, c, and e from above.
A student performs the experiment detailed in this lab. The student starts with 0.085 g of
copper wire. Referring to the balanced chemical equations in question one and applying
stoichiometric princples, answer the following questions. For full credit show a clear, concise set-
up and calculation.
a. How many moles of copper wire does the student have?
b. How many moles of copper(II) nitrate will the student produce?
c. How many moles of copper(II) hydroxide will the student produce?
d. How many moles of copper(II)oxide will the student produce?
![YOUT23RA
e. How any moles of copper(II) sulfate will the student produce?
(WEN)
f. How many moles of zinc metal does the student need to react completely with the
copper(II) sulfate?
(60) 020 € (pol.
g. How many grams of zinc metal does the student need to react completely with the
copper(II) sulfate?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F54779e31-9f51-4ea7-b33e-96294f7c4cb4%2F01049259-b417-4323-87ef-713a89733a79%2Fh5z4nxr_processed.jpeg&w=3840&q=75)
Transcribed Image Text:YOUT23RA
e. How any moles of copper(II) sulfate will the student produce?
(WEN)
f. How many moles of zinc metal does the student need to react completely with the
copper(II) sulfate?
(60) 020 € (pol.
g. How many grams of zinc metal does the student need to react completely with the
copper(II) sulfate?
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