LUnt (IMrate ion), and then reduce the copper(II) ion to copper(I) by the te copper(II), remove the addition of excess copper metal. ono to n ovlo The chemical reactions you will carry out in this lab are shown below. 1) Cu(s) + 4HNO3(aq) → Cu(NO3)2(aq) + 2NO2(g) + 2H2O(1) 2il ed 2) 2HNO3(aq) + Na2CO3(s)→ H2O(1) ±ÇO2(g) + 2NaNO3(aq) 0. bay 3) Cu(NO3)2(aq) + NazCO3(s) → ÇUCO:(s) + 2NANO3(aq) 4) CUCO3() + 2HC((aq) CuCh9) + H2O@ + CO2«g) 12 5) CuC2(aq) + Cu(s) 2CUCI) BEPpe to anstmoo adi The reactions will be carried out in such a way that the copper metal added in the first reaction will determine the amount of copper(I) chloride that forms in the last reaction because it is the limiting reagent in all reactions where it's involved. In other words, all the other reagents used for this preparation will be added in excess. The theoretical yield is then based on the amount of copper added in the first reaction. 20 Calculations: cwoda 1n bluoda Theoretical yield = -g CuC) " mole CuCl 1 mole Cu 1 mole Cu(NO3)2 X. 1 mole CuCO3 1 mole CuCl2 2 mole CuCl -g Cu x - - g Cu 1 mole Cu 1 mole Cu(NO3)2 1 mole CuCO3 * 1 mole CuCl2 oLas 1st You need to fill in the molar masses of Cu and of CuCl. Experimental yield x 100 bouos a ni Tuqgo2 ucvoaroo bor 0%Yiel
LUnt (IMrate ion), and then reduce the copper(II) ion to copper(I) by the te copper(II), remove the addition of excess copper metal. ono to n ovlo The chemical reactions you will carry out in this lab are shown below. 1) Cu(s) + 4HNO3(aq) → Cu(NO3)2(aq) + 2NO2(g) + 2H2O(1) 2il ed 2) 2HNO3(aq) + Na2CO3(s)→ H2O(1) ±ÇO2(g) + 2NaNO3(aq) 0. bay 3) Cu(NO3)2(aq) + NazCO3(s) → ÇUCO:(s) + 2NANO3(aq) 4) CUCO3() + 2HC((aq) CuCh9) + H2O@ + CO2«g) 12 5) CuC2(aq) + Cu(s) 2CUCI) BEPpe to anstmoo adi The reactions will be carried out in such a way that the copper metal added in the first reaction will determine the amount of copper(I) chloride that forms in the last reaction because it is the limiting reagent in all reactions where it's involved. In other words, all the other reagents used for this preparation will be added in excess. The theoretical yield is then based on the amount of copper added in the first reaction. 20 Calculations: cwoda 1n bluoda Theoretical yield = -g CuC) " mole CuCl 1 mole Cu 1 mole Cu(NO3)2 X. 1 mole CuCO3 1 mole CuCl2 2 mole CuCl -g Cu x - - g Cu 1 mole Cu 1 mole Cu(NO3)2 1 mole CuCO3 * 1 mole CuCl2 oLas 1st You need to fill in the molar masses of Cu and of CuCl. Experimental yield x 100 bouos a ni Tuqgo2 ucvoaroo bor 0%Yiel
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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Calculate the theoretical yield. My cu is 1.006 g
Transcribed Image Text:LUnt (IMrate ion), and then reduce the copper(II) ion to copper(I) by the
te copper(II), remove the
addition of excess copper metal. ono to n
ovlo
The chemical reactions you will carry out in this lab are shown below.
1) Cu(s) + 4HNO3(aq) → Cu(NO3)2(aq) + 2NO2(g) + 2H2O(1)
2il ed
2) 2HNO3(aq) + Na2CO3(s)→ H2O(1) ±ÇO2(g) + 2NaNO3(aq)
0.
bay
3) Cu(NO3)2(aq) + NazCO3(s) → ÇUCO:(s) + 2NANO3(aq)
4) CUCO3() + 2HC((aq)
CuCh9) + H2O@ + CO2«g)
12
5) CuC2(aq) + Cu(s) 2CUCI)
BEPpe
to anstmoo adi
The reactions will be carried out in such a way that the copper metal added in the first
reaction will determine the amount of copper(I) chloride that forms in the last reaction
because it is the limiting reagent in all reactions where it's involved. In other words, all
the other reagents used for this preparation will be added in excess. The theoretical yield
is then based on the amount of copper added in the first reaction.
20
Calculations:
cwoda
1n bluoda
Theoretical yield =
-g CuC)
" mole CuCl
1 mole Cu 1 mole Cu(NO3)2
X.
1 mole CuCO3
1 mole CuCl2
2 mole CuCl
-g Cu x -
- g Cu
1 mole Cu
1 mole Cu(NO3)2 1 mole CuCO3 * 1 mole CuCl2
oLas 1st
You need to fill in the molar masses of Cu and of CuCl.
Experimental yield
x 100
bouos a ni Tuqgo2
ucvoaroo
bor
0%Yiel
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