2. In a laboratory experiment you react 20.0 mL of 25% by mass C2H&N2 with 8.000 NiCl2.6H2O to obtain the product Ni(NH2CH¿CHNH2y3Cl2 complex. The C2HạN2 solution used in this experiment is 25.0% by mass, with a density (d) of 0.950 g/mL. (MW NICI2.6H2O= 237.69 g/mole, MW C2H&N2=60.10 g/mole, MW tris(ethylenediamine)nickel(I)chloride = 309.89 g/mole) a. Write down the balanced equation of the synthesis. b. Determine the number of moles of each reactant that you use. c. Determine which reactant is the limiting reactant, giving your reasoning. Show all your work to get full credit. (5 points) d. Calculate your percent yield if the dry product weighs 7.000 g.
2. In a laboratory experiment you react 20.0 mL of 25% by mass C2H&N2 with 8.000 NiCl2.6H2O to obtain the product Ni(NH2CH¿CHNH2y3Cl2 complex. The C2HạN2 solution used in this experiment is 25.0% by mass, with a density (d) of 0.950 g/mL. (MW NICI2.6H2O= 237.69 g/mole, MW C2H&N2=60.10 g/mole, MW tris(ethylenediamine)nickel(I)chloride = 309.89 g/mole) a. Write down the balanced equation of the synthesis. b. Determine the number of moles of each reactant that you use. c. Determine which reactant is the limiting reactant, giving your reasoning. Show all your work to get full credit. (5 points) d. Calculate your percent yield if the dry product weighs 7.000 g.
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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![2.
In a laboratory experiment you react 20.0 mL of 25% by mass C2H&N2
with 8.000 NiCl2.6H20 to obtain the product Ni(NH2CH2CH½NH2j3Cl2 complex. The
C2H3N2 solution used in this experiment is 25.0% by mass, with a density (d) of
0.950 g/mL.
(MW NICI2.6H2O= 237.69 g/mole, MW C2HgN2=60.10 g/mole,
MW tris(ethylenediamine)nickel(II)chloride = 309.89 g/mole)
a. Write down the balanced equation of the synthesis.
b. Determine the number of moles of each reactant that you use.
c. Determine which reactant is the limiting reactant, giving your reasoning. Show all
your work to get full credit. (5 points)
d. Calculate your percent yield if the dry product weighs 7.000 g.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4a3911b3-6865-46e2-bd9c-a74f2e98b2fe%2F0458c086-0331-4c19-ad39-635161ed0bae%2F07cen4m_processed.png&w=3840&q=75)
Transcribed Image Text:2.
In a laboratory experiment you react 20.0 mL of 25% by mass C2H&N2
with 8.000 NiCl2.6H20 to obtain the product Ni(NH2CH2CH½NH2j3Cl2 complex. The
C2H3N2 solution used in this experiment is 25.0% by mass, with a density (d) of
0.950 g/mL.
(MW NICI2.6H2O= 237.69 g/mole, MW C2HgN2=60.10 g/mole,
MW tris(ethylenediamine)nickel(II)chloride = 309.89 g/mole)
a. Write down the balanced equation of the synthesis.
b. Determine the number of moles of each reactant that you use.
c. Determine which reactant is the limiting reactant, giving your reasoning. Show all
your work to get full credit. (5 points)
d. Calculate your percent yield if the dry product weighs 7.000 g.
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