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Challenge Stoichiometry

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1 Challenge Stoichiometry
Lesson 7

2 A 10.0 g sample of a Cu/Ag alloy reacted with concentrated HNO3 according to the following equations. A total of g of NO2 was isolated. Assuming a 100 % yield of NO2, determine the mass of Cu and Ag in the alloy. Cu(s) HNO3(aq) → Cu(NO3)2(aq) NO2(g) H2O(l) Ω g ?g 2Ag(s) HNO3(aq) → AgNO3(aq) NO2(g) H2O(l) (10 - Ω) g ?g 10.0 g 8.986 g

3 A 10.0 g sample of a Cu/Ag alloy reacted with concentrated HNO3 according to the following equations. A total of g of NO2 was isolated. Assuming a 100 % yield of NO2, determine the mass of Cu and Ag in the alloy. Cu(s) HNO3(aq) → Cu(NO3)2(aq) NO2(g) H2O(l) 2Ag(s) HNO3(aq) → AgNO3(aq) NO2(g) H2O(l) Ω g Cu x mole x 2 mole NO2 x g = Ω 63.5 g 1 mole Cu 1 mole 10 – Ω g Ag x mole x 2 mole NO2 x g = Ω 107.9 g 2 mole Ag 1 mole Ω Ω = Ω = Note the loss of a sig fig! Ω = 4.62 g Cu = g Ag

4 A g sample of brass, a Cu/Zn alloy, is completely reacted with concentrated HNO3 according to the following equations. A total of g of NO2 was isolated. Assuming a 100 % yield of NO2, determine the mass of Cu and Zn in the alloy. Cu(s) HNO3(aq) → Cu(NO3)2(aq) NO2(g) H2O(l) Ω g ?g Zn(s) HNO3(aq) → Zn(NO3)2(aq) NO2(g) H2O(l) (10 - Ω) g ?g 10.0 g g

5 A g sample of brass, a Cu/Zn alloy, is completely reacted with concentrated HNO3 according to the following equations. A total of g of NO2 was isolated. Assuming a 100 % yield of NO2, determine the mass of Cu and Zn in the alloy. Cu(s) HNO3(aq) → Cu(NO3)2(aq) NO2(g) H2O(l) Zn(s) HNO3(aq) → Zn(NO3)2(aq) NO2(g) H2O(l) Ω g Cu x mole x 2 mole NO2 x g = Ω 63.5 g 1 mole Cu 1 mole 10 – Ω g Zn x mole x 2 mole NO2 x g = Ω 65.4 g 1 mole Zn 1 mole Ω Ω = Ω = Ω = g Cu 10.00 – = g Zn

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