a) For the equation Cu2O + C Cu + CO, if 2.73 moles of C are reacted with an excess of Cu2O, how many moles of CO would be produced? _______________moles
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a) For the equation Cu2O + C Cu + CO, if 2.73 moles of C are reacted with an excess of Cu2O, how many moles of CO would be produced? _______________moles
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b) For the equation Co(NO3)3 + (NH4)2S Co2S3 + NH4NO3, if 79.2 g of Co(NO3)3 are reacted with an excess of (NH4)2S, how many moles of NH4NO3 would be produced? ______________moles
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c) For the equation (NH4)2CO3 CO2 + H2O + NH3, if 4.01 moles of (NH4)2CO3 reacted, what is the theoretical yield of CO2? _________________g
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d) For the equation N2H4 NH3 + N2, if the theoretical yield is 28.0 grams of N2, what mass in grams of N2H4, would have to react? ______________g
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e) For the equation FeS + HCl FeCl2 + H2S, if 35.0g of FeS is added to 35.0g of HCl and allowed to react, what is the theoretical yield of H2S? __________________g
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f) Using the numbers from problem e) above, if 10.2 g of H2S were obtained in the lab (actual yield), what is the percent yield? __________________%
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g) How many grams of K2C2O4, potassium oxalate, would contain 182 grams of pure potassium?
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b) How many grams of strontium nitrate, Sr(NO3)2, are needed to prepare 3.40x103mL of a 0.925 M solution? ____________________
a) What is the molarity of a solution made by dissolving 6.08g of sodium acetate, CH3COONa, in water, and diluting it to a total volume of 0.750L? _________M
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c) To what volume should 50.0mL of a 6.00M HCl stock solution be diluted to obtain a 1.50M HCl solution? How much water should be used?
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d) A 38.5mL sample of 0.875M AgNO3 solution is mixed with 51.0mL sample of 0.744M NaCl solution. The AgCl precipitated has a mass of 2.06g. Calculate the limiting reactant, the theoretical yield, and percent yield.
AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq)
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