1. For the following chemical reaction, what mass of silver nitrate in grams wil

Question

1. For the following chemical reaction, what mass of silver nitrate in grams will be needed to produce 2.71 mol of calcium nitrate? cai2+2agno3=2 agi+ca(no3)2

2.Given the following chemical equation, determine how many grams of N2 are produced by 9.29 g of H2O2 and 5.54 g of N2H4.

3.a) The balanced reaction equation for combustion of heptane, C7H16, is given below. If the reaction produced 40.5 g CO2, how many grams of heptane were burned?

C7H16+11O2-->7CO2+8H20

4.b) The reaction of limestone with hydrochloric acid is given below. If the reaction produced 40.5 g CO2, how many grams of HCl reacted?

CACO3+2HCl-->CaCl2+CO2+H2O

Explanation / Answer

1) CaI2 + 2AgNO3 -------> 2AgI + Ca(NO3)2

As per the balanced reaction 1 mole of calcium nitrate is formed by 2 moles of silver nitrate

Thus, 2.71 moles of calcium nitrate will be formed by 5.42 moles of silver nitrate

Now, molar mass of silver nitrate = 169.87 g/mole

Thus, mass of silver nitrate required = moles*molar mass = 5.42*169.87 = 920.6954 g

2) The question is wrong. If it is correct please provide the reaction beacause I think that he correct reaction is :-

5 N2H4 + 15 H2O2 = 10 HNO3 + 2 H20

3) C7H16 + 11O2 -----------> 7CO2 + 8H2O

Molar mass of CO2 = 44 g/mole

Thus, moles of CO2 produced = mass/molar mass = 40.5/44 = 0.92

Now, 7 moles of CO2 is produced by 1 mole of heptane

Thus, 0.92 moles of CO2 is produced by 0.92/7 = 0.1315 moles of heptane

Now, molar mass of heptane = 100 g/mole

Thus, mass of heptane burnt = 0.1315*100 = 13.15 g

4) CaCO3 + 2HCl ----------> CaCl2 + CO2 + H2O

Molar mass of CO2 = 44 g/mole

Thus, moles of CO2 produced = mass/molar mass = 40.5/44 = 0.92

Now, 1 mole of CO2 is produced by 2 moles of HCl

Thus, 0.92 moles of CO2 is produced by 1.841 moles of HCl

Now, molar mass of HCl = 36.5 g/mole

Thus, mass of HCl required = moles*molar mass = 1.841*36.5 = 67.19 g

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