Question

1.) An aqueous solution containing 5.66 g of lead(II) nitrate is added to an aqueous solution containing 6.30 g of potassium chloride. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. balanced chemical equation What is the limiting reactant? The percent yield for the reaction is 79.2 % . How many grams of precipitate is recovered? precipitate recovered: How many grams of the excess reactant remain? excess reactant remaining:

2.) Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide. 4 HCl ( aq ) + MnO 2 ( s ) ⟶ MnCl 2 ( aq ) + 2 H 2 O ( l ) + Cl 2 ( g ) A sample of 43.3 g MnO 2 is added to a solution containing 48.5 g HCl . What is the limiting reactant?

What is the theoretical yield of Cl2? If the yield of the reaction is 84.1%,84.1%, what is the actual yield of chlorine?

3.) Assuming an efficiency of 49.90%,49.90%, calculate the actual yield of magnesium nitrate formed from 110.3 g of magnesium and excess copper(II) nitrate.

Mg+Cu(NO3)2⟶Mg(NO3)2+Cu

4.) Write and balance the equation for the complete combustion of acetylene, C2H2. Phase symbols and energy changes are optional.

5.) Calculate the number of pounds of CO2 released into the atmosphere when a 16.0 gallon tank of gasoline is burned in an automobile engine. Assume that gasoline is primarily octane,C8H18, and that the density of gasoline is 0.692 g⋅mL−1. This assumption ignores additives. Also, assume complete combustion.

6.) Write the net ionic equation, including phases, that corresponds to the reaction Fe(NO3)2(aq)+K2CO3(aq)⟶FeCO3(s)+2KNO3(aq)

7.) For the chemical reaction 2HBr(aq)+Ba(OH)2(aq)⟶2H2O(l)+BaBr2(aq) write the net ionic equation, including the phases.

8.) Complete and balance the molecular equation for the reaction of aqueous sodium sulfate, Na2SO4, and aqueous barium nitrate, Ba(NO3)2. Include physical states. Enter the balanced net ionic equation for this reaction. Include physical states.

Answer 1