Answer to Question #170432 in General Chemistry for mel

Question

1.) Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide.

4HCl(aq) + MnO₂(s) --> MnCl₂ (aq) + 2H₂O(l) + Cl₂(g)

A sample of 34.5 g MnO₂ is added to a solution containing 50.5g HCl.

what is the limiting reactant? MnO₂ or HCl

what is the theoretical yield of Cl₂?

theoretical yield:________?_______g Cl₂

If the yield of the reaction is 87.3%, what is the actual yield of chlorine?

Actual yield:_________?________g Cl₂

5.) Assuming an efficiency of 38.70%, calculate the actual yield of magnesium nitrate formed from 130.7g of magnesium and excess copper (II) nitrate

Mg + Cu(NO₃)₂ --> Mg(NO₃)₂ + Cu

Actual yield:_________?_______g

6.) A sample of 9.65g of solid calcium hydroxide is added to 33.5 mL of 0.500 M aqueous hydrochloric acid.

write the balanced chemical equation for the reaction. Physical states are optional.

Chemical equation:____________________?

what is the limiting reactant? hydrochloric acid or calcium hydroxide

How many grams of salt are formed after the reaction is complete?

mass of salt:__________?____________g

how many grams of the excess reactant remain after the reaction is complete?

excess reactant remaining:___________?_______g

Answer 1

the limiting reagent is MnO2

1mole of Cl is formed when 4 moles of HCl are reduced by 1 mole of MnO2

$Theoretical=( actual/percentage)$

Theoretical yield =?

If 50.5g of HCl react then 50.5/36.5= 1.38moles

Theoretical yield of chlorine is then ;

1.38× 35.5= 49.9g