Question

Solid magnesium reacts with aqueous hydrochloric acid, HCI, to form aqueous magnesium chloride and hydrogen, H₂, gas at 298 K and 1 atm pressure. 

a. Write a balanced chemical equation, including phases, to describe this reaction. 

b. If a 1.512-g sample of magnesium is added to 0.2558 moles of hydrochloric acid, how many moles of hydrogen gas are formed? 

c. In an actual experiment in which the amounts of magnesium and hydrochlorie acid from part b (above) are reacted, 1.23 L of H₂ gas are collected. What is the percentage yield? 

Answer 1

first write the balanced equation and then find the moles from that identify the limiting reactant and calculate the percent yield as follows