Question
In: Chemistry
Solid magnesium reacts with aqueous hydrochloric acid, HCI, to form aqueous magnesium chloride and hydrogen, H2, gas at 298 K and 1 atm pressure
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?
Solutions
Expert Solution
first write the balanced equation and then find the
moles from that identify the limiting reactant and calculate the
percent yield as follows
queen_honey_blossom answered 2 years agoRelated Solutions
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1: A piece of solid magnesium is reacted with hydrochloric acid to form hydrogen gas: Mg(s)...
1:
A piece of solid magnesium is reacted with hydrochloric acid to
form hydrogen gas:
Mg(s) + 2
HCl(aq) à MgCl2(aq) + H2(g)
What volume of hydrogen gas (in mL) is collected over water at
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PLEASE make sure there are the right number of significant
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0.36g
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E.54.0 grams
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