Problem: Consider the reaction between Mg(s) and HCl(aq) to produce aqueous magnesium chloride and hydrogen gas. What volume of hydrogen at STP will be produced when 12.15 g of magnesium reacts with an excess of hydrochloric acid?A. 1.00 LB. 2.00 LC. 5.6 LD. 11.2 LE. 22.4 L

🤓 Based on our data, we think this question is relevant for Professor Dixon's class at UCF.

FREE Expert Solution
FREE Expert Solution

We will calculate the amount of hydrogen gas (H2(g)) produced from Mg(s). The limiting reactant is Mg(s) since HCl(aq) is in excess.

Let’s first write the balanced reaction equation:

Reactants:

Mg(s)
HCl(aq)

Products:

aqueous magnesium chloride

▪ magnesium → group 2A → +2 charge → Mg2+ 
▪ chloride → group 7A → -1 charge → Cl- 
*criss cross the charges of Mg2+ and Cl- and that would be the subscript of each ion
▪ aqueous magnesium chloride → MgCl2(aq)

hydrogen gas → diatomic hydrogen gas → H2(g)

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Problem Details

Consider the reaction between Mg(s) and HCl(aq) to produce aqueous magnesium chloride and hydrogen gas. What volume of hydrogen at STP will be produced when 12.15 g of magnesium reacts with an excess of hydrochloric acid?

A. 1.00 L

B. 2.00 L

C. 5.6 L

D. 11.2 L

E. 22.4 L

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