Question

One reaction that produces hydrogen gas can be represented by the following unbalanced chemical equations:
Mg(s) + HCl(aq) --> MgCl2(aq) + H2(g)
a. what mass of HCl is consumed by the reaction of 2.50 moles of magnesium?
b. What mass of each product is produced in part a?

I do not know where to even start to figure this problem out, except balancing the formula. I did some math and I have an answer but I am not sure if it is right or not.

Answer 1

Answer on Question #56532 - Chemistry – General chemistry

Question

One reaction that produces hydrogen gas can be represented by the following unbalanced chemical equations:

$$\mathrm{Mg}(s) + \mathrm{HCl}(aq) \rightarrow \mathrm{MgCl_2}(aq) + \mathrm{H_2}(g)$$

a. what mass of HCl is consumed by the reaction of 2.50 moles of magnesium?

b. What mass of each product is produced in part a?

I do not know where to even start to figure this problem out, except balancing the formula. I did some math and I have an answer but I am not sure if it is right or not.

Answer:

Balanced reaction equation:

$$\mathrm{Mg}(s) + 2\mathrm{HCl}(aq) \rightarrow \mathrm{MgCl_2}(aq) + \mathrm{H_2}(g)$$

a. 2.50 moles of magnesium react with 5.00 moles of hydrogen chloride. Therefore the mass of HCl consumed by the reaction of 2.50 moles of magnesium is:

$$m(HCl) = n(HCl) * M(HCl) = 5.00 \cdot 36.5 = 182.5\,g$$

b. If 2.50 moles of magnesium react, 2.50 moles of magnesium chloride and 2.50 moles of hydrogen are produced. Therefore the mass of $\mathrm{MgCl_2}$ produced is:

$$m(MgCl_2) = n * M = 2.50 \cdot 95.3 = 238.3\,g$$

The mass of $\mathrm{H_2}$ produced is:

$$m(H_2) = n(H_2) * M = 2.50 * 2.0 = 5.00\,g$$

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