2. Consider the reaction represented by the (unbalanced) equation: Mg(s) + HCl(a

Question

2. Consider the reaction represented by the (unbalanced) equation: Mg(s) + HCl(a) MgCl,(aq)+ H2(g) Determine the mass of H,(g) that can be produced from the following: a. 10.0 g Mg(s) reacts completely with HCl(aq). b. 20.0 g HCI (aq) reacts completely with Mg(s). The mass of oxygen gas that would be needed to completely react with 10.0 g of hydrogen gas to form water is instead reacted completely with methane (CH) to form carbon dioxide and water. Determine the mass of carbon dioxide produced. 3.

Explanation / Answer

The balanced reaction will be

Mg + 2HCl = MgCl2 + H2

molar mass of Mg = 24.3g

molar mass of HCl = 36.5g

molar mass of H2 = 2g

molar mass of MgCl2 = 95.2g

As the reaction proceeds 1 mole Mg reacts with 2 mole HCl to give 1mole MgCl2 and 1 mole H2

So,

(a)No. of moles in 10 g 0f Mg = 10/12 =0.83 which completely reacts with 2 times HCl to produce 1 times H2 i.e- 0.83 mole of H2

Hygrogen molecule produced = 0.83 * 2g = 1.67g

(b) No of moles for 20 g HCl = 20 / 36.5 = 0.55 mole

It will give half of the molar molar amount of HCl i.e = 0.275 mole

So , mass of H2 produce = 0.275 * 2 = 0.55g

Related Questions

Navigate

• Browse (All)
• Browse 2
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.