Question

A 2.25 gram sample of zinc metal reacts with 5.00 grams of hydrochloric acid to give zinc chloride and hydrogen gas according the blanced equation:

Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) Molar mass ZnCl2: 136.28 g/mol

a. What is the limiting reactant?

b. What mass of ZnCl2 can be formed? (This is called the theoretical yield.)

Answer #1

Number of moles of Zn = 2.25 g / 65.38 g/mol = 0.0344 mole

Number of moles of HCl = 5.00g / 36.46 g/mol = 0.137 mole

from the balanced equation we can say that

1 mole of Zn requires 2 mole of HCl so

0.0344 mole of Zn will require 0.0688 mole of HCl

but we have 0.137 mole of HCl which is in excess so

Zn is the limiting reactant

1 mole of Zn produces 1 mole of ZnCl2 so

0.0344 mole of Zn will produce 0.0344 mole of ZnCl2

1 mole of ZnCl2 = 136.28g

0.0344 mole of ZnCl2 = 4.69 g

Therefore, the theoreticale yield of ZnCl22 = 4.69g

Zinc metal reacts with hydrochloric acid to produce zinc
chloride and hydrogen gas according to the equation below. What
volume of hydrogen gas would be produced at 0.998 atm and 27
degrees C if 15.11 g of zinc reacted with excess hydrochloric
acid?
Zn(s) + 2HCl(aq) ---> ZnCl2(aq) + H2(g)

Zinc metal reacts with hydrochloric acid according to the
following balanced equation.
Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g)
the hydrogen gas is collected over water at a temperature of
20.0 degrees celsius and a total pressure of 775.2 mmHg. a total of
1.85 L of gas is collected. the vapor pressure of water at 20.0
degrees celsius is 17.55 mmHg. what is the mass of hydrogen gas (in
grams) formed

A)
Zinc metal reacts with excess hydrochloric acid to
produce hydrogen gas according to the following
equation:
Zn(s) + 2HCl(aq) ------------>
ZnCl2(aq) + H2(g)
The product gas, H2, is collected over
water at a temperature of 20 °C and a pressure of
757 mm Hg. If the wet
H2 gas formed occupies a volume of
7.17L, the number of moles of Zn
reacted was ___________ mol. The vapor pressure of water is
17.5 mm Hg at 20 °C.
B) Oxygen...

Zinc metal reacts with hydrochloric acid according to the
following balanced equation. Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When
0.103 g of Zn(s) is combined with enough HCl to make 55.0 mL of
solution in a coffee-cup calorimeter, all of the zinc reacts,
raising the temperature of the solution from 21.7 ∘C to 24.4
∘C.

Zinc reacts with hydrochloric acid according to the reaction
equation Zn (s)+2HCl (aq)--> ZnCl2 (aq) + H2(g) How many
milliliters of 2.50 M HCl(aq) are required to react with 3.55 g of
an ore containing 37.0% Zn(s) by mass?

Zinc reacts with hydrochloric acid according to the reaction
equation
Zn(s) + 2HCL (aq) -----------> ZnCl2(aq) + H2(g)
How many milliliters of 2.00 M HCl(aq) are required to react
with 7.05 g of an ore containing 38.0% Zn(s) by mass?

Zinc reacts with hydrochloric acid according to the reaction
equation
Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g)
How many milliliters of 6.50 M HCl(aq) are required to react
with 3.05 g of Zn(s)?

Zinc metal reacts with hydrochloric acid according to the
following balanced equation. Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When
0.106 g of Zn(s) is combined with enough HCl to make 54.5 mL of
solution in a coffee-cup calorimeter, all of the zinc reacts,
raising the temperature of the solution from 21.6 ∘C to 24.5 ∘C.
Find ΔHrxn for this reaction as written. (Use 1.0 g/mL for the
density of the solution and 4.18 J/g⋅∘C as the specific heat
capacity.) In kJ/mol.

Zinc metal reacts with hydrochloric acid according to the
following balanced equation. Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When
0.107 g of Zn(s) is combined with enough HCl to make 51.6 mL of
solution in a coffee-cup calorimeter, all of the zinc reacts,
raising the temperature of the solution from 22.2 ∘C to 24.3 ∘C.
Find ΔHrxn for this reaction as written. (Use 1.0 g/mL for the
density of the solution and 4.18 J/g⋅∘C as the specific heat

Zinc metal reacts with hydrochloric acid according to the
following balanced equation. Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When
0.119 g of Zn(s) is combined with enough HCl to make 53.4 mL of
solution in a coffee-cup calorimeter, all of the zinc reacts,
raising the temperature of the solution from 21.7 ∘C to 24.5 ∘C.
Part A Find ΔHrxn for this reaction as written. (Use 1.0 g/mL for
the density of the solution and 4.18 J/g⋅∘C as the specific heat
capacity.)

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 9 minutes ago

asked 13 minutes ago

asked 44 minutes ago

asked 49 minutes ago

asked 51 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago