Question

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

Answer #1

Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g)

dry H2 gas pressure = total pressure of the gas - the vapor pressure of water at 20.0 degrees celsius

= 775.2 - 17.55

= 757.65 mm Hg

pressure of dry H2 gas in atm. = 0.997 atm.

according to PV = nRT ==> PV = (mass/mol.wt)*RT

mass = P*V*mol.wt/RT

mass =( 0.997*1.85*2)/(0.0821*293)

mass = 0.153 gm.

mass of H2 gas = 0.153 gm.

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.

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...

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degrees C if 15.11 g of zinc reacted with excess hydrochloric
acid?
Zn(s) + 2HCl(aq) ---> ZnCl2(aq) + H2(g)

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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

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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.)

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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 50.6 mL of
solution in a coffee-cup calorimeter, all of the zinc reacts,
raising the temperature of the solution from 21.5 ∘C to 24.4 ∘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.)

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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.

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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)?

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milliliters of 2.50 M HCl(aq) are required to react with 3.55 g of
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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
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