Question

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.

Answer #1

Mass of solution = density * volume = 1.00 * 55.0 = 55.0 g.

Specific heat capacitiy of solution = 4.184
J/g.^{0}C

Change in temperature = 24.4 - 21.7 = 2.7 ^{0}C

Heat change = mass * specific heat capacity * change in temperature

q = 55.0 * 4.184 * 2.7

q = 621. J

And

Mass of Zn = 0.103 g.

Molar mass of Zn = 65.3 g/mol

Moles of Zn = mass / molar mass = 0.103 / 65.3 = 0.00158 mol

Therefore,

Enthalpy change per mol of Zn = q / n = 621. / 0.00158 = 393702 J / mol = 393.7 kJ/mol of Zn

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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
0.119 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.
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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
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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
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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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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?

Manganese reacts with hydrochloric acid to produce manganese(II)
chloride and hydrogen gas. Mn(s)+2HCl(aq) → MnCl2(aq)+H2(g). When
0.605 g Mn is combined with enough hydrochloric acid to make 100.0
mL of solution in a coffee-cup calorimeter, all of the Mn reacts,
raising the temperature of the solution from 23.2 ∘C to 28.7 ∘C.
Find ΔHrxn for the reaction as written. (Assume that the specific
heat capacity of the solution is 4.18 J/g∘C and the density is 1.00
g/mL.)

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chloride and hydrogen gas.
Mn(s)+2HCl(aq) →
MnCl2(aq)+H2(g)
When 0.615 g Mn is combined with
enough hydrochloric acid to make 100.0 mL of solution in a
coffee-cup calorimeter, all of the Mn reacts, raising the
temperature of the solution from 24.0 ∘C to 28.4 ∘C.
Find ΔHrxn = ? kJ for the reaction as written. (Assume
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degrees C if 15.11 g of zinc reacted with excess hydrochloric
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Zn(s) + 2HCl(aq) ---> ZnCl2(aq) + H2(g)

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