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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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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solution in a coffee-cup calorimeter, all of the zinc reacts,
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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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How many milliliters of 2.00 M HCl(aq) are required to react
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Zinc metal reacts with hydrochloric acid according to the
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Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g)
the hydrogen gas is collected over water at a temperature of
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