Question

The reaction of zinc with hydrochloric acid is represented by the reaction Zn(s) + 2 HCl(aq)...

The reaction of zinc with hydrochloric acid is represented by the reaction

Zn(s) + 2 HCl(aq) ↔ ZnCl2(aq) + H2(g) -- ΔH = -152.5 kJ

How many grams of zinc reacted with an excess of HCl (100.0 mL) if the temperature of the calorimeter increased from 25.0°C to 31.83 °C? Assume the heat capacity of the solution is the same as pure water (4.184 J/g*°C), the density of the solution is 1.00 g/mL and there is no loss of heat to the surroundings.

Homework Answers

Answer #1

Solution"- volume of solution would be same as the volume of HCl that is 100.0 mL

density of solution = 1.00 g/mL

mass of solution = 100.0 mL x 1.00g/mL = 100.0 g

delta T = 31.83 - 25.0 = 6.83 0C

q = m c deltaT

q = 100.0 x 4.184 x 6.83

q = 2857.672 J = 2.86 kJ

From balanced equation, 152.5 kJ of heat is released when 1 mol of Zn is used. How many moles of Zn are used when 2.86 kJ of heat is released.

2.86 kJ x 1mol/152.5 kJ = 0.0188 mol

We would convert these moles to grams on multiplying the moles with atomic mass of Zn.

0.0188 mol x 65.38g/1mol = 1.23 g

So, 1.23 g of Zn were reacted.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When 0.107 g...
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...
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.)
Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When 0.106 g...
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 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.)
Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When 0.106 g...
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 reacts with hydrochloric acid according to the reaction equation Zn(s) + 2HCl(aq) -> ZnCl2(aq) +...
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 0.103 g...
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) +...
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)...
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?
When 0.109 g of Zn(s) combines with enough HCl to make 55.7 mL of HCl(aq) in...
When 0.109 g of Zn(s) combines with enough HCl to make 55.7 mL of HCl(aq) in a coffee cup calorimeter, all of the zinc reacts, which increases the temperature of the HCl solution from 23.2 °C to 24.8 °C: Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) Calculate the enthalpy change of the reaction ΔHrxn in J/mol. Insert your answer in kJ, but do not write kJ after the number. (Assume the density of the solution is 1.00 g/mL and the...
When 0.113 g of Zn(s) combines with enough HCl to make 53.6 mL of HCl(aq) in...
When 0.113 g of Zn(s) combines with enough HCl to make 53.6 mL of HCl(aq) in a coffee cup calorimeter, all of the zinc reacts, which increases the temperature of the HCl solution from 23.3 °C to 24.7 °C: Zn(s) + 2HCl(aq) → ZnCl2​(aq) + H2​(g) Calculate the enthalpy change of the reaction ΔHrxn​ in J/mol. Insert your answer in kJ, but do not write kJ after the number. (Assume the density of the solution is 1.00 g/mL and the...