You want to determine AH for the reaction Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) To...
Zinc reacts with hydrochloric acid according to the reaction equation Zn(s)+2HCl(aq)⟶ZnCl2(aq)+H2(g)Zn(s)+2HCl(aq)⟶ZnCl2(aq)+H2(g) How many milliliters of 2.00 M HCl(aq)2.00 M HCl(aq) are required to react with 8.55 g Zn(s)?
1. 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 50.1 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 21.9 ∘C to 24.6 ∘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.) ΔHrxn ΔHrxn =...
please help Zinc reacts with hydrochloric acid according to the reaction equation Zn(s) +2HCl(aq) ? ZnCl2(aq)-H2(g How many milliliters of 4.50 M HCl(aq) are required to react with 5.25 g of an ore containing 50.0% Zn(s) by mass? Number mL
Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When 0.102 g of Zn(s) is combined with enough HCl to make 54.6 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 21.9 ∘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 capacity
Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s)+2HCl(aq)?ZnCl2(aq)+H2(g) When 0.112 g of Zn(s) is combined with enough HCl to make 54.9 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 21.7 ?C to 23.9 ?C. Find ?Hrxn 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.) Answer should be in kJ/mol.
5. Zinc metal reacts with hydrochloric acid according the following balanced equation. Zn(s) + 2HCl(aq) à ZnCl2(aq) + H, (g) When 0.115 g of Zn(s) dissolves in 50.0 mL of HCl in a coffee-cup calorimeter, the temperature rises from 22.5 °C to 23.7 °C. Assume 1.0 g/mL for density of the solution and 4.18 J/g °C as the specific heat capacity, calculate: a) DH in kJ per mole of Zn(s) b) DH in kJ per gram of Zn(s)
Zinc metal reacts with hydrochloric acid according to the following balanced equation: Zn(s)+2HCl(aq)→ ZnCl2(aq)+H2(g) When 0.105 g of Zn(s) is combined with enough HCl to make 50.4 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.2 ∘C to 24.7 ∘C. Find ΔHrxn for this reaction as written. (Use 1.00 g/mL for the density of the solution and 4.18 J/(g⋅∘C) as the specific heat capacity.) Express your answer in kilojoules...
Determine S°rxn for Zn (s) + 2HCl (aq) ZnCl2 (aq) + H2 (g). Substance S° (J/mol ⋅ K) Zn(s) 60.9 HCl(aq) 56.5 H2(g) 130.58 Zn2+(aq) −106.5 Cl−(aq) 55.10 We were unable to transcribe this imageWe were unable to transcribe this image
Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g) When 0.104g 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 22.4 Celcius to 24.7Celcius. Find the delta Hrxn (in kJ/mol) for this reaction as written. (Use 1.0g/mL for the density of the solution and 4.18 J/g *Celcius as the specific...
Zinc reacts with hydrochloric acid according to the reaction equation shown. Zn(s)+2HCl(aq)⟶ZnCl2(aq)+H2(g) How many milliliters of 5.00 M HCl(aq) are required to react with 2.65 g of an ore containing 26.0 % Zn(s) by mass? volume: mL