Question

1. Zinc metal and aqueous silver nitrate react according to the equation: Zn(s) + 2AgNO3 ---> 2Ag (s) + Zn(NO3)2 When 5.00 g of Zn reacts with an excess of AgNO3, (1.47x10^1) grams of silver are produced. What is the percent yield?

2.What is the molarity of a solution made by dissolving (7.54x10^0) g (assume 3 sig. figs.) of silver nitrate in water to make (4.164x10^1) mL of solution?

3. What is the molarity of a solution made by diluting (5.318x10^1) mL of 18.7 M ammonia with enough water to form (8.38x10^2) mL of solution?

Answer #1

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 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 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 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 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) + H2(g)
How many milliliters of 6.50 M HCl(aq) are required to react
with 3.05 g of Zn(s)?

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) + 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?

1. You need to make an aqueous solution of
0.241 M zinc bromide for an
experiment in lab, using a 300 mL volumetric
flask. How much solid zinc bromide should you
add?
2.How many milliliters of an aqueous solution of
0.132 M calcium chloride is
needed to obtain 8.00 grams of the salt?
1. In the laboratory you dissolve 22.3 g of
silver nitrate in a volumetric flask and add water
to a total volume of 250 mL.
What is...

1 What is the molarity of a solution made by dissolving 4.17 g
of magnesium nitrate [Mg(NO3)2] in enough
water to make 22.0 mL of solution
2 Upon heating 118 g MgSO4 · 7 H2O:
(a) how many grams of water can be obtained?
(b) how many grams of anhydrous compound can be obtained?

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