Question

Zn + HCl --> 2ZnCl2 + H2

Assuming you start with 10.0 g of zinc and 10.0 g hydrochloric acid, identify the limiting reagent and determine what mass of the other reagent will remain after the reaction runs to completion.

Answer #1

you have given reaction is wrong the correct reaction is

Zn + 2HCl
ZnCl_{2} + H_{2}

molar mass of Zn = 65.38 gm/mole that mean 1 mole of Zn = 65.38 gm Zn

molar mass of HCl =36.4609gm/mol that mean 1 mole of HCl =36.4609gm mol then 2 mole HCl = 72.9218 gm

According to reaction 1 mole of Zn react with 2 mole of HCl that mean 65.38 gm of Zn require 72.9218 gm of HCl

then 10 gm of Zn require 72.921810/65.38 = 11.15 gm of HCl

but HCl taken only 10 gm threfore HCl is limiting reagent

for 72.9218 gm of HCl require 65.38 gm of Zn then 10 gm of HCl require 1065.38/729218 =.8.96 gm of Zn

we taken 10 gm of Zn thus 10 - 8.96 = 1.04 gm of Zn remain after reaction runs to completion.

Use the equation Zn + 2HCl -> ZnCl2 +
H2
If you react 71.24 g Zn with 91.53 g HCl, what mass of zinc
chloride is produced? And what is the limiting reactant in this
situation? Show all calculations.

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?

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...

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 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
0.119 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 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.

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 8 minutes ago

asked 9 minutes ago

asked 15 minutes ago

asked 26 minutes ago

asked 26 minutes ago

asked 31 minutes ago

asked 39 minutes ago

asked 40 minutes ago

asked 54 minutes ago

asked 58 minutes ago

asked 1 hour ago

asked 1 hour ago