Question

Magnesium reacts with acid according to the equation: Mg + 2 H+ yields Mg2+ + H2 If 0.883 g of magnesium is added to 25.5 mL of 1.809 M HCl solution at 25°C and 1.00 atm, how many liters will be occupied by the dry hydrogen which is produced? The vapor pressure of water at 25°C is 3.2 kPa

Answer #1

: Mg + 2 H+ yields Mg2+ + H2

First calculate the number of moles of Mg as follows:

0.833 g /24.305 g/mol = 0.0342 mol Mg

Now moles of HCl as follows:

25.5 ml * 1.809 mol /1000 ml = 0.0461 mol HCl

here HCl is a limiting agent

HCl is limiting agent due to following reasons:

- It completely reacted in the reaction.
- It determines the amount of the product in mole.

Now calculate the moles of H2 as follows:

0.0461 mol HCl *1 mol of H2/ 2 mol HCl

= 0.02305 mol H2

According to gas law volume of gases is calculated as follows:

PV=nRT

V = nRT /P

Here R= 0.08206 (L*atm)/(mol*K) , P= 1.0 atm L, T = 298 K

V = nRT /P

V = 0.02305mol *0.08206 (L*atm)/(mol*K) *298K / 1.0 atm

**V=0.564 -L**

A piece of solid magnesium is reacted with dilute hydrochloric
acid to form hydrogen gas: Mg(s) + 2 HCl(aq) Æ MgCl2(aq) + H2(g)
What volume of H2 is collected over water at 28 °C by reaction of
1.25 g of Mg with 50.0 mL of 0.10 M HCl? The barometer records an
atmospheric pressure of 748 torr and the vapor pressure of water at
this temperature is 28.35 torr.
I am not quite sure what to do with the vapor...

Mg metal reacts with HCl to produce hydrogen gas.
Mg(s)+2HCl(aq)→MgCl2(aq)+H2(g)
What volume of hydrogen at 0 ∘C and 1.00 atm (STP) is released
when 8.80 g of Mg reacts?
Express your answer with the appropriate units.
How many grams of magnesium are needed to prepare 5.75 L of H2
at 745 mmHg and 16 ∘C?
Express your answer with the appropriate units.

If 10.0 grams of magnesium is added to a solution containing
1.00 mole of hydrochloric acid, how many grams of hydrogen gas are
produced?
Mg(s) + 2 HCl(aq) → H2(g) + MgCl2(aq)

Magnesium, an alkaline earth metal reacts with water producing
hydrogen gas. If one decides to collect the hydrogen over water at
20oC and the total amount of gas collected is 0.639 L with a
pressure of 1.11 atm, what is the amount of hydrogen in g in the
sample? Note: the vapor pressure of water at 20oC is 17.5 torr. The
balanced equation is: Mg(s) + 2 H2O(l) -> Mg(OH)2(aq) + H2(g)
The mass of hydrogen collected over water is...

Calcium carbonate, CaCO3, reacts with stomach acid (HCl,
hydrochloric acid) according to the following equation:
CaCO3(s)+2HCl(aq)→ CaCl2(aq)+H2O(l)+CO2(g)
One tablet of Tums, an antacid, contains 500.0 mg of CaCO3.
a) If one tablet of Tums is added to 34.5 mL of a 0.250 M HCl
solution how many liters of CO2 gas are produced at STP?
Express your answer with the appropriate units.

A piece of
sodium metal reacts completely with water as follows 2Na(s) +
2H2O(l)+2NaOH(aq)+ H2(g) The hydrogen gas generated is collected
over water at 25.0oC. The volume of the gas is 246 mL measured at
1.00 atm. Calculate the number of grams of sodium used in the
reaction. (Vapor pressure of water at 25°C 0.0313 atm.)

A 0.442 gram sample of a metal, M, reacts completely with
sulfuric acid according to:
M(s) + H2SO4(aq) -->
MSO4(aq) + H2(g)
A volume of 201 mL of hydrogen is collected over water; the
water level in the collecting vessel is the same as the outside
level. Atmospheric pressure is 756.0 Torr and the temperature is 25
°C. The vapor pressure of water at various temperatures can be
found in this table. Calculate the molar mass of the metal.

A 0.502 gram sample of a metal, M, reacts completely with
sulfuric acid according to: M(s) + H2SO4(aq) ----> MSO4(aq)
+H2(g) A volume of 217 mL of hydrogen is collected over water; the
water level in the collecting vessel is the same as the outside
level. Atmospheric pressure is 756.0 Torr and the temperature is 25
°C. The vapor pressure of water at various temperatures can be
found in this table. Calculate the molar mass of the metal.

A 0.528 gram sample of a metal, M, reacts completely with
sulfuric acid according to:
M(s) + H2SO4(aq) → MSO4(aq) + H2(g)
A volume of 205 mL of hydrogen is collected over water; the
water level in the collecting vessel is the same as the outside
level. Atmospheric pressure is 756.0 Torr and the temperature is 25
°C. The vapor pressure of water at various temperatures can be
found in this table. Calculate the molar mass of the metal.

When 0.854 g of impure zinc reacted with an excess of
hydrochloric acid, 244 mL of hydrogen gas was collected over water
at 10.0 °C. The external pressure was 714.96 Torr. The vapor
pressure of water at various temperatures can be found in this
table.
a. Calculate the volume the dry hydrogen would occupy at 1.00
atm and 298 K.
b. What amount, in moles, of H2 gas was collected at 10.0
°C?
c.Calculate the percentage purity of the zinc...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 3 minutes ago

asked 15 minutes ago

asked 25 minutes ago

asked 42 minutes ago

asked 46 minutes ago

asked 54 minutes ago

asked 55 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago