Question

1. Hydrogen produced in the following reaction is collected over
water at 23^{o}C and 742 Torr:

2Al + 6HCl --> 2AlCl_{3} +
3H_{2}

What volume (mL) of the gas will be collected in the reaction of 1.50 g Al with excess HCl?

2. Sample of O2 gas has a volume of 50.0 L at a pressure of 750. mmHg. What is the final volume, in liters, of the gas at 2.0 atm?

3. What is the mass, in grams, of 475 mL of nitrogen gas at STP?

4. A 25.0 mL bubble is released from a diver's air tank at a
pressure of 4.00 atm and a pressure of 11^{o}C. What is the
volume, in mL, of the bubble when it reaches the ocean surface,
where the pressure is 1.00 atm and the temperature is
18^{o}C?

5. You vaporize a liquid substance at 100 ^{o}C and 755
mmHg. The volume of 0.548 g of vapor is 237 mL. What is the
molecular mass of the substance?

6. Given the following chemical equation:

4NH_{3} + 5O_{2} -->
4NO + 6H_{2}O

What volume (mL) of oxygen at 35 ^{o}C and 2.15 atm is
needed to produce 100.0 g of NO?

Answer #1

1. Hydrogen produced in the following reaction is collected over
water at 23oC and 742 Torr: 2Al + 6HCl --> 2AlCl3 + 3H2 What
volume (mL) of the gas will be collected in the reaction of 1.50 g
Al with excess HCl?
2. Sample of O2 gas has a volume of 50.0 L at a pressure of 750.
mmHg. What is the final volume, in liters, of the gas at 2.0
atm?
3. What is the mass, in grams, of...

Hydrogen produced from a hydrolysis reaction was collected over
water. The data is compiled in the table. Total volume of H2(g)
collected = 95.42 mL Temperature = 23.0 °C Barometric pressure =
742 mmHg Vapor pressure of water at 23.0 °? = 21.0 mmHg Calculate
the moles of hydrogen gas produced by the reaction.

The hydrogen gas formed in a chemical reaction is collected over
water at 30.0 ∘C at a total pressure of 736 mmHg
Part A
What is the partial pressure of the hydrogen gas collected in
this way?
Part B
If the total volume of gas collected is 722 mL , what mass of
hydrogen gas is collected?

The hydrogen gas produced by reaction between magnesium metal
and hydrochloric acid is collected via water displacement. The gas
in the collection flask has a volume of 0.0450 L at 25.0oC. If the
atmospheric pressure is 755 torr, how many moles of hydrogen gas
were collected. The vapor pressure of water at 25oC is 23.8
torr

A sample of nitrogen gas is produced in a reaction and collected
under water in a graduated cyliner. The temperature is 26.3
oC and the volume of gas is 45.6 mL.
During this experiment the total pressure in the graduated cylinder
is 745 mm Hg. How many grams of nitrogen
were collected? (The vapor pressure of water at 26oC is
25.2 torr.)

Information:
In this experiment, you will fill a gelatin capsule with an alloy
sample. If the mass of the gelatin capsule is 0.123 g, and the mass
of the capsule plus alloy sample is 0.215 g, calculate the
mass, in grams, of the alloy sample. - 0.092 g
The alloy sample is dissolved in HCl and
H2
gas
is produced and collected over water. The volume of
H2
gas produced is 89.5 mL. What is the volume of gas, in...

Exercise
11.106--- Part B
Consider the
reaction:
2NiO(s)→2Ni(s)+O2(g)
If O2 is collected
over water at 40 ∘C and a total pressure of 747 mmHg , what volume
of gas will be collected for the complete reaction of 25.51 g of
NiO?
Exercise
11.107---- Part C
How many grams of
hydrogen are collected in a reaction where 1.84 L of hydrogen gas
is collected over water at a temperature of 40 ∘C and a total
pressure of 747 torr ?

31.47 mL of hydrogen gas was collected over water, at
200C and 774-mmHg atmospheric pressure, when 0.0321 g of
magnesium was reacted according to the following equation:
Mg
(s) + 2 HCl
(aq) MgCl2(aq) + H2(g)
The pressure of water vapor at 20 0C is 18 mmHg.
Calculate the Gas constant based on the experimental results
above. Show all your work. Furthermore, why is gas collected over
water not pure?

A sample of oxygen gas was collected over water. The total
pressure was 735 torr, the volume was 555 mL, and the temperature
was 31.0ºC. What mass of oxygen was collected? The vapor pressure
of water at 31.0ºC is 33.7 torr.

1 in = 2.5 cm. 1 atm = 760 torr density of mercy = 13.6 g/mL at
25 oC gravity = 9.8 m/s2
R = 0.082 L.atm/mol.K PV =
nRT
Force = mass x acceleration
Pressure = Force/area
Today’s atmospheric pressure is 32.0” of mercury. What is the
pressure in ‘atm’ units?
The burette used in the lab has a cross-section area of 1
cm2 so that a height of 1 cm provides a volume of 1
cm3 (that is...

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