Question

1 in = 2.5 cm. 1 atm = 760 torr density of mercy = 13.6 g/mL at
25 ^{o}C gravity = 9.8 m/s^{2}

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
cm^{2} so that a height of 1 cm provides a volume of 1
cm^{3} (that is 1 mL).

(a) What is the mass of mercury in a burette filled up to a height
of 76 cm? Give the answer in kg units.

(b) What is the force of this 76 cm mercury column acting downward
due to gravity? [Note: As long as you use SI units for mass and
acceleration, the SI unit for force is Newtons]

(c) Pressure is Force per unit area. What is pressure due to this
76 cm mercury column? [Note: the cross sectional area of the column
is given in non SI unit. As long force and area are in SI units,
the SI unit for pressure is Pascal.]

(d) You have learned that 1 atm pressure is 76 cm of mercury. Based
on the math you did in this problem, what is the value of 1 atm in
Pascal units?

(a) Container A has a volume of 5.0 L and is filled with 5.0
grams of hydrogen gas at 25^{o}C. What will be the pressure
of hydrogen gas in the container?

(b) Another container (container B) has a volume of 10.0 L and is
also filled with 5.0 grams of hydrogen gas at 25 ^{o}C.
What will be the pressure of hydrogen gas in this container?

(c) If container A and container B are connected with each other
using a small glass tube to allow free flow of gas between them,
what will happen to the pressure of hydrogen gas? If it is
affected, find the new value.

N_{2} (g) + 3 H_{2} (g) à 2 NH_{3} (g).
In a reaction, 24.0 g of nitrogen and 14.0 g of hydrogen are
reacted to produce ammonia in 5.0 L rigid container at 25
^{o}C .

(a) What will be the pressure inside the container before the
reaction starts?

(b) What is the limiting reactant in this reaction?

(c) After the reaction is completed, how many moles of product and
how many moles of unreacted reactant will be present?

(d) What will be the pressure in the container after the reaction
is complete?

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...

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...

96.1 g of solid iron reacts with 0.0500 L of water (density =
0.997 g/mL) to form iron(III)oxide and hydrogen gas. If the
reaction takes place in a 10.0 L container at 400.0 K, what
pressure in atm would be measured?
When 0.62 mols of aluminum metal react with 4.55 mols of HCl
according to the reaction below what will be the final pressure
(in atm) if the two substances react in a solid steel
chamber with a volume of...

1)A system at equilibrium contains I2(g) at a pressure of 0.10
atm and I(g) at a pressure of 0.16 atm . The system is then
compressed to half its volume. A)Find the pressure of I2 when the
system returns to equilibrium. Express your answer to two
significant figures and include the appropriate units.
i got 0.27 and was wrong
2)Solid carbon can react with gaseous water to form carbon
monoxide gas and hydrogen gas. The equilibrium constant for the
reaction...

1. A sample of gas occupies 5.27 L at a pressure of 2.63 atm.
Determine the new pressure (in atm) of the sample when the volume
changes to 4.56 L at constant temperature.
2. Determine the temperature (in °C) of a 4.77-mol sample of
CO2 gas at 6.11 atm in a container with a volume of 47.2
L.
3. Convert the pressure measurement of 2395 mmHg into units of
atmospheres.
4. A latex balloon has a volume of 87.0 L...

A weather balloon contains 222 L of He gas at 20. °C and 760.
mmHg. What is the volume of the balloon when it ascends to an
altitude where the temperature is -40. °C and 540. mmHg?
1
What volume does 12.5 g of Ar gas at a pressure of 1.05 atm and
a temperature of 322 K occupy? Would the volume be different if the
sample were 12.5 g of He gas under the same conditions?
How many moles...

1. A sample of methane gas (CH4) at 24.4 oC is either heated or
cooled. The pressure increases from 1.21 atm to 3.80 atm, and the
volume of the sample changes from 1.02 L to 4.61 L. To what
temperature, in oC, was the methane heated or cooled?
2. An effusion container is filled with 5 L of an unknown gas.
It takes 321 s for the gas to effuse into a vacuum. From the same
container under the same...

The density of acetone is 0.7899 g•cm-3. If 8.0 mL of acetone is
vaporized at 81.0 oC and atmospheric pressure, what would the
volume be in liters? (Do not include the units in your answer.
Report a numerical answer only with significant digits. Assume 2
significant digits in atmospheric pressure.)

The density of acetone is 0.7899 g•cm-3. If 8.0 mL of acetone is
vaporized at 81.0 oC and atmospheric pressure, what would the
volume be in liters? (Do not include the units in your answer.
Report a numerical answer only with significant digits. Assume 2
significant digits in atmospheric pressure.)

1) At standard temperature and pressure (0 ∘C and 1.00 atm ),
1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume
would the same amount of gas occupy at the same pressure and 45 ∘C
?
Express your answer with the appropriate units.
2) One mole of an ideal gas is sealed in a 22.4-L container at a
pressure of 1 atm and a temperature of 273 K. The temperature is
then increased to 304...

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