Question

Part A) A certain amount of chlorine gas was placed inside a cylinder with a movable piston at one end. The initial volume was 3.00 L and the initial pressure of chlorine was 1.40 atm . The piston was pushed down to change the volume to 1.00 L. Calculate the final pressure of the gas if the temperature and number of moles of chlorine remain constant.

part B) In an air-conditioned room at 19.0 ∘C, a spherical balloon had the diameter of 50.0 cm. When taken outside on a hot summer day, the balloon expanded to 51.0 cm in diameter. What was the temperature outside in degrees Celsius? Assume that the balloon is a perfect sphere and that the pressure and number of moles of air molecules remains the same.

Part C) A cylinder with a movable piston contains 2.00 g of helium, He, at room temperature. More helium was added to the cylinder and the volume was adjusted so that the gas pressure remained the same. How many grams of helium were added to the cylinder if the volume was changed from 2.00 L to 3.70 L ? (The temperature was held constant.)

Answer #1

a)Since temperature and moles of chlorine remain constant gas law equation PV=nRT

gas law equation becomes P1V1= P2V2( since RHS, nRT remains constant)

P1= 1.4 atm , V1= 3L , V2=1L, P2=?

P2= P1V1/V2= 1.4*3/1 =4.2 atm

b) when pressure and number of moles remain constant, PV= nRT becones P is proportional to T

V1/T1= V2/T2

T1= 19 deg.c= 19+273.15= 292.15K

V1^{= (}4/3)*3.412*(50/2)^{3}
cm3 V2= (4/3)*3.412*(51/2)^{3}

T2=V2*T1/V1= (51/50)^{3} *292.15=310.13K

c) from PV=nRT

moles= mass/Molecular weight =2/4 =0.5

V_{1}/n_{1}= V_{2}/n_{2} ( since
P and T remained constant)

n2= V2*n1/V1= (3.7/2)*0.5 =0.925 moles

Mass of helium =0.925*4= 3.7 gms

A certain amount of chlorine gas was placed inside a cylinder
with a movable piston at one end. The initial volume was 3.00 L and
the initial pressure of chlorine was 1.64 atm . The piston was
pushed down to change the volume to 1.00 L. Calculate the final
pressure of the gas if the temperature and number of moles of
chlorine remain constant.
Enter a numerical answer only, in terms of
atm.
Please show all work

A cylinder with a movable piston contains 2.00 g of helium, He,
at room temperature. More helium was added to the cylinder and the
volume was adjusted so that the gas pressure remained the same. How
many grams of helium were added to the cylinder if the volume was
changed from 2.00 L to 2.526 L ? (The temperature was held
constant.)
Enter your answer in units of grams.
Please show all work

Consider 4.30 L of a gas at 365 mmHg and 20. ∘C . If the
container is compressed to 2.90 L and the temperature is increased
to 32 ∘C , what is the new pressure, P2, inside the container?
Assume no change in the amount of gas inside the cylinder.
What pressure would it take to compress 250. L of helium gas
initially at 1.00 atm into a 2.00 L tank at constant
temperature?
A balloon filled with 2.00 L...

A 6.0-cm-diameter cylinder of nitrogen gas has a 4.0-cm-thick
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shown in the figure, and the air above the piston is evacuated.
When the gas temperature is 15 ∘C , the piston floats 20cm above
the bottom of the cylinder.
A. What is the gas pressure?
B. How many gas molecules are in the cylinder?
C. Then 1.5 JJ of heat energy are transferred to the
gas. What is the new equilibrium temperature...

A quantity of air is contained in a cylinder provided
with a movable piston. Initially the
pressure of the air is 4 × 107 N/m2
, the volume is 1.5 m3
and the temperature is 400 K.
Assume air is an ideal gas. (a) What are the final volume and
temperature of the air if it is
allowed to expand isothermally from initial conditions until the
pressure is 3 × 107 N/m2
and
then is cooled at constant volume until...

1. A sample of gas in a cylinder as in the example in Part A has
an initial volume of 48.0 L , and you have determined that it
contains 1.20 moles of gas. The next day you notice that some of
the gas has leaked out. The pressure and temperature remain the
same, but the volume has changed to 12.0 L . How many moles of gas
(n2) remain in the cylinder? Express your answer with the
appropriate units....

Part A
Consider 4.30 L of a gas at 365 mmHg and 20. ∘C . If the
container is compressed to 2.70 L and the temperature is increased
to 30. ∘C, what is the new pressure, P2, inside the
container? Assume no change in the amount of gas inside the
cylinder.
Express your answer with the appropriate units.
Part B
A cylinder, with a piston pressing down with a constant
pressure, is filled with 2.00 moles of a gas (n1),...

An ideal gas is enclosed in a cylinder with a movable piston on
top of it. The piston has a mass of 8,000 g and an area of 5.00
cm2 and is free to slide up and down, keeping the
pressure of the gas constant.
(a) How much work is done on the gas as the temperature of 0.155
mol of the gas is raised from 30.0°C to 330°C?
_______ J

Part A
A balloon is floating around outside your window. The
temperature outside is -11 ∘C , and the air pressure is 0.700 atm .
Your neighbor, who released the balloon, tells you that he filled
it with 4.90 moles of gas. What is the volume of gas inside this
balloon?
Part B
A 10.0 L gas cylinder is filled with 5.60 moles of gas. The tank
is stored at 25 ∘C . What is the pressure in the tank?...

A cylinder, with a piston pressing down with a constant
pressure, is filled with 2.00 moles of a gas (n1), and its
volume is 49.0 L (V1). If 0.500 mole of gas leak out, and
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