Question
In: Chemistry
1. The stopcock connecting a 1.00 L bulb containing krypton gas at a pressure of 414...
1. The stopcock connecting a 1.00 L bulb
containing krypton gas at a pressure of
414 mm Hg, and a 1.00 L bulb
containing oxygen gas at a pressure of
792 mm Hg, is opened and the gases are allowed to
mix. Assuming that the temperature remains constant, what is the
final pressure in the system?
mm Hg
2. A mixture of oxygen and
helium gases is maintained in a
5.33 L flask at a temperature of
13°C. If the partial pressure of
oxygen is 0.432 atm and the
partial pressure of helium is
0.314 atm, what is the total pressure in the
flask?
atm
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
The stopcock connecting a 4.10 L bulb containing krypton gas at a pressure of 4.80 atm,...
The stopcock connecting a 4.10 L bulb containing krypton gas at
a pressure of 4.80 atm, and a 3.21 L bulb containing carbon dioxide
gas at a pressure of 2.22 atm, is opened and the gases are allowed
to mix. Assuming that the temperature remains constant, the final
pressure in the system is _____atm
The stopcock connecting a 1.00 L bulb containing helium gas at a pressure of 554 torr,...
The stopcock connecting a 1.00 L bulb containing helium gas at a
pressure of 554 torr, and a 1.00 L bulb containing krypton gas at a
pressure of 504 torr, is opened and the gases are allowed to mix.
Assuming that the temperature remains constant, the final pressure
in the system is ____torr
If a 1.00 L flask containing 1.00 atm of SO2 is connected to a 4.00 L...
If a 1.00 L flask containing 1.00 atm of SO2 is connected to a
4.00 L flask containing 1.00 atm of O2, and the gases are allowed
to mix and react to form SO3 at 25°C, predict the total pressure
(PT) in the flask after the reaction is over
a. 1.10 atm
b.
0.300 atm
c.
0.900 atm
d.
0.200 atm
A 1.00 L sample of a gas at 25.0
A 1.00 L sample of a gas at 25.0
A sample containing 5.20 g 02 gas has a volume of 31.0 L . Pressure and...
A
sample containing 5.20 g 02 gas has a volume of 31.0 L . Pressure
and temp remain constant .
1- what is the new volume if O.300 mole O2 gas is added. V
=
2- what is the volume after 7.50 g he is added to the o2 gas
already in the container?
1.A sample of krypton gas occupies a volume of 7.55 L at 54.0°C and0.530 atm. If...
1.A sample of krypton gas occupies a volume of
7.55 L at 54.0°C
and0.530 atm.
If it is desired to decrease the volume of the
gas sample to 4.69 L,
whileincreasing its pressure to
0.710 atm, the temperature of the gas sample at
the new volume and pressure must be °C.
2.
A sample of krypton gas occupies a volume of
6.09 L at 64.0°C and
360.torr.
If the volume of the gas sample is decreased to
3.81 L, while...
Partial Pressure Question A. A mixture of krypton and oxygen gases, in a 9.68 L flask...
Partial Pressure Question
A. A mixture of krypton and
oxygen gases, in a 9.68 L flask
at 34 °C, contains 8.73 grams of
krypton and 8.09 grams of
oxygen. The partial pressure of
oxygen in the flask is ___ atm and the total
pressure in the flask is___ atm.
B.A mixture of argon and
helium gases is maintained in a
9.06 L flask at a pressure of
2.61 atm and a temperature of 71
°C. If the gas mixture contains...
A 5.00-L flask contains nitrogen gas at 25°C and 1.00 atm pressure. What is the final...
A 5.00-L flask contains nitrogen gas at 25°C and 1.00 atm
pressure. What is the final pressure in the flask if an additional
2.00 g of N2 gas is added to the flask and the flask cooled to
-55°C?
a.) 0.987 atm
b.) 1.35 atm
c.) 1.84 atm
d.) 0.255 atm
At 1.00 atm pressure and 273 K one mole of gas should occupy 22.4 L. What...
At 1.00 atm pressure and 273 K one mole of gas should occupy
22.4 L. What volume would one mole of gas occupy at 21
oC and 1.00 atm?
In the Molar Mass of Magnesium experiment:
a) At the end of the reaction, the temperature was 21.5
oC (294.65 K), 99.2 mL of gas were formed, and the
pressure was 1.00 atm in the gas syringe. The Gas Constant has a
value of 0.08206 L atm/ (mol K) (Pay attention...
1.00 moles of a gas is at a temperature of 273 Kelvin and has a pressure...
1.00 moles of a gas is at a temperature of 273 Kelvin and has a
pressure of 1.00x105Pa.
What is its initial volume?
STEP 1: Its pressure is doubled while keeping its volume
constant. What is its temperature after this step?
STEP 2: Its temperature is held constant while it it is reduced
back to its initial pressure. What is the the volume after this
step?
Draw a PV diagram showing the two step (it doesn’t have to have
numbers,...
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