Question
In: Chemistry
1.The total pressure of a mixture of O2(g) and H2(g) is 1.95 atm. The mixture is...
1.The total pressure of a mixture of O2(g) and H2(g) is 1.95 atm. The mixture is ignited and the resulting water is removed. The remaining mixture is pure H2(g) and exerts a pressure of 0.210atm when measured at the same temperature and volume as the original mixture. What were the mole fractions of O2(g) and H2(g) in the original mixture?
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
A mixture of H2(g) and O2 (g) at 1.50 atm in a rigid container at temperature...
A mixture of H2(g) and O2 (g) at 1.50 atm
in a rigid container at temperature T is ignited. The remaining
gas, which is entirely H2 (g) exerts a pressure of 0.30
atm at tempertaure T. Assume that the gases are ideal and the
H2O(l) formed in the combustion reaction
takes up negligible volue in the container. Determine the mole
fraction of O2(g) in the original mixture.
A mixture of H2(g) and O2 (g) at 1.50 atm in a rigid container at temperature...
A mixture of H2(g) and O2 (g) at 1.50 atm
in a rigid container at temperature T is ignited. The remaining
gas, which is entirely H2 (g) exerts a pressure of 0.30
atm at tempertaure T. Assume that the gases are ideal and the
H2O(l) formed in the combustion reaction
takes up negligible volue in the container. Determine the mole
fraction of O2(g) in the original mixture.
A mixture of CH4 (g) and C2H6 (g) has a total pressure of 0.53 atm. Just...
A mixture of CH4 (g) and C2H6 (g) has a total pressure
of 0.53 atm. Just enough O2 was added to the mixture to bring about
it's complete combustion to CO2 (g) and H2O (g). The total pressure
of the two product gases is found to be 2.2 atm. Assuming constant
volume and temperature, find the mole fraction of CH4 in the
original mixture.
A mixture of CH4 (g) and C2H6 (g) has a total pressure of 0.53 atm. Just...
A mixture of CH4 (g) and C2H6 (g) has a total pressure
of 0.53 atm. Just enough O2 was added to the mixture to bring about
it's complete combustion to CO2 (g) and H2O (g). The total pressure
of the two product gases is found to be 2.2 atm. Assuming constant
volume and temperature, find the mole fraction of CH4 in the
original mixture.
A mixture containing N2O4, N2O, and O2, all at an initial partial pressure of 4.60 atm,...
A mixture containing N2O4, N2O,
and O2, all at an initial partial pressure of 4.60 atm,
is allowed to achieve equilibrium according to the equation below.
At equilibrium, the partial pressure of O2 is observed
to have decreased by 0.28 atm. Determine Kp for this
chemical equilibrium. Report your answer to 3 significant figures
in scientific notation.
2N2O4(g) ⇌ 2N2O(g) +
3O2(g)
A mixture containing N2O4, N2O, and O2, all at an initial partial pressure of 4.60 atm,...
A mixture containing N2O4, N2O,
and O2, all at an initial partial pressure of 4.60 atm,
is allowed to achieve equilibrium according to the equation below.
At equilibrium, the partial pressure of O2 is observed
to have decreased by 0.28 atm. Determine Kp for this
chemical equilibrium. Report your answer to 3 significant figures
in scientific notation.
2N2O4(g) ⇌ 2N2O(g) +
3O2(g)
H2O(l)+40.7kJ->H2O(g) Assume at exactly 100.0°C and 1.00 atm total pressure, 1.00 mole of liquid water and...
H2O(l)+40.7kJ->H2O(g) Assume at exactly 100.0°C and 1.00
atm total pressure, 1.00 mole of liquid water and 1.00 mole of
water vapor occupy 18.80 mL and 30.62 L, respectively.
Part 1: Calculate the work done on or by the system when 3.25
mol of liquid H2O vaporizes. ____J
Part 2: Calculate the water's change in internal energy.
____kJ
A tank, containing O2 and H2, has a volume of 4.00 L and at total pressure...
A tank, containing O2 and H2, has a volume of 4.00 L and at
total pressure is 24.44 atm. Calculate the mass of oxygen of which
mole fraction is 0.4 in the tank at 25.0 °C .
A mixture of CO2 and Kr weighs 41.0 g and exerts a pressure of 0.729 atm...
A mixture of CO2 and Kr weighs 41.0 g and exerts a pressure of
0.729 atm in its container. Since Kr is expensive, you wish to
recover it from the mixture. After the CO2 is completely removed by
absorption with NaOH(s), the pressure in the container is 0.193
atm. (a) How many grams of CO2 were originally present? (b) How
many grams of Kr can you recover?
PART A A mixture of He, Ar, and Xe has a total pressure of 2.20 atm...
PART A
A mixture of He, Ar, and Xe has a total pressure of 2.20 atm .
The partial pressure of He is 0.400 atm , and the partial pressure
of Ar is 0.450 atm . What is the partial pressure of Xe? Express
your answer to three significant figures and include the
appropriate units.
PART B
A volume of 18.0 L contains a mixture of 0.250 mole N2 , 0.250
mole O2 , and an unknown quantity of He....
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