A mixture of 0.734 atm ClF3 , 0.436 atm F2 , and 0.482 atm ClF
is heated in a closed vessel to 700 K .
ClF3(g)↽−−⇀ClF(g)+F2(g)?p=0.140 at 700 K Calculate the equilibrium
pressure of each gas at 700 K. Are you able to break this question
down as much as possible please? Thank you so much because I am
really struggling.
A mixture of 0.750 mol H2 and 0.750 mol I2
was placed in a 1.00 L flask at 430°C. The equilibrium constant
Kc for the reaction is 54.3 at this temperature.
Calculate the concentration of H2, I2, and HI
at equilibrium.
H2
+ I2
⇌
2 HI
Chlorine gas reacts with fluorine gas to form chlorine
trifluoride. Cl 2 (g)+3 F2 (g)→2 ClF 3 (g) A 2.20 L reaction
vessel, initially at 298 K , contains chlorine gas at a partial
pressure of 337 mmHg and fluorine gas at a partial pressure of 793
mmHg .
Part A
Identify the limiting reactant and determine the theoretical
yield of ClF3 in grams.
Express your answer with the appropriate units.
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?
A mixture of isobutylene (0.350 atm partial pressure at 500 K)
and HCl(0.550 atm partial pressure at 500 K) is allowed to reach
equilibrium at 500 K. What are the equilibrium partial pressures of
tert-butyl chloride, isobutylene, and HCl?
The equilibrium constant KpKp for the gas-phase thermal
decomposition of tert-butyl chloride is 3.45 at 500
K:
(CH3)3CCl(g)⇌(CH3)2C=CH2(g)+HCl(g)
a) clculate the partial pressure (in atm) of Ne and Ar in the
container. gas mixture in a 1.45 L at 298 K container contains 10.0
g of Ne and 10.0 g of Ar. Calculate the partial pressure (in ) of
and in the container.
PNe = 4.22 atm , PAr = 4.22 atm
PNe = 8.36 atm , PAr = 4.22 atm
PNe = 8.36 atm , PAr = 8.36 atm
PNe = 4.22 atm , PAr = 8.36...
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 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.
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....
Part A
A mixture of He, Ar, and Xe has a total pressure of 2.70 atm .
The partial pressure of He is 0.450 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....