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In: Chemistry
An equalibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has partial pressures of 217.0 Torr, 13.2 Torr,...
An equalibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr, respectively. A quantity of Cl2(g) is injected into the mixture, and the total pressure jumps to 263.0 Torr. The appropriate chemical equation is PCl3(g) + Cl2(g) forward and reverse arrows PCl5(g)
Calculate the new partial pressures after equilibrium is reestablished.
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has partial pressures of 217.0 Torr, 13.2 Torr,...
An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has
partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr,
respectively. A quantity of Cl2(g) is injected into the mixture,
and the total pressure jumps to 263.0 Torr (at the moment of
mixing). The system then re-equilibrates. The appropriate chemical
equation is
PCl3(g) + Cl2(g) <---> PCl5(g)
Calculate the new partial pressures after equilibrium is
reestablished.
P PCl3 = ? torr
P PCl2 = ? torr
P PCl5 = ? torr
An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has partial pressures of 217.0 Torr, 13.2 Torr,...
An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has
partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr,
respectively. A quantity of Cl2(g) is injected into the mixture,
and the total pressure jumps to 263.0 Torr (at the moment of
mixing). The system then re-equilibrates. The appropriate chemical
equation is PCl3(g)+Cl2(g) <---> PCl5(g)
Calculate the new partial pressures after equilibrium is
reestablished. Answers in Torr
Phosphorus pentachloride decomposes at higher temperatures. PCl5(g) ⇄ PCl3(g) + Cl2(g) An equilibrium mixture at some...
Phosphorus pentachloride decomposes at higher temperatures.
PCl5(g) ⇄ PCl3(g) + Cl2(g)
An equilibrium mixture at some temperature consists of
3.03 g PCl5, 208.23 g/mol
4.86 g PCl3, 137.33 g/mol
3.59 g Cl2, 70.91 g/mol
in a 1.00-L flask.
If you add 1.31 g of Cl2, how will the equilibrium be
affected and what will the concentration of PCl5 be when
equilibrium is reestablished?
shift left
shift right
no shift will occur
[PCl5] = mol/L
Phosphorus pentachloride decomposes at higher temperatures. PCl5(g) ⇄ PCl3(g) + Cl2(g) An equilibrium mixture at some...
Phosphorus pentachloride decomposes at higher
temperatures.
PCl5(g) ⇄ PCl3(g) + Cl2(g)
An equilibrium mixture at some temperature consists of
5.93 g PCl5, 208.23 g/mol
4.86 g PCl3, 137.33 g/mol
3.59 g Cl2, 70.91 g/mol
in a 1.00-L flask.
If you add 1.31 g of Cl2, how will the equilibrium be affected
and what will the concentration of PCl5 be when equilibrium is
reestablished?
shift left
shift right
no shift will occur
[PCl5] = mol/L
The reaction: PCl5(g) <-> PCl3(g) + Cl2(g) has Kc=0.0900. A 0.1000 mol sammple of PCl5 is...
The reaction: PCl5(g) <-> PCl3(g) +
Cl2(g) has Kc=0.0900. A 0.1000 mol sammple of
PCl5 is placed in an empty 1.00 flask and the above
reaction is allowed to come to equilibrium at a certain temp. How
manny moles of PCl5, PCl3 and Cl2,
respectively, are present at equilibrium?
For the equilibrium PCl5(g) PCl3(g) + Cl2(g), Kc = 4.0 at 228°C. If pure PCl5 is...
For the equilibrium PCl5(g) PCl3(g) + Cl2(g), Kc = 4.0 at 228°C.
If pure PCl5 is placed in a 1.00-L container and allowed to come to
equilibrium, and the equilibrium concentration of PCl5(g) is 0.26
M, what is the equilibrium concentration of PCl3?
The reaction below is exothermic: PCl3 (g) + Cl2 (g) <---> PCl5 (g) Which change will...
The reaction below is exothermic: PCl3 (g) + Cl2 (g) <--->
PCl5 (g) Which change will increase the number of moles of of PCl5
(g) present?
A. The volume of the reaction vessel is tripled
B. The reaction vessel is cooled
C. Some of the Cl2 is removed
D. Krypton gas is added to the reaction vessel
What is the percent yield for the reaction PCl3(g) + Cl2(g) --> PCl5(g) if 119.3 g...
What is the percent yield for the reaction PCl3(g)
+ Cl2(g)
--> PCl5(g)
if 119.3 g of PCl5
are formed when 61.3 g of Cl2
reacts with 125.5g PCl3?
Gaseous phosphorus pentachloride decomposes according to the reaction PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)...
Gaseous phosphorus pentachloride decomposes according to the
reaction
PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)
The equilibrium system was analyzed at a particular temperature,
and the concentration of the substances present were determined to
be [PCl5] = 1.1 x10-2 M, [PCl3] = 0.325 M, and [Cl2] = 3.9 x 10-3
M. Calculate the value of K for the reaction.
The equilibrium constant K=0.36 for the reaction PCl5 (g) PCl3 (g) +Cl2 (g). (a) Given...
The equilibrium constant K=0.36 for the reaction PCl5 (g)
PCl3 (g) +Cl2 (g). (a) Given that 2.0 g of PCl5 was initially
placed in the reaction chamber of volume 250 cm3, determine the
molar concentration in the mixture at equilibrium. (b) What is the
percentage of PCl5 decomposed.
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