Question

In: Chemistry

Consider the following reaction: COCl2(g) CO(g) + Cl2(g) If 6.56×10-3 moles of COCl2, 0.377 moles of...

Consider the following reaction: COCl2(g) CO(g) + Cl2(g) If 6.56×10-3 moles of COCl2, 0.377 moles of CO, and 0.372 moles of Cl2 are at equilibrium in a 16.9 L container at 772 K, the value of the equilibrium constant, Kp, is

2.A student ran the following reaction in the laboratory at 597 K:

COCl2(g) CO(g) + Cl2(g)

When she introduced COCl2(g) at a pressure of 0.710 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of COCl2(g) to be 0.299 atm.  

Calculate the equilibrium constant, Kp, she obtained for this reaction.  

Solutions

Expert Solution

Dear student,

Please give a positive rating if satisfied with the answer.


Related Solutions

Consider the following reaction where Kp = 1.57 at 600 K: CO(g) + Cl2(g) COCl2(g) If...
Consider the following reaction where Kp = 1.57 at 600 K: CO(g) + Cl2(g) COCl2(g) If the three gases are mixed in a rigid container at 600 K so that the partial pressure of each gas is initially one atm, what will happen? Indicate True (T) or False (F) for each of the following: 1. A reaction will occur in which COCl2(g) is produced 2. Kp will decrease. 3. A reaction will occur in which CO is produced. 4. Q...
Consider the following reaction at equilibrium: CO(g)+Cl2(g)⇌COCl2(g) Part A Predict whether the reaction will shift left,...
Consider the following reaction at equilibrium: CO(g)+Cl2(g)⇌COCl2(g) Part A Predict whether the reaction will shift left, shift right, or remain unchanged if COCl2 is added to the reaction mixture. Predict whether the reaction will shift left, shift right, or remain unchanged if  is added to the reaction mixture. -shifts left -shifts right -remains unchanged Part B Predict whether the reaction will shift left, shift right, or remain unchanged if Cl2 is added to the reaction mixture. Predict whether the reaction will...
Phosphine decomposes by the following reaction: COCl2(g) <---> CO(g) + Cl2(g) Kc = 8.3 x 10-4...
Phosphine decomposes by the following reaction: COCl2(g) <---> CO(g) + Cl2(g) Kc = 8.3 x 10-4 Calculate the concentration of each component when 2.55 g of phosphine decomposes in a 25.0mL flask.
At 100.0 C, the equilibrium constant for the reaction: CO (g) + Cl2 (g) <--> COCl2...
At 100.0 C, the equilibrium constant for the reaction: CO (g) + Cl2 (g) <--> COCl2 (g) has a value of 4.6 x 109. If 0.40 mol of COCl2 is placed into a 10.0 L flask at 100.0 C, what will be the equilibrium concentration of all species? (A simplifying approximation that will make the solution of the resulting equation easier is to note that x is much less than 0.040mol/L. This means that 0.040 -x is approximately 0.040.)
A student ran the following reaction in the laboratory at 610 K: CO(g) + Cl2(g) COCl2(g)...
A student ran the following reaction in the laboratory at 610 K: CO(g) + Cl2(g) COCl2(g) When she introduced 0.183 moles of CO(g) and 0.211 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of Cl2(g) to be 6.72×10-2 M.   Calculate the equilibrium constant, Kc, she obtained for this reaction. 2.A student ran the following reaction in the laboratory at 546 K: COCl2(g) CO(g) + Cl2(g)   When she introduced 0.854 moles of COCl2(g) into a 1.00...
For the following reaction Kc = 2.20 ✕ 102 at 74°C. CO(g) + Cl2(g) ↔ COCl2(g)...
For the following reaction Kc = 2.20 ✕ 102 at 74°C. CO(g) + Cl2(g) ↔ COCl2(g) Find the equilibrium concentrations of all chemical species starting with [CO] = 0.105 M and [Cl2] = 0.105 M. [CO] = M [Cl2] = M [COCl2] = M
For the following reaction Kc = 2.20 ✕ 102 at 74°C. CO(g) + Cl2(g) ↔ COCl2(g)...
For the following reaction Kc = 2.20 ✕ 102 at 74°C. CO(g) + Cl2(g) ↔ COCl2(g) Find the equilibrium concentrations of all chemical species starting with [CO] = 0.179 M and [Cl2] = 0.287 M. [CO] = M [Cl2] = M [COCl2] = M
For the following reaction, Kc = 255 at 1000 K. CO(g)+Cl2(g)⇌COCl2(g) A reaction mixture initially contains...
For the following reaction, Kc = 255 at 1000 K. CO(g)+Cl2(g)⇌COCl2(g) A reaction mixture initially contains a COconcentration of 0.1470 M and a Cl2concentration of 0.173 M at 1000 K A)What is the equilibrium concentration of COat 1000 K? B)What is the equilibrium concentration of Cl2 at 1000 K? C)What is the equilibrium concentration of COCl2 at 1000 K?
For the following reaction, Kc = 255 at 1000 K. CO(g)+Cl2(g)⇌COCl2(g) A reaction mixture initially contains...
For the following reaction, Kc = 255 at 1000 K. CO(g)+Cl2(g)⇌COCl2(g) A reaction mixture initially contains a CO concentration of 0.1490 M and a Cl2concentration of 0.180 M at 1000 K. a) What is the equilibrium concentration of CO at 1000 K? b) What is the equilibrium concentration of Cl2 at 1000 K? c ) What is the equilibrium concentration of COCl2 at 1000 K?
part a the reaction COCl2(g)<-->CO(g)+Cl2(g) has an equilibrium constant Kc=2.19*10^-10 at 100 degree celcius. is the...
part a the reaction COCl2(g)<-->CO(g)+Cl2(g) has an equilibrium constant Kc=2.19*10^-10 at 100 degree celcius. is the following mixture at equilibrium, and if not, which direction must it shift to reach equilbrium? [COCl2]=3.30*10^-3 M, [CO]=6.2*10^-9 M, [Cl2]=2.00*10^-9 M part b when additional lead ions are added to a saturated solution of PbSO4, which direction will the reaction shift? part c what is the pH of a 0.015 M solution of NaOH? part d the reaction 2SO2(g)+O2(g)<-->2SO3(g) has an equilibrium constant, Kp=0.345...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT