For the reaction shown here: COCl2 (g) --> CO (g) + Cl2 (g)
has a standard Gibb's Free Energy of -12.5 kJ. For each change
listed below, indicated how it would affect the spontaneity of the
reaction.
Remove CO
Add Cl2
Increase the temperature
Increase pressure
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For the reaction shown here: COCl2 (g) --> CO (g) + Cl2 (g) has a standard...
6 4 points For the reaction shown here: COCI, () --> CO(g) + Cl2 (8) has a standard Gibb's Free Energy of -12.5 kJ. For each change listed below, indicated how it would affect the spontaneity of the reaction. Remove CO Add C12 Increase the temperature Increase Spontaneity Decrease Spontaneity Increase Spontaneity Decrease Spontaneity Increase Pressure
Consider the reaction CO(g) + Cl2(g)---COCl2(g) Use the standard thermodynamic data in the tables linked above. Calculate delta G for this reaction at 298.15K if the pressure of COCl2(g) is reduced to 20.15 mm Hg, while the pressures of CO(g) and Cl2(g) remain at 1 atm. ANSWER: kJ/mol Consider the reaction 2SO2(g) + O2(g)----2SO3(g) Using the standard thermodynamic data in the tables linked above, calculate delta Grxn for this reaction at 298.15K if the pressure of each gas is 25.11...
1. Consider the reaction at equilibrium: CO(g) + Cl2(g) COCl2(g). Predict how addition of CO(g) will affect the equilibrium system. 2. What would be the net effect of decreasing the temperature on the following exothermic reaction? 3. What is the effect on the following equilibrium system if CaO(s) is added? 4. Consider the reaction at equilibrium. CO(g) + Cl2(g) ⟷ COCl2(g) Predict how addition of CO(g) will affect the equilibrium system. Please help explain the answers to these!
The system described by the reaction CO(g) + Cl2 (g) = COCl2 (g) is at equilibrium at a given temperature when Pco = 0.32 atm , Pci, = 0.12 atm , and Pcoci, = 0.58 atm . An additional pressure of Cl2 (g) = 0.41 atm is added. Part A Find the pressure of CO when the system returns to equilibrium. Express your answer using two significant figures. O ALQ * R 0 2 ? P= atm Submit Previous Answers...
The system described by the reaction CO(g)+Cl2(g)⇌COCl2(g) is at equilibrium at a given temperature when PCO= 0.30 atm, PCl2= 0.11 atm, and PCOCl2=0.58 atm. An additional pressure of Cl2(g)== 0.42 atm is added. Find the pressure of CO when the system returns to equilibrium.
The equilibrium constant in terms of pressures for the reaction COCl2(g) <--> CO(g) + Cl2(g) is Kp = 5.00 at 873 K. (a) A pure sample of gaseous phosgene, COCl2(g), is introduced into a rigid flask at a temperature of 873 K so that its original pressure is 0.121 atm. Calculate the fraction of this starting material that is converted to products at equilibrium. (b) A second sample of phosgene is introduced into a rigid flask at a temperature of...
1) At 100 oC, Keq = 1.5E8 for the reaction: CO(g) + Cl2(g) COCl2(g) Using appropriate approximation, calculate the partial pressure of CO at 100 oC at equilibrium in a chamber that initially contains COCl2 at a pressure of 0.293 bar.
Consider the reaction described by this equation: COCl2 (g) ⇌ CO (g) + Cl2 (g) If 2.00 mol of COCl2 (g) is introduced into a 10.0 L flask at 1000°C, calculate the equilibrium concentrations of all chemical species at this temperature. K = .329 at 1000°C.
Consider the following reaction: COCl2(g) = CO(g) + Cl2(8) A reaction mixture initially contains 1.6 M COC12. Determine the equilibrium concentrations of COCI, CO, and Cl2 if Kc for the reaction at this temperature is 8.33 x 10-4. Calculate this based on the assumption that the answer is negligible compared to 1.6. Use x is small approximation. Show Q Validity check [Cl2] = [CO]= [COCI2] = Calculate the reaction quotient, Q A % Validity Check A Calculate the A/ equilibrium...
1) For the following reaction: SO2Cl2(g)<-> SO2(g) + Cl2 (g) Kp=2.91x10^3 at 298K In the reaction at equilibrium, the partial pressure of SO2 is 137 torr and that of CL2 is 285 torr. The partial pressure of SO2Cl2 is [x]torr. 2) For the following reaction:NH4HS(s)<->NH3(g) + H2S (g) Kc=8.5x10^-3 At any given point the reaction mixture has solid NH4HS, NH3 at 0.166M and H2S at 0.166M. a) Is the reaction at equilibrium? b)Will more of the solid form, or will...