If I have the equilibrium constant for a reaction, how do I figure out the partial pressures of the components? Help! equilibrium constant for COCL2 is 4.63 x e-3 at 527 degree centrigrade COCL2(g)=CO(g) + CL2(g) at 0.760 atm how do I find the partial pressures in atm?
Chemistry is hard for me. Could you show me how to set up this problem? Thank you. At 700 degree C calculate the equilibrium for the reaction 2 H2(g) + S2(g)= 2 H2S(g) 2.50 moles of H2 1.35 x e-5 moles S2 8.70 moles of H2S in a 12.0 liter container
Can you show me how to set up the equation? What is the equilibrium constant if the equilibrium concentrations at 74 degrees centigrade to form carbonyl chloride are [CO]=1.2 x e-2 M [Cl2]=0.054 M [COCl2]= 0.14M CO(g) + Cl2(g)= COCl2(g)
Nitrozil bromide decomposes according to the following equation: 2NOBr(g) <--> 2NO(g)+ Br2(g) Kc=.600 At equilibrium 4.68 mol NOBr is present in a 1.00L flask. a. How much NO(g) and Br2 are present at equilibrium if initially only NOBr(g) was introduced? b. What was the initial concentration of NOBr in the flas
At a particular temperature, K = 3.75 for the following reaction. SO2(g) + NO2(g)<---> SO3(g) + NO(g) If all four gases had initial concentrations of 0.710 M, calculate the equilibrium concentrations of the gases. [SO3] M [NO] M [SO2] M [NO2] M
The solution calculates Ke for the following..the equilibrium concentration is below each. a)4 NH3 (g) + 3 O2 (g) ↔ 2 N2 (g) + 6 H2O g) + heat [0.010 [0.10] [0.0794] [0.10] b)N2 (g) + 3 H2 (g) + heat ↔ 2 NH3 (g) = (34...i think) [0.103] [0.240
1. The following data were collected for the rate of disappearance of NO in the reaction 2NO(g)+O2(g)-----> 2NO2(g) Experiment [NO](M) [O2](M) Initial Rate(M/s) 1 0.0126 0.0125 1.41 x 10^-2 2 0.0252 0.0250 1.13 x 10^-1 3 0.0252 0.0125 5.64 x 10^-2 a
At 700 K the equilibrium constant for the reaction is CCl4 (g) <--> C (s) + 2 Cl2 (g) is Kp = 0.76. A flask is charged with 2.00 atm of CCl4, which then reaches equilibrium at 700 K. a) What fraction of CCl4 is converted into C and Cl2? b) What are the partial pressures of CCl4 and Cl2 at equilibrium?
Hey there. I'm having problems with this question. Consider the following equilibrium, for which Kp = 0.0752 at 480 *C (degrees Celsius): 2 Cl2 (g) + 2 H2O (g) <--> 4 HCl (g) + 02 (g) a) What is the value of Kp for the reaction of 4 HCl (g) + 02 (g) <--> 2 Cl2 (g) + 2 H2O (g)? b) What is the value of Kp for the reac
108. Consider a solution that is .022M in Fe2+ and .014M in Mg2+ a. if potassium carbonate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? What minimum concentration of K2CO3 is required to cause the precipitation of the cation that precipita
Can you provide an example of a chemical reaction in dynamic equilibrium. What factors affect the equilibrium of the reaction provided. Why is it important to study chemical equilibrium? In what industries might such knowledge be particularly useful?
Consider this reaction: 2HI <--> H2 + I2 One mole of hydrogen iodide was placed in a reaction vessel and allowed to come to equilibirum. It was found that 0.2 mole of hydrogen iodide was left in the equilibrium mixture. Calculate Kc. 2HI <--> H2 + I2 Initial no. moles 1 <--> 0 0 Equil
Hi: We are given the following: zinc sulfate (solubility given as 96.5 g/100 ml's) zinc hydroxide ---- given Ksp = 2.1 x 10^-16 zinc sulfide ---- given Ksp = 1.1 x 10^-21 We are asked to calculate the Ksp for zinc sulfate and then asked to convert the Ksp's for zinc hydroxide and zinc sulfide into grams/100 ml uni
Describe why addition of a catalyst does not affect the equilibrium constant for a reaction. Response needs to be in a 200-300 word essay form.
The dissociation of solid silver chloride in water to produce silver ions and chloride ions has an equilibrium constant of 1.8 x10-18. Based on the magnitude of the equilibrium constant, is silver chloride very soluble in water? Explain your answer. Response needs to be in a 200-300 word essay response.
1, Calculate Ke for the following (equilibrium concentrations given below substances) a) PCl5 (g) + heat ↔ PCl3 (g) + Cl2 (g) [0.105] [0.219] [0.219] b) 2 SO2 (g) + O2 (g) ↔ 2 SO3 (g) + heat [0.0500] [0.0500] 0.103] c) CO2 (g) +
Consider the reaction by which silver chloride dissolves in ammonia: AgCl(s) + 2NH3 --> Ag(NH3)2^+(aq) + Cl^-(aq) (a) Taking Ksp AgCl = 1.8*10^-10 and Kf Ag(NH3)2^+ =1.7*10^7 , calculate K for this reaction.
Kp = 7.69 at 830C for 2SO3 = 2SO2 + O2. If a vessel at this temperature initially contained pure sulfur dioxide and if the partial pressure of sulfur trioxide = 0.100 atm, what is the partial products in the flask at equilibrium.
A mixture of 0.20 mol of CO2, 0.10 mol of H2, AND 0.16 mol of H20 is placed in a 2.0L reaction vessel. The following equilibrium is established at 500 K: CO2 + H2 = CO + H2O At equilibrium P of H2O is 3.51 atm. a) Calculate partial pressure for CO2, H2 and CO b) Calculate equilibrium constant for this reaction.
Given the following information: H2S (aq) <-> H+ (aq) + HS- (aq) K= 8.9 x 10^-8 H+ (aq) + S2- (aq) <-> HS- (aq) K= 8.3 x 10^12 determine the equilibrium constant for the reaction: H2S (aq) <-> 2 H+ (aq) + S2- (aq)
The equation is: 2CrO4(2-) (yellow) + 2H3O(+) = Cr2O7(2-) (orange) + 3H2O when adding HCl to the mixure - the color will become darker - chromate ions will react w/ the hydronium ion to form the orange color Now add salt to the above mixture - what will the color be (the mixture with the HCl) and explain your answer using L
1. For a certain chemical reaction, H= -156 kJ. Assuming the reaction is at equilibrium, classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction. a. a decrease in temperature R L no shift b. an increase in tempera
Part 1: Ammonia can be produced by the reaction of hydrogen gas and nitrogen gas, as shown below: N2(g) + 3H2(g) → 2NH3(g) Given that the standard free energy of formation (∆Gof) of NH3 (g) is -111 kJ/mol at 335 K, calculate the equilibrium constant, K, at this temperature. To express an answer in exponential
Calculate Keq for the following (equilibrium concentrations given below substances) a) 2 O3 (g) ↔ 3 O2 (g) + heat [6.0 x 10-1] [0.21] b) 2 CO2 (g) + heat ↔ 2 CO (g) + O2 (g) [0.103] [0.024] [1.18 x 10-2] c) NO2 (g) + O2 (g) +
Question 13 Phosgene (COCl2) is an extremely poisonous gas that was used extensively in World War I as a chemical warfare agent. At 300oC, phosgene decomposes to carbon monoxide and chlorine with a Kp = 6.8 x 10-2. Calculate the pressure in the vessel at equilibrium after placing 5.00 grams of pure phosgene in a 1.00 litre reac
Will a precipitate form when 250 ml of 0.33 M Na2CrO4 are added to 250 ml 0.12 M AgNO3 ? (Ksp Ag2CrO4= 1.1 e-12) What is the concentration of the silver ion remaining in solution?
If 2.50 gm of CuSO4 is dissolved in 9.0 X 10 to the 2nd mlof 0.30 M NH3, what are the concentrations of CU+2 Cu(NH3)4 NH3 at equilibrium?
Consider the following equilibrium process at 686°C: CO2(g) + H2(g) CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.050 M, [H2] = 0.045 M, [CO2] = 0.086 M, and [H2O] = 0.040 M. (a) Calculate Kc for the reaction at 686°C. (I got Kc=.52 which is correct but now I don't know how to d
The Kc for HBr(g) breaking into Br2 and H2 is 2.18 e 6 at 760 degrees C. If we start with 2.50 moles in a 12.0 Liters reaction vessel calculate the concentrations of H2, Br2 and HBr at equilibrium. Could you show me how to set up the problem?
A 6.1589 gm sample of ammonium hydrogen sulfide is placed in a 4.00L vessel at 24 degrees Celsius. After equilibrium the total pressure inside is 0.709 atm. Some solid ammonium hydrogen sulfide remains. What is the Kp for the reaction? What percentage of the solid has decomposed? If the volume of the vessel were doubl