Consider the following Decomposition Reaction: C5H6O3(g) = C2H6(g) + 3 CO(g) When a 5.63g sample of pure C5H6O3(g) was sealed into an otherwise empty 2.50L flask and heated to 200C, the pressure in the flask gradually rose to 1.63 atm and remained at that value. Calculate K for this reaction.
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
HOBr(aq) ----> H+(aq) + OBr-(aq) Ka = 2.3 x 10-9 1. Hydrobromous acid, HOBr, is a weak acid that disassociates in water, as represented by the equation above. (a) Calculate the value of [H+] in a HOBr solution that has pH of 4.95. (b) Write the equilibrium constant expression for the ionization of the HOBr in water,
5. In a saturated solution of MgF2 at 18C , the concentration of Mg2+ is 1.21 x 10-3 molar. The equilibrium is represented by the equation below MgF2(s) ---> Mg2+ (aq) + 2F- (aq) A) write the expression for the solubility product , Ksp , and calculate its value at 18C B) predict whether a precipitate of MgF2 will fo
If the following data is "true": H3PO4(aq)<--> H^+(aq) + H2PO4^-(aq) ...... .Ka1 = 7.5x10^-3 H2PO4^-(aq)<--> H+(aq) + HPO4^-2(aq) .............Ka2 = 6.2x10^-8 HPO4^-2(aq) <--> H+(aq) + HPO4^-3(aq) ............Ka3 = 4.8x10^-13 What is Ka for the reaction H3PO4(aq) <--> 3H^+(aq) + PO4^-3(aq)?
Answer the Questions based on Ag2CrO4 (Silver Chromate) and Ag3PO4 . Silver Chromate dissociates in water according to the equation. Ag2CrO(s)<->2Ag+ CrO4 Ksp= 2.6x10^-12 at 25 deg C. a) Write the equilibrium constant expression for Ag2CrO4 (Silver Chromate) b) Calculate the concentration, in mol L-1 of Ag in a saturated so
Consider the equilibrium: 3A <----> B You prepare a mixture with initial concentrations [A]0 = 0.61 mol/L, and [B]0 = 0. You wait until the mixture reaches equilibrium, and then you measure the concentration of B: [B]eq = 0.11 mol/L. From your experiment compute the equilibrium constant Kc of the reaction.
Answer the following questions relating to the solubilities of two silver compounds. Ag2CrO4 and Ag3PO4 Silver chronate dissociates in water according to the equation shown below Ag2CrO4 (s). = 2 Ag+ (aq) + CrO4 2- (aq) Ksp = 2.6 x 10^-12 at 25C A) write the equilibrium constant expression for the dissolving of Ag
Answer the following questions that relate to solubility of salts of lead and barium: A) A saturated solution is prepared by adding excess PbI2(s) to distilled water to form 1.0 L of solution at 25C. The concentrations of Pb2+ (aq) in the saturated solution is found to be 1.3 x 10^-3 M. The chemical equation for the dissoluti
1. Describe the equilibrium constant in terms of the law of mass action and write equilibrium constant expression for multiple equilibria. 2. Relate the constants and equilibrium constants and describe how equilibrium varies with temperature. 3. Use equilibrium constants to predict the direction of a reaction towards equil
Consider the equilibrium A <----> B. The equilibrium constant is Kc = 0.909, and the initial concentrations are [A]0 = 0.17 mol/L and [B]0 = 0 mol/L. Compute [A] after equilibrium has been reached. (in mol/L) (Using correct significant figures.)
In the reaction CO(g) + Cl2(g)<---> COCl2(g), Kc = 1200 at 395 K. What is the equilibrium value of [COCl2] if at equilibrium, [CO] = 2[Cl2] = 1/2[COCl2]? (in M) (Use correct significant figures.)
If the equilibrium concentrations found in the reaction 2 A(g) + B(g) <----> C(g) are [A] = 0.024 M, [B] = 0.0046 M, and [C] = 0.0062 M, calculate the value of Kc.
In the following reaction N2O4(g) <-----> 2 NO2(g), equilibrium is reached at a temperature at which partial pressure of NO2 P_NO2 = 3(P(of)N2O4)^1/2. What must be the value of equilibrium constant Kp at this temperature?
In the reaction 2H2(g) + S2(g) <-----> 2H2S(g), K(subscript)c = 6.28 x 10^3 at 900 K. What is the equilibrium value of [H2] if at equilibrium [H2S] = [S2]^(1/2)? (in M)
If the equilibrium concentrations found in the reaction A(g) + 2B(g) <----> 2C(g) are [A] = 0.025 M, [B] = 0.15 M, and [C] = 0.55 M, calculate the value of K (subscript)c.
The density of acetone vapor in equilibrium with liquid acetone, (CH3)2CO, at 32 degrees Celsius is 0.876 g/L. What is the vapor pressure of acetone, in mmHg, at 32 degrees Celsius? (Use correct significant figures.)
Im confused on how to set this problem up while incorporating the water, octanol, and air in one equation so I can solve for the mass. Help is much appreciated! thank you A stoppered flask at 25 C contains 250 mL water, 200 mL octanol, and 50 mL of air. An unknown mass of o-xylene is added to the flask and allowed to partit
A stoppered flask at 25 C contains 250 mL water, 200 mL octanol, and 50 mL of air. An unknown mass of o-xylene is added to the flask and allowed to partition among the phases. After equilibrium has been established, 5.0 mg of o-xylene are measured in the water. What is the total mass (g) of o-xylene present in the flask?
Could you please explain what formula and step are invovled and please provide (example) if possible A stoppered flask at 25 C contains 250 mL water, 200 mL octanol, and 50 mL of air. An unknown mass of o-xylene is added to the flask and allowed to partition among the phases. After equilibrium has been established, 5.0 mg of
I am trying to figure out a few questions/problems. -You want a column to have 6 theoretical plates. Your packing material has a HETP value of 1.5. What is the length of the column that you would need? I thought I would multiply the 6 TP by the HETP value. (This was a past quiz question) How do I solve this type of question?
Please see attached file. Consider the following reaction: CO2(g) + C(s) ----> 2CO(g) At equilibrium, at a certain temperature, the partial pressures of CO2(g) and CO(g) are 33.7 and 9.26 atm, respectively. Calculate the value of Kp.
1.) Calculate Ke for the following (equilibrium concentrations given below substances). See attached file for full problem description. 2.) For all three of the equilibria in problem #1 predict (1) how Ke is affected by an increase in temperature, (2) predict how the equilibrium will sh
Can you show me how to set up this problem? 2.44 gm of CuSO4 are dissolved in 9.0 x 10^2 ml of 0.30 Molar NH3. What are the concentrations of Cu+2, NH3, and Cu(NH3)4 at equilibrium?
The Haber process for ammonia synthesis is exothermic: N2(g) + 3H2(g) <--(double arrow for equilibrium) --> 2NH3(g) Change in H (degrees) = -92KJ If the equilibrium is constant Kc for this process at 500 Degrees Celsius is 6.0 X 10^-2, what is its value at 300 Degrees Celsius. I am not sure which equation I shou
Problem: Consider the following gas-phase equilibrium reaction: N2(g) + 02(g) <-- (double arrow for equilibrium) --> 2NO(g) Kc = 4.10 X 10 ^-4 at 2000 Degrees Celsius. If 1.0 mol of NO is introduced into a 1.0 L container at 2000 Degrees Celsius, what is the concentration of NO when equilibrium is reached.
1. Write the equilibrium constant expression (K) for the following reaction CS2 (g) + 4H2 (g) --> CH4 (g) + 2H2S (g) 2. Write the equilibrium constant expression (K) for the following reaction CuO (s) + H2 (g) --> Cu (s) + H2O (g) 3. Ammonium chloride is sometimes used as a flux in soldering because it decomposes upon he
Calculate the equilibrium constant of the following reaction at 25°C from standard potential data (available in emf (electromotive force tables) in any General Chemistry book; the library has many.) Sn(s) + 2 AgCl(s)-->2 Ag(s)+ SnCl2(aq)