Calculate the value of the equilibrium constant for each of the following reactions ( we abbreviate citric acid as H3Cit) using the Ka values for citric acid and for carbonic acid: H3Cit + HCO3- <--> H2Cit- + H2O +CO2 H3Cit + 3HCO3- <--> Cit3- + 3H2O +3CO2 Given Ka1 of H3Cit =8.4x10-4; Ka2 of H3Cit = 1.8x10-5; Ka3 of H3Ci
I am enclosing a problem is causing me some doubt. As you will read from the problem wording, It seems that the value should be 0.3 mole as well. However, it is not within the options. (See attached file for full problem description) --- When 2.0 mol of carbon disulfide and 4.0 mol of chlorine are placed in a 1.0 Liter fl
What is the Ecell and the equilibrium constant, Kc, for the cell represented by the combination of the following half-reactions? 2 Hg2+(aq) + 2e- equilibrium Hg2 2+(aq) E= 0.92V Cr3+(aq) + 3e- equilibrium Cr(s) E= -0.74 V
Please help answer the following problems. Include references in the solution. The hemoglobin molecule carries O2 in the blood from the lungs to the cells, where the O2 is released for metabolic processes. The molecule can be represented as Hb in its unoxygenated form and as Hb.O2 in its oxygented form. One reason CO is to
3. A complex ion forms between Ag+ and CN- to give [Ag(CN)2]- with a formation constant of 1.3 x 10 to the 21. To a 0.5 M aqueous solution of silver nitrate you and sufficient HCN to make it 2 M. The Ka for HCN is 6.03 x 10 negative 10. What are the equilibrium concentrations of Ag+, [Ag(CN)2]-2, H+, and HCN?
When hydrogen gas reacts with Iodine as a gas, Hydrogen Iodine is produced in its gaseous form. The equilibrium concetrations for both reactants were found to be 0.86 M and the product was found to be 0.27. Calculate the value of the equilibrium constant. How would pressure effect the equilibrium of this reaction?
Determination of the Molar Mass and Ionization Constant of a Weak Monoprotic Acid Acetic Acid + Water yields Conjugate Base + Hydronium Ion Or HA + H20; H30+ + A- Calculation of the ionization constant for acetic acid from the measured pH of acetic acid samples: Acetic Acid titrated with Sodium Hydroxide and the followin
Step by Step Explanation Ethylene, C2H4, will react with hydrogen gas under appropriate conditions to form ethane, C2H6. A 10.0-liter vessel is charged with 1.5 atm of hydrogen and 1.0 atm of ethylene at 25°C. The reaction is allowed to proceed to completion. Determine the total pressure in the vessel at 25° at the completi
Question states: In the reaction of ammonium chloride (as a solid) dissociating to produce ammonia and hydrogen chloride (both as gases), the equilibrium concentration of each product was found to be 3.71x10^-3 (they each have the same concentration, ammonia is 3.71x10^-3 and hydrogen chloride is 3.71x10^-3). Calculate the v
1. You have a 0.087565 M solution of a weak acid, HA, pH=4.18177. How many grams of NaA (molar mass = 62.476 g/mol) would you have to add to this solution (assume that there is no change in volume) to have a solution with a pH of 7.40000. Would this new solution be a good buffer? Please explain. 2. You have a mixture of
A.) Consider the reaction: 4HCl (aq) + MnO2 (s) <--> Cl2 (g) + 2 H2O (l) + MnCl2 (aq) Delta (H)degree The equilibrium is displaced to the left if: a. Catalyst is added b. pressure is lowered c. temp is lowered d. H2O is added e. none of these b.) Consider the following gas phase reaction at 25 oC. N2 (g) + C2H2
1. 4CuO(s) + CH4(g) CO2(g) + 4Cu(s) + 2H2O(g) The value of Kc for this reaction is 1.10 at 25.0°C. What is the value of Kp for this reaction? (R = 0.0821 L-atm/K-mol) a. 4.63 b. 26.9 c. 658 d. 37.2 e. 1.52 x 10-3 2. At a certa
Please help with the following problem. Provide a step by step solution. Solubility and the Common-Ion Effect. In problem 1 it was stated that the molar solubility of PbBr2 in pure water is 1.3 x 10-2 M. Calculate the molar solubility of PbBr2 in A) 0.20 M KBr and in B) 0.20 M Pb(NO3)2 Problem 1 in reference is: The Sol
LnP = - (delta H vap/ T) (1/T)+C ln P2 = lnP1 + delta H vap / R (1/T - 1/T2) )Gvap=)Hvap - T) Svap G=0
Calculating Equilibrium Concentrations. Consider the reaction SO2(g) + NO2(g) = NO(g) + SO3(g) at 460 C. What are the equilibrium concentrations of all reactants and products if the initial concentrations are [SO2]o = [NO2]o = 3.00 x 10-3 M and [NO]o = [SO3]o = 4.00 x 10-2 M? The value of the equilibrium constant for the
The Reaction Quotient. The reaction CS2(g) + 4 H2(g) <--> CH4(g) + 2 H2S(g) has an equilibrium constant of 0.28 at 900 C. Fill in the data table below. Please see the attached for the full question.
The Equilibrium Constant. Question: Consider the reaction 2 NO2Cl(g) = 2 NO2(g) + Cl2(g). A 12.0-L container holds these gases at equilibrium. What is the value of Kc for this reaction if there are 1.036 g NO2Cl, 5.962 g NO2, and 4.578 g Cl2 at equilibrium?
The Equilibrium Constant. Question: Consider the reaction SO2Cl2(g) = SO2(g) + Cl2(g), where Kc = 0.078 at 100 Degrees Celsius. What is the molarity of the chlorine gas at equilibrium if the equilibrium mixture contains 2.70 mol SO2Cl2 and 1.30 mol SO2 in a 25.0-L container?
The Equilibrium Constant. Question: Consider the reaction 2 NO(g) + 2 H2(g) = N2(g) + 2 H2O(g). A 3.00-L container is filled with a mixture of 0.300 mol NO, 0.150 mol H2, and 0.300 mol H2O. When the equilibrium is established [NO] = 0.062 M. What is the value of Kc?
Question: 1 mol of nitrogen and 1 mol of hydrogen are placed in a flask and allowed to come to equilibrium with the product ammonia (NH3). At equilibrium there are .8 moles of nitrogen present. What is the Keq for the reaction?
How do you complete a solubility Ksp problem? What is the solubility of aluminum hydroxide in water at 25 degrees Celsius if the Ksp is 3 x 10^-34? What is the concentration of Hydroxide at equilibrium? What is the concentration of a sulfide ion in a 1L solution of cuprous sulfide to which .03mol of cuprous nitrate has be
Calculating the equilibrium constant. I have had trouble with this problem. The EXACT question asks: Calculate the equilibrium constant at 298K for the following equation. Sn(+2)(aq) + MnO4(-1)(aq) ===> Sn(+4)(aq) + Mn(+2) I understand Kc = (Products^(stoic. coefficients))/(Reactants^(stoic. coeffic
If the formation of products is strongly favoured in this acid base system: HX+(B-)<>HB+(X-) The competing bases are B- and X-, am I correct? B- is a stronger base, am I correct ? Does K for this system have a large or small value and why? How would the equilibrium be affected by the addition of the soluble salt N
GIVEN THE EQUILIBRIUM CONSTANT VALUE OF Kc FOR THE FOLLOWING RECTION AT 300 CELSIUS N2(g) + 1/2 O2(g) N2O(g) Kc=3.4 * 10 XY -18(SQUARE ROOT) AT 300 CELSIUS N2O4(g) 2NO2(g) kc=4.6*10(SQUARE RROT OF -3 AT 300 CELSIUS 1/2N2(g) + O2(g)
A mixture of 1 mol of H2O (g) and 1 mol CO (g) is placed in an evacuated 1 liter reaction vessel at 1200 K at equilibrium 0.478 mols of O2 was present. Find Kc CO(g) + H2O (g)<--------> CO2 (g) + H2(g) Is this correct? E = 1-x 1-x <----> 0.478 + x + x 0.478 + x (x) / 1.0-2x+x2 0.478x + x2 It looks li
Equilibrium process at 686 deg C: C02(g) + H2 <---> CO(g) + H20(g) [CO2] is 0.086 M [H2] is 0.045 M [CO] is 0.050 M [H20] is 0.040 M Calculate Kc for the reaction at 686 deg C. If you add CO2 to increase it concentration to 0.55 mol/L, what will the concentrations off all the gases be when equilibrium is re-establis
1) A 0.223 molar solution of the weak acid, HA, with a pKa of 3.954 is titrated with a 0.142 molar solution of NaOH. What is the pH of the solution at the equivalence point of this titration? 2) 0.1405 mol of potassium cyanide (KCN) is used to prepare 609.1 mL of an aqueous solution. Take the pKa of hydrogen cyanide as 9.38.
I am a winemaker and in the course of my work I simply do not understand how to do a calculation of this sort. We usually express acidity (in wine) in terms of titratable acidity in grams tartaric acid per liter. Here is the information that I have: If 500 mg/L of lactic acid is added to distilled water and NaOH is added unti
Solve the following problems using the systematic approach to equilibrium problems. 1. Determine the concentration of Ag+, CN-, and HCN in a saturated solution of AgCN where the pH is fixed at 5.90. 2. Determine the concentration of NH4+, NH3, CH3COOH (acetic acid), and CH3COO- (acetate ion) if 0.0050 moles of ammonium acetate
What is the equilibirum pressure of COCL2 when COCL2 dissociates at 395 degree celcius where Kp = .0444 and the total pressure at equilibrium is 3.00 atm. COCl2 (g) arrow both ways CO (g) + Cl2 (g) Please explain how you get this answer, thank-you.