A.) For the reaction: 2Cl2 (g) + 2H2O(g) <----> 4HCl(g) + O2 (g), Kp = 6.4 x 10-6 at 500 K. If a fixed volume is filled with initial concentrations of these gases at 227 oC such that [Cl2] = 0.5 M, [H2O] = 0.40 M, [HCl] = 0.5 M, and [O2] = 0.015 M, in which direction will the reaction proceed? b.) 4.00 mol chlotine and 2.00 m
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
Complex-Ion Equilibria. When sufficient ammonia is added to a 0.00500 M silver nitrate solution to initially give 0.100 M aqueous ammonia, what is the molarity of the silver ion (Ag+) after the complex ion Ag(NH3)2+ has been formed at equilibrium? Ag+(aq) + 2 NH3(aq) = Ag(NH3)2+(aq)
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
The Solubility Product Constant. PbBr2 is a slightly soluble salt. Write A) the chemical equilibrium equation that describes the salt partially dissolving in water and B) the solubility product expression. C) Calculate the Ksp value for lead(II) bromide if the molar solubility in pure water is 1.3 x 10-2 M.
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?
At pH 6.00 and pE 2.70, what is the concentration of Fe2+ (mol/L) in equilibrium with Fe(OH)3?
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
I am having a hard time finding the equilibrium constant for this problem, can anyone help? Determine Equilibrium constant at 298K for: Sn(+2)(aq) + MnO4(-1)(aq) ==> Sn(+4)(aq) + Mn(+2)(aq)
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
The solubility of a product of Ca(OH)2 is 7.9 (10^-6) at 25 C. Will a precipitate form when 100mL of 0.10 mol/L of CaCl2 solution and 50.0 mL of 0.070 mol/L of NaOH solution are combined. Please explain the procedure to this answer by showing all steps.
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)
In the manufacture of sodium carbonate, NaHCO3(s) is decomposed by heating. 2 NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(g) Kp=0.23 at 100 celsius. 1- If a sample of NaHCO3(S) is brought a temperature of 100
The equilibrium constant Kc for the decomposition of phosgene, COCl2, is 4.63 x 10^-3 at 527 deg C. COCl2(g)<--->CO(g)+Cl2(g) Calculate the equilibrium partial pressure of all the components, starting with pure phosgene at 0.760 atm Answer should give partial pressures of COCl2, CO, Cl2. I do not understand also what i
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.
A mixture containing 3.9 moles of NO and 0.88 mole of CO2 was allowed to react in a flask at a certain temp according to the equation: NO(g)+CO2(g) f/r NO2(g)=CO(g) At equilibrium, 0.11 mole of CO2 present. Calculate equilibrium constant, Kc.
The equillibrium constant Kc for the reaction shown is 2.18 x 10^6 at 730 deg. C. H2(g)+Br2(g) <--> HBr(g) Starting with 3.30 moles of HBr in a 12.0 L reaction vessel, calculate the concentration of H2, Br2, and HBr at equil.
At 1000 deg. K, a sample of pure NO2 gas decomposes. 2NO2(g)f/r2NO(g) + O2(g) The equilibrium constant Kp is 158. analysis shows that the partial pressure of O2 is 0.14 atm at equilibrium. Calculate the pressure of NO and NO2 in the mixture in atm.
H20(l) f/r H+(aq) + OH-(aq) k1 is forward and K_1 is reverse if k1 = 2.4 x 10^-5 s^-1 and K_1=1.3 x 10^11/M *s Calculate the equilibrium constant K Calculate k=[H+][OH-] and [H+] and [OH-]. There should be four answers.
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
2-Pentanone forms a derivative on treatment with semicarbazide. Note that semicarbazide has two -NH2 groups that might react with the carbonyl of the ketone to form semicarbazone. Explain why it reacts the way it does.
Question: To colour spots on TLC plates for easier visualization after elution with a solvent, the plates can be "developed" in a sealed chamber containing solid iodine. Explain how the solid-vapor equilibrium operates in this instance.
50.0 g of N2O4 is introduced into an evacuated 2.00 Litre vessel and allowed to come to equilibrium with its decomposition product, N2O4(g) = 2 NO2(g). For this reaction Kc=0.133. Once the system has reached equilibrium, 5.00 g of NO2 additional is injected in to the vessel, and the system is allowed to equilibrate once again. C
If one starts with pure NO2(g) at a pressure of 0.500 atm, the total pressure inside the reaction vessel when 2NO2(g) = 2NO(g) + O2(g) reaches equilibrium is 0.674 atm. Calculate the equilibrium partial pressure of NO2. = means two arrows pointing opposite directions.
1.25 moles of NOCL were placed in a 2.50L reaction chamber at 427 degrees Celsius. After equilibrium was reached, 1.10 moles of NOCL remained. Calculate the equilibrium constant, K subletter c, for the reaction 2NOCL(g) = 2NO(g) + CL subnumber2(g). The equal is actually two arrows pointing in opposite directions, please show
I do not understand why a reaction (oxidation and reduction) can continue producing electricity if equilibrium (at a given temperature) has already been reached. For example, the conversion of Fe2+(aq) ion to Fe3+(aq) ion is necessary for the anode half reaction to continue producing electrons while the continued conversion of
Please show all work and explain the formulas through to the answer. 1. The Solubility Product Constant. PbBr2 is a slightly soluble salt. Write the chemical equilibrium equation that describes the salt partially dissolving in water and the solubility product expression. Calculate the Ksp value for lead(II) bromide if the
Please show all work and identify all parts of equations. Please remember that this is a first year course and keep answers simple. 1. The Equilibrium Expression. Write the equilibrium expression for each of the following systems. a. 3 NO(g) ----> N2O(g) + NO2(g) b. Zn(s) + 2 H+(aq) ----> Zn2+(aq) + H2(g) c. Ti