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Chemical Equilibrium

Solubility and common ion effect

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

Chemistry Derivative

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

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

Reaction quotient

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.

Find: The Equilibrium Constant

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?

Solve: Equilibrium constant

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?

Solving for the Equilibrium Constant

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?

Solve: Calculating the Equilibrium Constant

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?

Solubility Ksp calculations

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

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

Acid base equilibrium

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

Equilibrium Constant Value


Finding the equilibrium constant

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

Given concentration, change a product concentration, what is concentrations

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

Acid Base Equilibrium Questions

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.

Calculation of Amounts of Constituents in Acid-Base Equlibrium

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

Systematic Treatment of Equilibrium

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

Equilibrium/pressure problem

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.

Equilibrium charge reactions between hydrogen and deuterium

The equilibrium charge-exchange reaction between hydrogen and deuterium is given by: H2 + 2D+ (arrows) D2 + 2H+ Using the standard reduction potentials for each half reaction given below, determine which isoptope of hydrogen (H or D) prefers to be in the +1 state in aquesous solution under standard conditions. 2D+ + 2e- (righ

IR and HNMR spectra

Can you please help me determine the identity of this molecule. I know from the IR that it contains a carboxyl group, but I am not quite sure what the HNMR is showing. Can you please help me?

Temperature at Equilibrium

Find the Celcius temperature at which the reaction N2O4(g) <-> 2NO2(g) will be in equilibrium when both gasses are present at partial pressures of 1.00 atm. DeltaH degree(25 degree C) DeltaGdegree(25 degree C) NO2(g) 33.85 KJ/mol 51.8 KJ/mol N2O4 9.66 KJ/mol 98.29 KJ/mol

2-Pentanone and Semicarbazide

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.

Determine the Equilibrium Constant

Determine the equilibrium constant for the following reaction at 25 degrees celsius. N_2O_4 (gas) => 2NO_2 (gas), for which change of G at 25 celsius = +5.4kJ At 25 deg celsius the gas in reaction vessel has a dark brown color.

Determine Equilibrium Partial Pressure

An evacuated 4.0 L vessel containing solid sulfur is initially charged with 1.30 atm hydrogen gas at 44.9 celsius. Eventually, the following equilibrium is achieved: H_2(gas)+ S(solid) = H_2S (gas) Determine the equilibrium partial pressure of molecular hydrogen in the vessel given that K=0.68 for the reaction as written.

Calculating Equilibrium Constants

Equilibrium constants are known for the following reactions S(s) + (3/2) O2(g) =SO3(g) Ksubletterc =9.2 x 10^23 SO3(g) = SO2(g) + (1/2)O2(g) Kc= 4.8 x 10^-4 Thus for the reaction S(s)+O2(g) = SO2(g) Kc = ____________ Please show work = is actually two arrows pointing opposite each other

Equilibrium constant of a reaction in a sealed tube

Ethanol and Ethanoic acid react to form Ethyl ethanoate and water according to the equation C2H5OH + CH3COOH = CH3COOC2H5+H2O When two moles each of ethanol and ethanoic acid are allowed to react at 100 degrees celcius in a sealed tube, equilibrium is established when two-thirds of a mole of each of the reactants remains. Calc

Equilibrium constant of a reaction

5.00 mol of ammonia are introduced into a 5.00 Liter reactor vessel in which it partially dissociates at high temperatures. 2 NHsubnumber3(g) = 3Hsubnumber2(g) +Nsubnumber2(g) At equilibrium at a particular temperature, 1.00 mole of ammonia remains. Calculate Ksubletterc for the reaction. Please show work. Also, briefly descr


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


At 700 K, the reaction 2SO2(g) + O2(g) = 2SO3(g) has the equilibrium constant Kc = 4.3 x 10^6, and the following concentration are present:[SO2] = 0.010 M: [SO3] = 10.M : [O2] =0.010 M When the reaction system reaches equilibrium, what is the SO3 concentration? Please show work.

Equilibrium concentration

Consider the reaction Nsubnumber2(g) + Osubnumber2 = 2NO(g), for which Ksubletterc =0.10 at 2,000 degrees celcius. Starting with initial concentrations of 0.040 M of Nsubletter2 and 0.040 M of 0subnumber2, determine the equilibrium concentration of NO = means two arrows pointing opposite directions