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.
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
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.
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
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? See the attached file.
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 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.
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.
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.
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
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
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.
Consider the reaction Nsubnumber2(g) + Osubnumber2 = 2NO(g), for which Ksubletterc =0.10 at 2,000 degrees Celsius. 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.
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.
Phosgene, OCCLsubnumber2, a poisonous gas, decomposes according to the equation OCCLsubnumber2(g) = CO(g) +CLsubnumber2(g). Calculate K,subletterp, for this reaction if Ksublettterc = 0.083 at 900 degrees celcius please show work.
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
The equation constant for the reaction Ni(s) = 4CO(g) = Ni(CO)subnumber 4(g) is 5.0 x10^4 at 25 degrees celcius. What is the equilibrium constant for the reaction Ni(CO) subnumber4 (g)= NI(s) = 4CO(g)? the equal sign is actually two arrows pointing opposite directions.
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
For the following reaction at 600. K, the equilibrium constant, Kp, is 11.5 PCl5(g)<---> PCl3(g) + Cl2(g) Suppose that 3.010 g of PCl5 is placed in an evacuated 580. mL bulb, which is then heated to 600. K. a)What would be the pressure of PCl5 if it did not dissociate? b)What is the partial pressure of PCl5 at equilibri