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Chemical Equilibrium

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

Mass

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

Concentration

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

Calculate Ksubleter p

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.

Equilibriou constatnt

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.

The "role" of chemical equilibrium in electrochemical cells.

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

Solubility Equilibria

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

Chemical equilibrium and molarity

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

Chemical equilibrium of PCl5(g)<---> PCl3(g) + Cl2(g)

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

Equlibrium Concentrations

For the equilibrium PH3BCl <=> PH3 + BCl3, Kp = .052 at 60 degrees Celcius. Further, a solid PH3BCl3 is added to a closed .500 L vessel at 60 degrees celcius; the vessel is then charged with .0216 mol of BCl3. How would I calculate Kc and what would be the equlibrium concentration of PH3?

Total Gas Pressure

For the reaction 2NaHCO3 = Na2CO3 + CO2 + H20 a 5.00 gram sample of NaHCO3 is placed in an evacuated flask and the temperature is increased to 50 degrees celcius. What is the Total Gas Pressure in the flask at equilibrium? Kp=3.90 X 10-4 = (PCO2)(PH2O.)

Calculating solubility

Calculate solubility of AbBr in 6.0 M NH3. Assume the highest complex formed is Ag(NH3)2 +.

Equilibrium

Kf=1.38 x 10 -28th power M/s. Kr = 9.3 x 10 10th power M/s. Both constants are at 25 degrees Celsius, how would I find the equilibrium constant at 25 degrees Celsius?

Concentration and equilibrium

At 1495 degrees Celcius Kc for H2 + Br2 > 2HBR = 3 x 10 to the 4th power. H2 = .10 M Br2 = .20M What eqation(s)would I use or steps would I take to find the concentration of HBr?

Solving Equilibrium

Question: 4HCl + O2 > 2Cl2 + 2H2O HCl is at 2.30 atm, O2 is at 1.00 atm and they both react at 750 K. Equilibrium pressure of Cl2 is .93 atm. How do you go about finding the Kp at 750 K?

Equilibrium Concentrations

The equilibrium constant of the reaction A <--> 2B + C shown in Figure 9.3 (attached file) is 25.6 mol^2/L^2 at an unspecified temperature. The equilibrium concentrations in this system are [A]= 0.110 M, [B]= 1.78 M and [C]= 0.890 M. The reaction system is slugged with an additional amount of reactant, equal to a concentration o

Equilibrium

At an unspecified temperature, the equilibrium reaction system I2(g) + Cl2(g) <--> 2ICl(g) has a partial pressure of ICl(g) that is 5520 times the partial pressure of I2(g). In turn, the partial pressure of I2(g) is 2.75 times the partial pressure of Cl2(g). What is Kp for the equilibrium at this unspecified temperature?

Equilibrium Disassociation Constants

The equilibrium dissociation constant, K(subscript p), of the reaction H2-->2H/H2<--2H is 3.6 x 10^-33 atm. 1.00 mol of H2 is injected into a 10.5-L oven at 600 K and allowed to reach equilibrium. Calculate the total number of free hydrogen atoms in the reaction system.

Number of Moles

Part A: If we start with 0.500 moles of H2 (subscript) and 0.500 moles of I2 (subscript) in a 5.25 L reaction vessel at 698 K, how many moles of each of the three gases will be present at equilibrium? Equation: H2(subscript) + I2(subscript) <--> 2HI KEQ= 54.3 at 698 K Part B: The same set up as part A, but this time