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
At a certain temperature, K = 9.1e-4 (exponential notation) for the following reaction: FeSCN2+(aq) Fe3+(aq) + SCN -(aq) Calculate the concentrations of Fe3+, SCN -, and FeSCN2+ in a solution that is initially 2.0 M FeSCN2+.
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?
If in an 0.050 M aqueous solution of hydroxylamine, HONH2 at 20 degrees Celsius, [OH-] = 2.3 x 10 ^-5M, What is Kb for HONH2 at 20 degrees Celsius, and what are the equilibrium concentrations of HONH2, HONH3, and OH- in a 0.0010 M HONH2 solution. HONH2 + H2O = HONH3 + OH
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.)
NaOH is added to K2CrO4 and K2Cr2O7 separately in test tubes and a color change is noted. HCl is added to the same two separte solutions in fresh test tubes and a colour change is noted. Hcl is added to the first two mixtures NaOH is added two the second until a colour change is noted. A) What would the equations for the
Calculate solubility of AbBr in 6.0 M NH3. Assume the highest complex formed is Ag(NH3)2 +.
Calculate molar solubility of Fe(OH)2 in 0.10 Molar NaOH.
I have the following problem: the pKa values for H2SeO3 at 25 degrees C are 2.64 and 8.27. Write the base hydrolysis equilibrium equations for SeO3^2-(aq) and HSeO3 ^- (aq) ions, and calculate the equlibrium constant values for each equilibrium. I think that I am completely stuck on how to approach this equation. Please hel
A sodium hydroxide solution was standardized by weighing 2.425 g of oxalic acid, H2C2O4*2H2o and diluting it to 250 mL in a volumetric flask. Then 25.0 mL of this acid solution was titrated with 30.20 mL of base. Based on this information, how do I calculate the molarity of the sodium hydroxide solution?
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?
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?