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?
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?
Given two isomers (anomers) of a sugar with a specific rotational character, knowing the specific rotatoin of the equilibrium mixture, what are the percentages of each in the mix?
Q1. à¿-D-Galactopyranose has [à¿]D = +150.7o, and à¿-D-galactopyranose has [à¿]D = +52.8o. When either of them is dissolved in water and allowed to reach equilibrium, the specific rotation of the solution will be +80.2o. What are the percentages of each anomer at equilibrium?
Q1. ?-D-Galactopyranose has [?]D = +150.7o, and ?-D-galactopyranose has [?]D = +52.8o. When either of them is dissolved in water and allowed to reach equilibrium, the specific rotation of the solution will be +80.2o. What are the percentages of each anomer at equilibrium? (Original formatted question attached.) I reall
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
Please see the attached file for the fully formatted problem(s). Hydrogen gas is produced by the reaction of steam with "water gas," an equimolar mixture of H2 and CO obtained by the reaction of steam with coal. A stream of "water gas" mixed with steam is passed over a catalyst to convert CO to CO2 by the reaction: H2O(g) +
The Apparatus shown below consists of 3 temperature-jacketed 1.000 L bulbs connected by stopcocks. Bulb A contains a mixture of H2O(g), CO2(g), and N2(g) at 25 degrees C and a total pressure of 564 mmHg. Bulb B is empty and is held at a temperature of -70 degrees C. Bulb C is also empty and is held at a temperature of -196 degre
2NOBr(g) + Br2(g) <----> 2BrNO(g) @ equilibrium. NOBr is 34% dissociated at 25degreesC and total pressure is 0.25 atm. Calculate Kp and Kc. I know how to get Kp and Kc with given # of moles @ equilibrium, but cannot figure out how to get it from the percent dissociation. I tried inputting various values that I thought wer
The Ksp for silver iodide is 8.3 x 10^-17. What is the concentration of Ag+ in equilibrium with AgI(s) if [1-]= 1.0 x 10(^-1)M? a. 9.1 x 10(^-9)M b. 1.0 x 10(^-1)M c. 1.2 x 10(^-15)M d. 8.3 x 10(^-16)M e. 8.3 x 10(^-17)M
For the reaction below, the partial pressures of gases at equilibrium are as follows: H2=7.1x10^-5 atm, Cl2=2.5x10^-6 atm, and HCl=3.0atm. What is the value of the equilibrium constant Kp? H2(g)+Cl2(g) = 2HCl(g)
For which of the following reactions does Kc equal Kp? a. C2H4(g)+H2(g) (equilibrium sign) C2H6(g) b. H2(g)+l2(s) (equilibrium sign) 2Hl(g) c. 2S(s)+3O2(g) (equilibrium sign) 2SO3(g) d. SO2(g)+NO2(g) (equilibrium sign) SO3(g)+NO(g) e. both answers b and d
The value of the equilibrium constant for a particular reaction is 2.34 x 10^3 at 298k. Calculate the change in G for this reaction.
Hydrogen iodide can decompose into hydrogen and iodide gases. Kp for the reaction is 0.016. If 0.350 atm of Hl(g) is sealed in a flask, what would be the total pressure of the system when equilibrium is established? a. 0.258atm b. 0.279atm c. 0.350atm d. 0.385atm e. 0.412atm
At 25 degrees Celsius, the decomposition of dinitrogen tetraoxide has an equilibrium constant(Kp) of 0.144. If the equilibrium pressure of nitrogen dioxide is 0.298 atm, what is the pressure of dinitrogen tetraoxide? a. 2.07atm b. 0.162atm c. 0.617atm d. 0.0128atm
At a given temperature, the equilibrium constant (Kp) for the decomposition of dinitrogen dioxide is 0.172. If 0.224atm N2O4 is sealed in a flask, what partial pressure of NO2 will exist at equilibrium?
A reversible reaction described by the chemical equation shown below (equation one) has an equilibrium constant of 10. (S represents substrate, P represents product.) If we have a mixture containing [S]=2x10E-5 M and [P]=3x10E-5M, and we know that KmS=3x10E-5 M, Vmax (forward reaction) =2 micromole /(L min), and Vmax (reverse