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
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?
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.
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
When VO2+ reacts with Ti2+ in acid solution the products are V2+ and TiO2+. a) What is the potential of the cell Pt/VO2+, V2+//TiO2+, Ti2+/Pt if all species are a 1 M. b) Write the equilibrium constant expression and calculate the value of the equilibrium constant.
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
Which of the following will NOT change the ratio of the products to reactants in an equilibrium mixture for a chemical reaction involving gaseous species? a. increasing the pressure b. decreasing the volume c. addition of a solid reactant d. removal of a gaseus product e. none of the above
For the system CO(g)+H2O(g) <--> CO2(g)+H2(g) Kp is 1.6 at 900K. If 0.500 atm CO(g) and 0.500 atm H2O(g) are combined in a sealed flask, what is the equilibrium partial pressure of CO2(g)? a. 0.279 atm b. 0.308 atm c. 0.471 atm d. 0.608 atm e. 0.942 atm
Nitrosyl chloride decomposes according to this reaction: 2NOCl(g) (equilibrium sign) 2NO(g)+Cl2(g) 0.600 atm of nitrosyl chloride is sealed in a flask and allowed to reach equilibrium. If 27% of the NOCl decomposes, what is the equlibrium constant for the reaction? a. 0.00485 b. 0.781 c. 0.0300 d. 0.370 e.
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 equilibrium constant for a gas phase reaction is measured at two temperatures. At 100 degrees Celsius, the equilibrium constant is 36. At 200 degrees Celsius, the equilibrium constant is 147. Which of the following statements is correct for this equilibrium? a. the reaction is first order b. the reaction is endother
A voltaic cell is based uon the following overall reaction: 2H+(aq)+Sn(s)-->H2(g)+Sn2+(aq) where E=0.141V. Calculate the equilibrium constant at 25 degrees Celsius.
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.