**Problem Statement:**A quantity of HI was sealed in a tube, heated to 425°C, and held at this temperature until equilibrium was reached. The concentration of HI in the tube at equilibrium was found to be 0.0706 mol/L. Calculate the equilibrium concentration of H₂ (and I₂). For the gas-phase reaction:\[ \text{H}_2 + \text{I}_2 \leftrightarrow 2\text{HI} \]The equilibrium constant \( K_c \) at 425°C is 54.6.**Options:**(a) \( 9.55 \times 10^{-3} \, \text{M} \)(b) \( 1.17 \times 10^{-3} \, \text{M} \)(c) \( 1.85 \times 10^{-4} \, \text{M} \)(d) \( 4.78 \times 10^{-3} \, \text{M} \)(e) \( 2.34 \times 10^{-3} \, \text{M} \)

Step 1) equilibrium constant is defined as the ratio of the equilibrium concentrations of products…

9. A quantity of HI was sealed in a tube, heated to 425°C and held at this temperature until equilibrium was reached. The concentration of HI in the tube at equilibrium was found to be 0.0706 mol/L. Calculate the equilibirum concentration of H2 (and I2). For the gas-phase reaction, H2 + 12 2HI Kc = 54.6 at 4250C %3D

9. A quantity of HI was sealed in a tube, heated to 425°C and held at this temperature until equilibrium was reached. The concentration of HI in the tube at equilibrium was found to be 0.0706 mol/L. Calculate the equilibirum concentration of H2 (and I2). For the gas-phase reaction, H2 + 12 2HI Kc = 54.6 at 4250C %3D

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

ul Constant for the reaction. 2. Consider the reaction: A+B=C+3D A solution was prepared by mixing 50.00 mL of 1.00 x 10 M A, 100 mL of 2.00 x 10 MB, 10.0 mL of 1.0 M C and 75 mL of 1.50 x 10³M D. At equilibrium, the concentration of D was measured to be 6.0 x 10 M. a) Calculate the equilibrium concentrations of each species b) Calculate the equilibrium constant. 3. Consider the reaction: 2NO2(g) + Cl₂)* 2NOCI The initial pressure of NO, was 1.577 atm and the initial pressure of Cl₂ was 0.427 atm. At equilibrium, the partial pressure of NOCI is 0.624 atm. Calculate K.
Please Solve question 102
At 25 °C, K = 0.145 for the following reaction in the solvent CCI4. 2BrCI + Br2 + Cl2 A solution was prepared with the following initial concentrations: [BrCI] = 0.0454 M, [Br2]= 0.0329 M, and [Cl2]= 0.0241 M. What will their equilibrium concentrations be? [Br2] = M [Cl2] = i M [BrCI] = i M
For the reaction 2 NH3 = 3H₂ + N₂ The equilibrium concentrations were found to be [NH3]=0.250 M [H2]=0.450 M [N2]=0.800 M. What is the equilibrium constant for this reaction?
4
Consider the equilibrium: Sno, ()+ 20o ) Sn ()+ 200, le 5.0g of tin ( oide and 085 Mcarbon monoide were initially charged in a dosed reactor at room temperature and allowed to reach equilibrium. At equilibrium 0.65 Mof CO was measured. Calculate Ke for the equilibrium. O 0095 042 O022 11
17. When BaCO3 is first mixed with K3PO4 their concentrations are measured at: [BaCO3] = 0.968M and [K3PO4] = 0.745M. The reaction is allowed to progress until equilibrium is reached. At equilibrium [K₂CO3] = 0.804M. Calculate Keq. 3BaCO3(aq) + 2K3PO4 (aq) Ba3(PO4)2 (aq) + 3K₂CO3(aq) 18. For the following reaction, name 4 ways in which you can maximize the amount of product produced. CO(g) + 2H2(g) CH3OH(g) + heat
The initial concentration of Cl1- is 0.100M and the initial concentration of Co(H2O)62+ is 0.500 M. At equilibrium the concentration of CoCl42- is 0.0035. What is the value of the equilibrium constant for the reaction being studied?
4. Explain the effect of each of the following errors on the value of Ksp. Would you expect the Kp values will be higher than expected, lower than expected, or the same as expected, if: (a) A small amount of solid Ca(IO3)2 was present in the solution collected. (b) The graduated cylinder was not rinsed after transferring each sample into the flask or the rinses were not added to the respective sample.
Given these initial concentrations: [SCN-] = 0.000644 M, [Fe3+] = 0.000505 M, and [Fe(SCN)2+] = 0.000 M, determine the value for K if the [Fe(SCN)2+] at equilibrium is 0.0000856 M.
The equilibrium constant (Kp) is 0.11 at a particular temperature for the reaction: N204(9) = 2NO2(9) Given the following sets of initial conditions, what is the net change that must occur for the reaction to reach equilibrium? Does the reaction shift left to reach equilibrium, does the reaction shift right to reach equilibrium or is the reaction at equilibrium at these initial concentrations so no net change will occur? A. PNO, = 0.105 atm, PN,0, = 0.146 atm В. PNO, = 0.093 atm, PN,0, = 0.054 atm С. PNO, = 0.180 atm, PN,0, = 0.134 atm %3D D. PNO, = 0.088 atm, PN,0, = 0.07 atm Е. PNO, = 0.055 atm, PN,0, = 0.06 atm %3D %D A. right B. left C. left D. equilibrium left right E. > >
4. The mineral hydroxyapatite, Caro(PO4)(OH)2, dissociates in water according to the following equilibrium: Ca10(PO4)6(OH)2 10 Ca²+ (aq) + 6 PO³(aq) + 2OH(aq) a.) Write the K expression for this reaction b.) Suppose that solid hydroxyapatite is added to pure water and the reaction is allowed to reach equilibrium. At equilibrium, it is found that [OH] = 2.00 x 10 M. What is K?