In the overall reaction given by: H2(g) + 2 ICl(g) --> I2 (g) + 2 HCl(g)A)the concentration of H2 decreases at the same rate as ICl.B) the concentration of HCl increases equally as fast as I2C) the concentration of HCl increases twice as fast as I2.D) the concentration of all species are changing by the same amount at all times.

q27) very urgnatly required pls help

General Chemistry II Laboratory Manual, 2019 Revision 125 Determination of a Solubility Product Constant Pre-Lab Name: Date: 1) Write the solubility product equilibrium and the solubility product constant expression for barium fluoride. 2) A solution is made by placing solid barium fluoride into pure water. The barium ion concentration in this solution was found to be 1.1 x 108 M, what would the numerical value of Kp be for calcium fluoride? 3) A solution is made by diluting 10.0 mL of 0.021 M potassium dichromate to 200 mL. What is the molarity of the diluted solution?

5. Consider the following equilibrium, where both the forward and reverse directions are elementary reactions. COCI (g) + Cl (g) === CO (g) +Cl2 (g) a) Write the Equilibrium Expression. b) At 298 K, the rate constants for the forward and the reverse directions are 9.3 x 10 M's¹ and 14 x 100 M's respectively. What is the value for the equilibrium constant? c) If you start with [COCI] = 1.0 M and [CI] = 0.10 M, what are the concentrations of CO and Cl₂ at equilibrium? d) Sketch a graph of the relative concentrations of reactants and products versus Time. (Be sure to label everything)

b Jock Part A The following diagrams show the chemical reaction entrol over a four-hour time period. If C is blue and D is yellow, state whether or not the reaction has reached equilibrium in this time period. 1h esc Submit Provide Feedback alt The reaction has reached equilibrium because the total number of reactants and products does not change; the total concentration of C and D has not changed between 1 and 4 h. The reaction has not reached equilibrium because the number of reactants and products is still changing; the concentrations of C and D are still changing between 3 and 4 h. The reaction has reached equilibrium because the volume of the system does not change; the volume of the system has not changed between 1 and 4 h. The reaction has not reached equilibrium because the rate of the reaction is still changing; the rate of the reaction is still changing between 1 and 4 h. option 2 h Request Answer Q A Z 5.769 3h 2 W S AUG 9 VI X H command 4h #3 20 & F3 E D C OOD 100 F4 R F %…

6.B Consider the chemical equation A(aq) + 3B(aq) 5 2C(aq) with an equilibrium constant equal to 4.00 at a certain temperature. Each chemical is initially present at a concentration of 0.25 molar. (a) Set up a simple* expression for the equilibrium constant. (*freshman level) (b) Determine whether the forward or reverse reaction is occurring. (c) Set up an 1CE table to begin a calculation of the equilibrium composition. (d) Without a better calculator or resources on the internet, you cannot solve for the equilibrium composition. Which value for "x" works: 0.0261, 0.0315, or - 0.0129. If they all fail, then one of us did something wrong.

Consider the following graphical representation of concentration versus time for the equilibrium system: COC1₂(g) = Cl₂(g) + CO(g) AH = + 108 kJ 0.14 0.12- -C1₂ 0.10- CO 0.08 0.06- COCI₂ 0.04 0.02- 0.00 0 2 8 10 16 Time (min) a) What change was imposed at time = 4 minutes? Be specific. b) What change was imposed at time = 10 minutes? Be specific. c) What change was imposed at time = 14 minutes? Be specific. d) Using the data for the 12 minute mark, calculate the value of Keq at the temperature concerned. Show your work. Concentration (mol L-¹) 12 18

Which statements are always correct for a reaction at equilibrium? The forward and reverse reactions both continue. The concentrations of reactants and products are equal. The rates of the forward and reverse reactions are equal. I. II. |||. OII and III only I and III only I, II, and III I and II only

The following reaction is allowed to come to equilibrium and then the volume is increased.  Predict the effect of the indicated volume change once equilibrium is restored.                         H2O(g)            +          CO2(g)               double arrow              H2CO3(g)     The reaction will shift right.     The reaction will shift left.     There will be no effect.     Effect can not be determined from information provided.

NH4HS(s) = NH3(g) + H₂S(g) K = [NH3][H₂S] K = 1.2 x 10-4 What is the concentration of the H2S when the system reaches equilibrium? [H₂S] = [?] x 10¹¹ M Exponent (yellow) Coefficient (green) Enter