Consider the following reaction: 2A + 5B ⇌ 3C + 3D The average rate of appearance of D is given by ∆[D]/∆t . Comparing the speed of appearance of D and the speed of disappearance of A, we would obtain ∆[D]/∆t = ____x(-∆[A]/∆t). A) -2/3 B) +2/3   C) -3/2 D) +1 E) +3/2

An experiment involves the rxn: 2HI(g) ⇄ H2(g) + I2(g).   A sample of pure HI was placed inside a rigid container at a certain temperature. The table provides the initial and equilibrium concentrations for some of the substances in the rxn. Based on the data, which of the following is the value of the equilibrium constant (Keq) for the reaction, and why? Keq= 2.5×10−1, because [I2]eq = 2×[HI]eq. Keq= 6.3×10−2, because [I2]eq = ½ [HI]eq. Keq= 1.6×10−2, because [I2]eq = [H2]eq. Keq= 3.1×10−2, because [I2]eq = 2×[H2]eq.

For the following reaction: A(aq) + B(aq) ⇌ 2 C(aq) Given the following information, what is the equilibrium concentration of C in mol L-1? Initial concentration of A = 1.108 mol L-1 Initial concentration of B = 1.108 mol L-1 Initial concentration of C = 0 mol L-1 K = 0.4 x 10-5

At 777 K the reaction shown below is run with initial concentrations of [N2]=0.120 M and [O2] = 0.120 M.The reaction is allowed to reach equilibrium and has K=1.50x10-3 Calculate the concentration of NO at equilibrium.N2(g)+O2(g)↔2NO(g)

The following reaction is carried out with [PCl5]i = 0.400 M at 25°C (i means initial) The reaction: PCl5(g)⇌PCl3(g)+Cl2(g)  K= 0.00105  Using the small x approximation and "test x", could you please find the percent to two decimal places when testing x?  Thank you so much.

Part A It is possible to predict the equilibrium constant of a reaction by combining two or more reactions for which the value of K is known. When combining equilibrium constants, it is important to note the following: Determine the value of the equilibrium constant, Kpal, for the reaction • When a reaction is reversed, its K value is inverted; that is, Kreverse = 1/Kforward- • When the coefficients of a reaction are multiplied by a factor, the K value is raised to the power of that factor. • When reactions are added, their K values are multiplied. CO2 (g) = C(s) + 02(g). Kgoal =? by making use of the following information: 1. 2CO2 (g) + 2H20(1) = CH3COOH(1) + 202(g). K1 = 5.40 x 10-16 2. 2H2(g) + O2(g) = 2H,O(1). K2 = 1.06 x 1010 3. CH3COOH(1) = 2C(s) + 2H2(g) + O2(g). K3 = 2.68 x 10 9 Express your answer numerically. • View Available Hint(s) V ΑΣφ Kgoal = Submit Part B Determine the equilibrium constant, Kroal, for the reaction 4PCI, (g) = P4(s) + 10Cl2 (g), Kgoal =? by making use of…

Please show all your work please, thank you! Sorry, this question has many parts. The reaction O3(g)+O(g)→2O2(g), occurs via the following mechanism:Step 1: Cl(g)+ O3(g)→ClO(g)+O2(g); Ea=85 kJ/molStep 2: ClO(g)+ O(g)⇌Cl(g)+O2(g); Ea=10 kJ/mol Using the proposed mechanism, derive a rate law. *Hint: use the activation energies to determine the slower step. Show all of your work.

12. Which balanced chemical equation corresponds to the following equilibri, constant expression? Kp Po PBr2 A) 2 NOB (g) = 2 NO (g) + Br2(g) B) NO (g) + ½ Br2 (g) = NOBr (g) C) 2 NO (g) + Br2 (g) = NOBr D) 2 NO (g) + Br2 (g) = 2 NOBR 13. You know that Kc = 2.0 at a certain temperature for the gaseous reaction A + 2B = C + 4D. What would be the value of Kc for the reaction 2C + 8D = 2A + 4B A) 2.0 B) 0.50 C) 0.25 D) 4.0

The equilibrium concentratio ns of the reacting species are [CO]=0.050 M, [H2]=0.045 M, and [H₂O] = 0.04 M, [CO2] = 0.086 M a. Calculate the Kc for the reaction at 686C b. If we add CO2 to increase its concentration to 0.50 mol/L, what will the concentration of all the gasses be when equilibrium is reestablished?

Determine how the following changes affect the given equilblirium reaction that is held in a closed container.       A(g) + 2 B(s) ⇌ 3 C(g) + 3 D(s)      ΔH°rxn = −0.25 kJ/mol Adding some A(g)    Adding some D(s)    Removing some C(g)    Increasing the temperature    Halving the volume of the container        The following mechanism is proposed for the reaction  2 A2 + B2  →  2 C  A2 + B2  →  R + C  slow  A2 + R  →  C   fast  What is the rate law for the overall reaction?            A. rate = k[A2]   B. rate = k[A2]2 [B2]   C. rate = k[A2]2   D. rate = k[R]2    E. rate = k[A2][B2]