The image below shows the free energy diagrams for four different reactions (A, B, C and D), each going from reactant R to products P. Which of the following statements is correct about these reactions. IM IM. R R AG AG P Reaction progress Reaction progress D. IM IM M₂ P R R P Reaction progress P R = Reactants, P = Products AG TAG Reaction progress

How do you solve HWK1?

You are given the following:   H2 (g) + Br2 (g) 2 HBr (g) Kp = 7.9 x 1011                            H2 (g) 2 H (g) Kp = 4.8 x 10-41                                         Br2 (g) 2 Br (g) Kp = 2.2 x 10-15 What is Kp for the reaction shown below?                                H (g) +  Br (g)   HBr (g) Kp = ?

Consider the following equilibrium reaction: 2 NO (g)   +   O2 (g)   ⇋⇋   2 NO2 (g) What is the Kc expression? Select one: a. Kc=[NO2][NO][O2]Kc=[NO2][NO][O2] b. Kc=[NO2]2[NO]2+[O2]Kc=[NO2]2[NO]2+[O2] c. Kc=[NO]2[O2][NO2]2Kc=[NO]2[O2][NO2]2 d. Kc=2∗[NO2]2∗[NO][O2]Kc=2∗[NO2]2∗[NO][O2] e. Kc=[NO2]2[NO]2[O2]

Good hand written explanation Asap thanks Consider the reaction: AC (g) + 2 B (g) ↔ AB2 (g) + C (g)   ΔH = -224.5 kJ The system is sitting at equilibrium. Describe what will happen when each of the following stresses are applied.   The reaction will shift to the right.The reaction will shift to the left.The reaction will not be affected by this. B is selectively removed from the reaction vessel. The reaction will shift to the right.The reaction will shift to the left.The reaction will not be affected by this. Additional C is added to the reaction vessel. The reaction will shift to the right.The reaction will shift to the left.The reaction will not be affected by this. The temperature of the reaction vessle was raised.

Given this reaction at equilibrium, C(s) + CO2(g) D 2CO(g) (∆H° = 119kJ), explain the changes that would occur when the following stresses are applied: a.CO is removed. b.Heat is removed. c.CO2 is added.

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.

17. The following equilibrium system was found to contain 0.040M formaldehyde (CH₂O) at equilibrium. CH₂O(g) → H2(g) + CO(g) ΔΗ > 0 a. If the original concentration of formaldehyde was 0.080M, what is the equilibrium constant for this reaction? b. Suppose you needed to produce formaldehyde using the reverse reaction. Provide 3 different ways to increase the production of formaldehyde, explaining how each method would help.