SO2(g) + NO2(g) = SO3(g) + NO(g) Initial: 0.574 0.574 0.574 0.574 Change: +x +x Equilibrium: 0.574–x 0.574-x 0.574+x 0.574+x Therefore, (SO3][NO] (SO,][NO,] (0.574+æ)(0.574+æ) (0.574 – a)(0.574 – æ) K = 3.68 = What is the value of x?

For any reversible reaction containing a double arrow such as: Reactants ⟷⟷ Products the statement "equilibrium shifts to the right" means: Group of answer choices; - The reaction can only go in the forward direction. - The reaction can only go in the reverse direction. - A stress will cause a portion of reactants to disappear and some additional products to appear. - A stress will cause a portion of products to disappear and some additional reactants to appear

Nitrosyl bromide decomposes to NO and Br2 in an endothermic process (A,H° = 16.3 kJ/mol-rxn). 2 NOBr(g) ⇒ 2 NO(g) + Br2 (g) Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. a. adding more NOBr(g) shift left shift right O no change b. adding more Br₂(g) shift left shift right O no change c. increasing the volume of the reaction flask shift left shift right O no change d. lowering the temperature shift left shift right O no change

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Consider the following equilibrium:  CO(g) + NO2(g) ↔   CO2(g) + NO(g)  At a specific temperature the equilibrium concentrations where determined to be: [CO] = 0.0033M [NO2] = 0.021M  [CO2] = 0.59M [NO] = 0.59M a-      Calculate the value of the equilibrium constant b-      Describe the position of the equilibrium

Which answer below correctly describes the calculation to find the equilibrium expression for K4? Co(g) + 3H2(g) CS2(g) + 2H2S(g) CH4(g) + H20(g) K1 CH4(g) + 2S2(g) K2 CO(g) + H20(g) CS2(g) + 2H2S(g) + 3CO2(g) = 4CO(g) + 2S2(g) + 2H20(g) CO2(g) + H2(g) K3 K4 Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. K1 x (K2)¬1 x (K3)³ a b K1 x K2 x K3 3(K) x K х Кз d K1 x K2 x (K3)³ Use the following series of reactions to determine the value of the equilibrium constant K.j: NOz + H30+ - C5H5NH+ + OH- 2H20(1) = H30+ + OH° C5H5N + HNO, = C5H5NH+ + NO, Reaction1: HNO2 + H20(1) Kcı =?? -6- Reaction2 : C5 H5N + H20(1) Kc2 = 1.70 × 10 Reaction3 : Ксз — 1.01 X 10 14 Reaction4 : Kc4 = 1.19 x %3D Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a 7.07 X 10-4 b 2.01 X 10-25 9.93 X 1024 d 4.17 X 10-24 6.86 X 1034 e

Consider the reaction: SO₂(g) + 1/2O₂(g) ⇒ SO3 (9) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K2, for the reactions below: 2S(s) + 30₂(g) ⇒ 2SO3 (9) K₁ S(s) + O₂(g) → SO₂(g) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter K if the first equilibrium constant should be squared. K= An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer.

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