Calculate K. for the following reaction: 2NOB1(g) = 2NO(g) + Br2 (g) Express your answer to two significant figures.

As an EPA scientist studying catalytic converters and urban smog, you want to find K for the following reaction: 2NO₂(g) N₂(g) + 20₂ (g) Use the following data to find the unknown K: (1) NO(g) = N₂ (g) + O₂ (g) (2) 2NO₂ (g) 2NO(g) + 0₂ (g) Round your answer to 2 significant figures. 0. X 5 K=? K=2.1 x 10° K=1.1×105

Calculate Kc for the following equilibrium. Be sure to use the correct significant figures. 2 SO2 (g) + O2 (g) ⇌ 2 SO3 (g) Kp = 2.5 x 10^10 at 425. K

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Suppose a 250. mL flask is filled with 1.6 mol of CH, 1.8 mol of H,O and 0.70 mol of CO. This reaction becomes possible: () +H,0(g) C0(g) +3H,(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity CO. You can leave out the M symbol for molarity. CH, H,0 CO H, initial change equilibrium Explanation Check © 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use| Privacy I Accessibility 口ロ X

Suppose a 250. mL flask is filled with 0.20 mol of N2 and 2.0 mol of NO. The following reaction becomes possible: N2(g) + O2(g) = 2NO(g) The equilibrium constant K for this reaction is 0.693 at the temperature of the flask. Calculate the equilibrium molarity of N2. Round your answer to two decimal places. Шм

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Suppose a 250. mL flask is filled with 0.50 mol of H, and 0.90 mol of HI. This reaction becomes possible: H, (g) +1,(g) = 2HI (g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of H,. You can leave out the M symbol for molarity. H2 HI initial ? change equilibrium

Consider the following reactions and their respective equilibrium constants: NO(g) + ½Br₂(g) = NOBr(g); K = 5.3 2NO(g) = N₂(g) + O₂(g); K = 2.1 × 10³⁰ Use these reactions and their equilibrium constants to predict the equilibrium constant for the following reaction: N₂(g) + O2(g) + Br₂(g) = 2NOBr(g) Express your answer using two significant figures.