Consider the reaction:S(s) + O2(g);SO2(g)Write the equilibrium constant for this reaction in terms of the equilibrium constants, Ką and K,, forreactions a and b below:а.) 2 S(8) + 3 О2(g)2 SO3(g) Kab.) SO2(g) + 1/2 02(g)SO3(g)K,K =

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Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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Chapter1: Chemical Foundations

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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A student ran the following reaction in the laboratory at 282 K: 2NO(g) + Br2(g) = 2NOBr(g) When she introduced 0.170 moles of NO(g) and 0.137 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.135 M. Calculate the equilibrium constant, K., she obtained for this reaction. K.
Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas. N₂O4(9) = 2 NO₂(g) Three experiments were run starting with different initial amounts of N₂O4(g) ([N₂O4lo in the table). The systems were allowed to reach equilibrium and the concentrations for each gas were measured (in units of moles/Liter). For each of the boxes below, calculate the ratios indicated by the column heading. This will show the mathematical relationship that exists between the concentrations of NO₂ and N₂O4 at equilibrium. Be sure to round to the correct number of significant figures. [NO₂] / [N₂04] Exp[N204]0[NO₂] [N₂04] 1 2 3 3.8 3.1 2.1 2.98 2.3 2.64 1.8 2.06 1.1 2 [NO₂] / [NO₂]²/ [N₂04] [N₂04] Based on your calculations, indicate whether each statement is True (T) or False (F): 1. Each experiment started with a different initial concentration of N₂O4. 2. The ratio ([NO₂] / [N₂O4]) is equal to a constant value. 3. The ratio (2 [NO₂] /…
Two reactions and their equilibrium constants are given. (Arrows are going back and forward) A+2B↽−−⇀2C. K1= 2.33 2C↽−−⇀D. K2= 0.114 Calculate the value of the equilibrium constant for the reaction D↽−−⇀A+2B. K=?
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6. Write the equilibrium constant expressions for the following reactions. a. 2Zns (s) + 302 (g) = 2Zn0(s) + 2S02 (g) b. C (s) + CO2 (g) = 2c0 (g) c. CH;CO,H (aq) = CH;COF (aq) + H* (aq)
A student ran the following reaction in the laboratory at 1083 K: 2503(g) 2sO2(g) + 02(g) When she introduced 7.36x10-2 moles of SO3(g) into a 1.00 liter container, she found the equilibrium concentration of SO3(g) to be 4.23x10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc II
At 25 °C, K. = 1.6 x 10-34 for the reaction %3D 2HCI(g) + I2(s) 2HI(g) + Cl2(g) Suppose 0.100 mol of HCI and solid I, are placed in a 1.00 L container. What will be the equilibrium concentrations of HI and Cl, in the container?
A student ran the following reaction in the laboratory at 700 K: N2 (g) + 3H₂(g) — 2NH3 (9) When she introduced 0.0350 moles of N₂(g) and 0.0529 moles of H₂(g) into a 1.00 liter container, she found the equilibrium concentration of H₂(g) to be 0.0512 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Ke = |
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At room temperature when HI (aq) is added to potassium bisulfite, KHSO3(s), sulfur dioxide is formed and the reaction vessel becomes cold. HI (aq) + KHSO3(s)→ SO2(g) + H2O(l) + K+(aq) + I-(aq). A.)Once the process has reached equilibrium at room temperature, which of the following must be true? choose one....(ΔH<TΔS, ΔH=TΔS, ΔH>TΔS, or need more info). B.) Once the process has reached equilibrium at room temperature, which of the following must be true? choose one....(ΔSuniv<0, ΔSuniv=0, ΔSuniv>0, or need more info).

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Consider the reaction: S(s) + O2(g); SO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, Ką and K,, for reactions a and b below: а.) 2 S(8) + 3 О2(g) 2 SO3(g) Ka b.) SO2(g) + 1/2 02(g) SO3(g) K, K =