Suppose that you work at Turkish Patent and Trademark Office and a patent application came across your desk claiming that a new catalyst which causes higher equilibrium concentrations for the following reaction, under the same temperature and pressure conditions was developed. N205 - 2 NO2 + 1/2 O2 (all reactant and products are gases) Would you approve or decline this application? Explain.

Suppose that you work at Turkish Patent and Trademark Office and a patent application came across your desk claiming that a new catalyst which causes higher equilibrium concentrations for the following reaction, under the same temperature and pressure conditions was developed. N205 - 2 NO2 + 1/2 O2 (all reactant and products are gases) Would you approve or decline this application? Explain.

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

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

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2. At 1250°C, methane reacts with water as follows: CO(g) + 3H2(g = CH49) + H2O(g) In one experiment the equilibrium concentrations of the gases were [CH4] = 1.57 x 10-3, [H2O] = 3.42 x 10-3, [CO] = 2.17 × 10-3, and [H2] = 1.13 x 10-3. Calculate Keq at this temperature.
The reaction is at equilibrium at some temperature, T, and the following equilibrium concentrations are measured: [SO2] = 0.90 M, [O2] = 0.35 M, and [SO3] = 1.1 M. Write the equilibrium expression for this reaction. Calculate Keq for the reaction at temperature, T.
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10 The equilibrium reaction of 2 moles of SOe) plus 1 mole of Oxe) produces 1 mole of SO3(g)- What is the equilibrium constant expression for this reaction. 2(g)
1. The diagrams below represent the following reversible chemical reaction: H2(g) + 12 (g) =2 HI (g) At 448 °C, the equilibrium constant, K, for this reaction is 51 Initial Conditions: Temperature = 448 °C Volume of the container = 2.0 L 0 = 1 mole H2 (g) = 1 mole I2 (g) 00 00 .. 00 00 •. What is the initial molar concentration of hydrogen. [H:]? What is the initial molar concentration of iodide, [I2]? M This system will reach equilibrium when rate of the forward reaction is equal to the rate of the reverse reaction. Write the equilibrium constant expression, Kc, for this reaction: Calculate the equilibrium concentrations for H;(g), I (g) and HI (g) H2(g}_ + l2 (g) 2 HI (g) [H2] [L2] [HI Initial Change Equilibrium +2x -X-
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Given the following reaction, the equilibrium constant, and the initial concentrations; answer the four bullet questions. 2 NO2 (g) - 2 NO (g) + O2 (g) Kc = 1.56 x 10-10 Initial Species Concentration (M) NO2 5.62 x 10-10 NO 3.99 x 10-16 O2 9.35 x 10-3 • Set up the equilibrium expression, and calculate the reaction quotient (Q). Note: ^ means "to the" Q = [ Select ] • How does Q compare to K? Q is [ Select]
Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO₂(g) + H₂O(1)→2 HNO3(aq) + NO(g) At a certain temperature, a chemist finds that a 3.4 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound NO₂ H₂O HNO3 NO amount 5.9 g 142.0 g 15.1 g 12.0 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. с K = D 0 C x10 X Ś
NA van wwwwwwww 1. For the reaction, 2 NO (g) + 2 H₂ (g) = following equilibrium concentrations: [NO]= 8.1 x 10-³ M [N2] = 0.053 M N₂ (g) + 2 H₂O (g), calculate Keq given the [H₂] = 4.1 x 10-5 M [H₂O]= 2.9 x 10-³ M 2. Given the reaction, UO2 (g) + 4 HF (g) = UF4 (g) + 2 H₂O (g), predict the effect each of the following will have on the equilibrium of the reaction (shift to the reactant side, the product side, or no shift). a. Uranium dioxide (UO2) is added. c. Water vapor is removed. b. Hydrogen fluoride (HF) reacts with the walls of the reaction vessel. - 3. At a certain temperature, Keq = 150 for the reaction being studied in today's lab. Use Equation (3) to calculate the concentrations of Fe³+ and SCN in a solution that has an equilibrium FeSCN2+ concentration of 4.5 x 105 M. Assume the equilibrium concentrations of Fe³+ and SCN are equal.
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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.