Jan 31, 2018 · Generally speaking, this can be shown to be a consequence of the Arrhenius equation, which attempts to make predictions about the change observed in rate constants based upon observed changes in temperature.
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The reaction of nitrogen with oxygen to form nitric oxide can be represented by the following equation. N 2 ( g ) + O 2 ( g ) ↔ 2NO( g ) R = 0.08206 L·atm/mol·K At 2000°C, the equilibrium constant, K c , has a value of 4.10 × 10 -4 .

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  • What is K p? 2NO(g) + O 2 (g) ⇌ 2NO 2 (g) 4 (10 points) Consider the following reaction at a particular temperature: 2HI(g) ⇌ H 2 (g) + I 2 (g) A 2.00 L flask is filled with 0.320 mol of HI and allowed to reach equilibrium. At equilibrium, [HI] = 0.098 M. Calculate K c. Since [HI] = 2. 5 (10 points) At a particular temperature, the reaction ...
  • You can study other questions, MCQs, videos and tests for Chemistry on EduRev and even discuss your questions like For the following three reactions (I), (II) and (III) equilibrium constants are given (I) CO(g) + H2O(g)→CO2(g) + H2(g); K1 (II) CH4(g) + H2O(g)→CO(g) + 3H2(g); K2 (III) CH4(g) + 2H2O(g)→CO2(g) + 4H2(g); K3Which of the ...

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Exercise 3 Calculating the Values of K. The following equilibrium concentrations were observed for the Haber process at 127°C: [NH3] = 3.1 X 10-2 mol/L [N2] = 8.5 X 10-1 mol/L [H 2] = 3.1 X 10-3 mol/L. a. Calculate the value of K at 127°C for this reaction. b. Calculate the value of the equilibrium constant at 127°C for the reaction:

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Changing the pressure can't make any difference to the K p expression. The position of equilibrium doesn't need to move to keep K p constant. Changing temperature. The facts. Equilibrium constants are changed if you change the temperature of the system. K c or K p are constant at constant temperature, but they vary as the temperature changes.

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result of the reaction, the equilibrium amounts of Fe3+ and HSCN will be less than they would have been if no reaction had occurred; for every mole of FeSCN2+ that is formed, one mole of Fe3+ and one mole of HSCN will react. According to the general law, K eq for reaction 3 takes the following form. [Fe ][HSCN] [FeSCN ][H ] K 3 2 eq + + + = (4) 1

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Mar 04, 2018 · K_c = 2.25 * 10^(3) You know that when the following reaction takes place at 753^@"C" "H"_ (2(g)) + "I"_ (2(g)) rightleftharpoons color(red)(2)"HI"_ ((g)) the initial concentrations of the two reactants are ["H"_ 2]_ 0 = "3.10 M" " " and " "["I"_ 2]_ 0 = "2.55 M" and the equilibrium concentration of iodine gas is ["I"_2] = "0.0200 M" This tells you that the concentration of iodine gas ...

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Determine the empirical formula of an oxide of iron which has 69.9% iron and 30.1% dioxygen by mass. Q:-In a reaction A + B2 → AB2 Identify the limiting reagent, if any, in the following reaction mixtures. (i) 300 atoms of A + 200 molecules of B (ii) 2 mol A + 3 mol B (iii) 100 atoms of A + 100 molecules of B (iv) 5 mol A + 2.5 mol B

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These reactions have the equilibrium constants: H SO2 = [SO 2. H 2 O ]/p SO2. K s1 = [H +][HSO 3-]/[SO 2. H 2 O] K s2 = [H +][SO 3 2- ]/[HSO 3-] K w = [H +][OH-] ; This is called the ion product of water: K w = 10-14 M 2 @ 298 K. The concentrations of the dissolved species are: [SO 2. H 2 O] = H SO2 p SO2 [HSO 3-] = K s1 [SO 2. H 2 O]/[H +] = H SO2 K s1 p SO2 /[H +]

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Jan 31, 2012 · ∆G° = – RT ln K. Since K is the equilibrium constant, we are at equilibrium, the amounts of products and reactants in the mixture are fixed, and the sign of ∆G° can be thought of as a guide to the ratio of the amount of products to the amount of reactants at equilibrium and therefore the thermodynamic favorability of the reaction.

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Consider the following reaction in the Contact process for the production of sulfuric acid for parts (a) to (d) in this question. 2SO + O 2SO (a) Write the equilibrium constant expression for the reaction. (1) 2 2 3 (b)(i) State the catalyst used in this reaction of the Contact process.

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