pls help me thank u Consider the following reaction:N₂(g) + O₂(g) — 2NO(g)If the equilibrium partial pressures of N₂, O₂, andNO are 0.15 atm, 0.33 atm, and 0.050 atm, respec-tively, at 2200°C,Calculate Kp.E.A reaction vessel contains NH3, N₂, and H₂ at equi-librium at a certain temperature. The equilibriumconcentrations are [NH3] = 0.25 M. [N₂] = 0.11 M.and [H₂] = 1.91 M. Calculate the equilibrium con-stant K for the synthesis of ammonia if the reactionis represented as(a) N₂(g) + 3H₂(g) —(b) N₂(g) + H₂(g) →2NH3(g)NH3(g)

Given, N2(g) + O2(g) ⇌ 2NO(g) Equilibrium partial pressure of all the species are, PN2 = 0.15 atm…

Answered: Consider the following reaction: N₂(g)…

Consider the following reaction: N₂(g) + O₂(g) 2NO(g) If the equilibrium partial pressures of N₂. O₂, and NO are 0.15 atm, 0.33 atm, and 0.050 atm, respec- tively, at 2200°C, Calculate Kp.

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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CH6_Chem103 - Kenai Peninsu X + to.mheducation.com/ext/map/index.html?_con=con&external_browser=0&launchUrl=https%253A%252F%252Fclasses.alaska.edu%252Fwebapps... 054 520 2 X 9 part 2 Homework i 47:54 J bok 50 O int rint erences C 125 aw 11 :0 FI 2 Question 11 - Chapter 9 part 2 X Determine the volume (in mL) of a 13.3 MHC2H3O2 stock solution must be used to prepare 200.0 mL of a solution that is 0.719 M HC2H302. F2 W mL HC2H302 # 3 00 20 F3 E $ 4 000 000 F4 R % 5 F5 U 8 DII F8 1 ( 9 DD F9 0 3 F10 Help P Sav
Can you show how to out this calculation in the calculator? Everytime I do it, I get a different answer.
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2. Run V (NH4)2S₂08 (mL) 20.00 20.00 10.00 5.00 20.00 15.00 1 2 3 4 5 6 [S₂082-] (mol/L) 0.04 0.04. 0.02 0.01 10.09 10.03. VKI (mL) 20.00 10.00 20.00 20.00 8.00 15.00 [1-] (mol/L) 0.08 0.07 0.08 0.08 0.032 V Na₂S₂03 (mL) 10.00 10.00 10.00 10.00 10.00 10.00 [S₂032-] (mol/L) 6.001 0.001 0.001 10.001 0.001 0.001 These calculated concentrations should be entered in the Data Table for this experiment for runs 1-6. To calculate the concentration of [12], use Equation (3) and the concentration of [S₂03²]. In a constant-temperature run described in the procedure section of this experiment, the solution turned blue in 50 s. a) Consider the concentration of [S₂032] in the mixed solution shown in the las column of the table from the previous exercise. Calculate the concentration c [12] final formed in this reaction. b) Calculate the rate of the reaction.
Data Analysis: 1. Create an Absorbance (Y) vs. Concentration (X) graph using data from the six standard solutions above. 2. Perform a linear trendline analysis of your six data points. Display the equation and R² value on the graph with a minimum of 8 decimal places. 3. On the same graph, perform a 2nd order polynomial trendline analysis of your six data points. Display the equation and R² value on the graph with a minimum of 8 decimal places. 4. Turn in your graph as the last page of this report. 5. On a separate piece of paper calculate the concentration of the unknown solution using both the linear and 2nd order polynomial trendline equations (Show all work) 6. Choose the best unknown concentration from #4 above and report it with three significant figures in the unknown data table above.
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