For chemical reactions where all reactants and products are in the gas phase the amount of eachgas in the vessel can be expressed either as partial pressures or as concentrations. As such theequilibrium constant for a gas phase reaction can also be expressed in terms of concentrations orpressures. For the general reaction,Part AaA(g) + bB(g) - cC(g) + dD(g)For the reactionK,and K.2CH(g) = C,H2(9) + 3H2(9)(P.(AyK. = 0.140 mol L- at 1727 °C. What is K, for the reaction at this temperature?It is possible to interconvert between K, and K. usingEnter your answer numerically.K, = K-(RT)An> View Available Hint(s)where R = 0.08314 L bar molKand An is the difference in stoichiometric coefficientsbetween gaseous products and gaseous reactants.к, 3 3870 bar?If we assume that the gaseous reactant and products are "ideal" and the partial pressures of thereactants and products were expressed in bar, then the thermodynamic equilibrium constant, Kis the magnitude (or numerical value) of Kp.Prevlous Answerev Correct• Part BWhat is the unitless themodynamic equilibrium constantfor the reaction in part A?Express your answer numerically.• View Available Hint(s)Templates Symbols undo redo Teset keyboard shortcuts HelpK = 21.8SubmitPrevioun AnewereX Incorrect; Try Again; 5 attempts remaining For chemical reactions where all reactants and products are in the gas phase the amount of eachgas in the vessel can be expressed either as partial pressures or as concentrations. As such theequilibrium constant for a gas phase reaction can also be expressed in terms of concentrations orpressures. For the general reaction,Incorrect; Try Again; 5 attempts remainingaA (g) + bB(g) = cC(g) + dD(g)and Ke• Part CJA"BIt is possible to interconvert between K, and K. usingFor the reactionN2(9) + 3H2(9) = 2NH3(9)K, = K-(RT)AnK, = 3.85 x 10-3 bar 2 at 315 °C. What is K. for the reaction at this temperature?where R = 0.08314 L bar mol Kand An is the difference in stoichiometric coefficientsbetween gaseous products and gaseous reactants.Enter your answer numerically.> View Available Hint(s)If we assume that the gaseous reactant and products are "ideal" and the partial pressures of thereactants and products were expressed in bar, then the thermodynamic equilibrium constant, Kis the magnitude (or numerical value) of K.Tempiates Symdols undo regoo fes keyboard shortcuts HelpK. =L mol 2Submit• Part DWhat is the unitless themodynamic equilibrium constant K for the reaction in part C?Express your answer numerically.> View Available Hint(s)TemplatesSumfolundo redo Tese keyboard shortcuts HelpK=Submit

Given2 CH4(g) ⇌ C2H2(g) + 3H2(g)Kc = 0.140 mol2L-2No of moles of gaseous product = 1 mole of C2H2…

For the reaction 2CH,(9) -== C,H2(9) + 3H2(g) K = 0.140 mol L at 1727 °C. What is K, for the reaction at this temperature? Enter your answer numerically. > View Available Hint(s) K, = 3870 bar Prevlous Anewere Correct Part B What is the unitless themodynamic equilibrium constant K for the reaction in part A? Express your answer numerically. > View Available Hint(s) Templates Symbols undo regio teset keyboard shortouts Help K = 21.8

For the reaction 2CH,(9) -== C,H2(9) + 3H2(g) K = 0.140 mol L at 1727 °C. What is K, for the reaction at this temperature? Enter your answer numerically. > View Available Hint(s) K, = 3870 bar Prevlous Anewere Correct Part B What is the unitless themodynamic equilibrium constant K for the reaction in part A? Express your answer numerically. > View Available Hint(s) Templates Symbols undo regio teset keyboard shortouts Help K = 21.8

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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ju sited Free Online Survey... Search Home - Academia... Submit Answer Retry Entire Group Modules [References] Use the References to access important values if needed for this question. Consider the following reaction where Kp = 0.160 at 298 K. 2NOBr(g) 2NO(g) + Br₂(g) If the three gases are mixed in a rigid container at 298 K so that the partial pressure of each gas is initially one atm, what will happen? Indicate True (T) or False (F) for each of the following: 1. A reaction will occur in which NOBr(g) is produced. 2. K, will increase. 3. A reaction will occur in which NO is produced. 4. Qp is greater than Kp. 5. The reaction is at equilibrium. No further reaction will occur. hp 8 Create Your Rubric -... 8 more group attempts remaining || K The Utility Experts ... E P insert » C 4x 12/ bac
Consider the reaction A(g)+ 2B(g) =AB₂(g) with Kp = 0.00575 at a given temperature. At the same temperature, a reaction mixture contains all three gases each with partial pressure = 1.00 atm. Which expressions are best suited (conforms to what is happening at the molecular level) to solve for the change in concentration of species A? Select all that apply. 174= (1.00+x)(1.00+2x)² (1.00-x) 0.00575 = 0.00575 = 174= (1.00+x) (1.00-x)(1-2x)²) (1.00-x) (1.00+x)(1.00+2x)² (1.00-x) (1.00+x)(1+2x)²)
Part A The value of K, for nitrous acid (HNO,) at 25 °Cis 4.5 x 10 4 Part B Part C What is the value of AG at equilibrium? Express your answer using one significant figure. AG = 0 kJ Submit Previous Answers v Correct By definition, the Gibbs free energy of a reaction is zero when it is at equilibrium. Forward and reverse reactions continue to occur dynamically, but there is Part D What is the value of AG when [H'] = 5.1 x 10 2 M. [NO,] = 6.2 x 10 4M and (HNO2] = 0.21 M? Express your answer using three significant figure. ? AG = kJ Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
Please write full calculations and explain math At 700 K, the reaction2SO2(g) + O2(g) ⇌ 2SO3(g) has the equilibrium constant K = 4.3 × 106, and the following initial partial pressures present: pSO2 = 0.010 bar; pO2 = 0.010 bar; pSO3 = 10. bar. Calculate Q and predict in what direction the reaction will proceed to reach equilibrium.
2) Calculate the numeric value of the equilibrium constant K for reaction at 298 K: 2 NO2 (g) → N₂O4 (g) from Data Section: les of das Athina.pdf-Adebe Acrobat Reader (54-b0) You SignWindow H Tools Home 827-31.40 - Tables of data Atkin x a Table 2.7 (Continued) Neon Ne(g) Nitrogen N₂(g) N(g) NO(g) N₂O(g) NO₂(g) N₂O₂(g) N₂O5(s) N₂O,(g) 1081 (12 of 4) TTATO (11 A M/(g mol-¹) 20.18 28.013 14.007 30.01 44.01 46.01 92.1 108.01 108.01 OO 201 8. P AH*/(kJ mol-¹) 0 0 +472.70 +90.25 +82.05 +33.18 +9.16 -43.1 +11.3 174 17 AG/(kJ mol-¹) 0 0 +455.56 +86.55 +104.20 +51.31 +97.89 +113.9 +115.1 ℗ 30 31 x Sign In &00 S B D 2 C %
For the reaction X(g) + 2Y(g) = 3Z(g) K, = 2.08x10-2 at a temperature of 325 °C. Calculate the value of Kc . Express your answer numerically. View Available Hint(s) V ΑΣφ K = %3D