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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