What is the equilibrium constant expression for 3Cl2(g) + NH3(g) = NC13(g) + 3HCI(g)? [NH, ][Cl,] [NCI, ][HCI] [NH, ][Cl,} [NCI, J[HC1} [NCI, ][HCI] [NH,][Cl,] (А) К. (В) К, . %3D [NCI, J[HCI} [NH, ][Cl,]' (C) K̟ (D) K.

Which is the correct equilibrium constant expression for the following reaction? NiO(aq) + H2(g) Ni(l) + H2O(g)       a)  Kc = [H2]/[H2O]   b)  Kc = [NiO] [H2]/[Ni][H2O]   c)  Kc = [H2O]/[H2][NiO]   d)  Kc = [Ni][H2O]/[NiO] [H2]   e)  Kc = [Ni] [H2O]/[H2]

a Choose the equilibrium expression for the following heterogeneous equilibrium: Cag N2 (s) +6H, 0(1) = 3Ca(OH)2 (8) + 2NH, (g) OK= [NH," [Ca(OH),) K = [Ca, N2] NH, [Ca(OH), [Ca,N2][H,O]° [NH,] K = 16 券 K= [H, O]° b Choose the equilibrium expression for the following heterogeneous equilibrium: 4Fe(s) +302(g) 2Fe, O3 (s) 1. K = OK= [0,1'[Fe(s)] Fe, Os = [0,] OK- K 3. 1. [02]

At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant, Kc, which is a mathematical expression based on the chemical equation. For example, in the reaction aA+bB⇌cC+dD where a, b, c, & d are the stoichiometric coefficients, the equilibrium constant is Kc=[C]c[D]d[A]a[B]b & where [A][A], [B][B], [C][C], and [D][D] are the equilibrium concentrations. If the reaction is not at equilibrium, the quantity can still be calculated, but it is called the reaction quotient, Qc, instead of the equilibrium constant, Kc.Qc=[C]tc[D]td[A]ta[B]tb where each concentration is measured at some arbitrary time t. Part A  A mixture initially contains AA, BB, and CC in the following concentrations: [A]= 0.700 M, [B]= 1.40 M, & [C]= 0.550 M. The following reaction occurs and equilibrium is established: A+2B⇌CA+2B⇌C At equilibrium, [A]= 0.520 M & [C]= 0.730 M. Calculate the value of the equilibrium constant, Kc.

Express the equilibrium constant for this reaction:   2 NH3(g) <=>  N2(g) + 3 H2(g)     K = [NH3]2 / ([NH3]2 x [N2])     K = ([NH3]2 x [N2]) / [H2]3     K =  ([N2] x [H2]3) / [NH3]2

O KINETICS AND EQUILIBRIUM Helen v Using the small x approximation to solve equilibrium problems A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 3 O2(g) = 203(g) K,= 1. x 10-6 d. He fills a reaction vessel at this temperature with 15. atm of oxygen gas. Use this data to answer the questions in the table below. olo Can you predict the equilibrium pressure of O3, using only the tools O yes available to you within ALEKS? O no If you said yes, then enter the equilibrium pressure of O, at right. I atm Round your answer to 1 significant digit. Explanation Check II

At equilibrium, the concentrations in this system were found to be [N,] = [0,] = 0.200 M and [NO] = 0.500 M. %3D %3D %3D N,(g) + 0,(g) =2 NO(g) If more NO is added, bringing its concentration to 0.800 M, what will the final concentration of NO be after equilibrium is re-established? [NOJfinal %3D TOOLS x10 about us privacy policy terms of, use contact us help careers 4:40 A 4/25/20 End Insert 888 F12 Home Pく F7 F9 F10 F11 F4 F5 F6 F8

-cnow-owl.cengagenow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator-assignment-take S ot ts This question has multiple parts. Work all the parts to get the most points. [References] Phosphorus pentachloride decomposes at high temperatures. PCl5 (g) PC13 (g) + Cl2 (g) An equilibrium mixture at some temperature consists of 3.56 g of PCl5, 4.86 g of PCl3, and 3.59 g of Cl2 in a 1.00-L flask. a If you add 1.31 g of Cl2, how will the equilibrium be affected? shift left shift right no shift will occur pt pts 1 pt b What will the concentration of PC15 be when equilibrium is reestablished after addition of 1.31 g Cl₂? 1 pt [PC15] = mol/L 1 pt Submit 1 pt 1 pt Submit Answer Try Another Version 4 item attempts remaining ent 80 a F4 F2 F3 # SA % Cengage Learning | Cengage Technical Support F5 1 MacBook Air F6 A DII F7 F8 * A F9

Write the equilibrium expression for 2NO(g) + 2H2(g) = N2(g) + 2H20(g). a. Ke = [H20]2 [N2] / [NO]² [H2]² O b. Kc [N2]/ [NO]2 [H2]? %3D O c. Ke [NO]? [H2]? / [H2O]² [N2] %3D

Nitrogen monoxide, NO, is formed in automobile exhaust by the reaction of N2 and Og (from air). N2 (9) + O2(9) - 2NO(9) The equilibrium constant (K.) is 0.0025 at 2127°C. If an equilibrium mixture at this temperature contains 0.082 mol N, and 0.026 mol O2 per liter, what is the concentration of NO? Concentration = M