Write the equation for the reaction that corresponds to each of the following reaction quotients.
(a)
(b)
(c)
(d)
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CHEMISTRY: ATOMS FIRST VOL 1 W/CONNECT
- Consider the following hypothetical reactions and their equilibrium constants at 75C, 3A(g)3B(g)+2C(g)K1=0.31 3D(g)+2B(g)2C(g)K1=2.8 Find the equilibrium constant at 75C for the following reaction A(g)D(g)+53B(g)arrow_forwardThe following two diagrams represent the composition of an equilibrium mixture for the reaction A2 + B2 2AB at two different temperatures. Based on the diagrams, is the chemical reaction endothermic or exothermic? Explain your answer using Le Chteliers principle. (A atoms are red and B atoms are green in the diagrams.)arrow_forwardThe equilibrium constant, Kc, is 1.05 at 350 K for the endothermic reaction 2 CH2Cl2(g) CH4(g) + CCl4(g) Which of the diagrams for Question 111 represents an equilibrium mixture at 350 K? Diagrams for Question 111.arrow_forward
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- Write the mathematical expression for the reaction quotient, QC, for each of the following reactions (a) N2(g)+3H2(g)2NH3(g) (b) 4NH3(g)+5O2(g)4NO(g)+6H2O(g) (C) N2O2(g)2NO2(g) (d) CO2(g)+H2CO(g)+H2O(g) (e) NH4CI(s)NH3(g)+HCI(g) (f) 2Pb( NO3)2(s)2PbO(s)+4NO2(g)+O2(g) (g) 2H2(g)+O2(g)2H2O(g) (h) S8(g)8S(g)arrow_forwardAt 1 atm and 25 C, NO2 with an initial concentration of 1.00 M is 3.3103 decomposed into NO and O2. Calculate the value of the equilibrium constant for the reaction. 2NO2(g)2NO(g)+O2(g)arrow_forwardDistinguish between the terms equilibrium constant and reaction quotient. When Q = K, what does this say about a reaction? When Q K, what does this say about a reaction? When Q K. what does this say about a reaction?arrow_forward
- Given the following descriptions of reversible reactions, write a balanced net ionic equation (simplest whole-number coefficients) and the equilibrium constant expression (K) for each. (a) Liquid acetone (C3H6O) is in equilibrium with its vapor. (b) Hydrogen gas reduces nitrogen dioxide gas to form ammonia and steam. (c) Hydrogen sulfide gas (H2S) bubbled into an aqueous solution of lead(ll) ions produces lead sulfide precipitate and hydrogen ions.arrow_forwardSuppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?arrow_forwardFor the reaction A2 + 2B 2AB, diagram I depicts an initial reaction mixture, where A2 molecules are red and B atoms are green. Which of the diagrams II through IV is a possible equilibrium state for the reaction system? There may be more than one correct answer.arrow_forward
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