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- solu tion ammonivm oxelete solu tion added of is to Chloride. of G Wite the Penta mmine chlolo wbal1 bulenced cqu equation for above reactio n -OWLV2 | Online teaching and I X + ow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-take K [Review Topica] [References] ts (M) Use the References to access important values if needed for this question. M) The equilibrium constant, K„, for the following reaction is 2.74 at 1.15×10³K. M) 2SO3(g) 2SO2(g) + O2(g) M If an equilibrium mixture of the three gases in a 13.7 L container at 1.15×10°K contains S0z at a pressure of 1.17 atm and atm. SO2 at a pressure of 1.47 atm, the equilibrium partial pressure of O2 isThe equilibrium constant for the reachin is 49 at 4sor. 24. following reachion the into Fo.22mole of t2,0.22mile of rm, H,and 0-66mcle of HI were H.r AT were Put into enevacuated TL container would the sustem be at equiliforem? HE not, what must ocur to eguilioim) Heoit b=レHI sCcur estableh GJ
- Given that the Ka for HOCl is 3.5 10-8, calculate the K value for the reaction of HOClwith OH- at 25oC.im/takeAssignment/takeCovalentActivity.do?locator=assignment-take [References] Use the References to access important values if needed for this question. Solid potassium bromide is slowly added to 125 mL of a 0.0542 M silver nitrate solution. The concentration of bromide ion required to just initiate precipitation is М.Use the References to access important values if needed for this question. The value of K, for phenol (a weak acid) , C,H3OH , is 1.00×10-10. Write the equation for the reaction that goes with this equilibrium constant. (Use H30* instead of H*.) Submit Answer Retry Entire Group No more group attempts remain
- 1. Which of the following correctly describes the equilibrium constant for the gas-phase reaction between Hland Ozlto form gaseous Ke a) [H2O] [H2](O2) Ke b) [H2O]2 [H2](O2) K. = c) [H2O]2 [H2]2(O2) Ke d) [H2[02] [H2O]2 e) K.Le Châtelier’s principle is related ultimately to the rates ofthe forward and reverse steps in a reaction. Explain (a) why anincrease in reactant concentration shifts the equilibrium positionto the right but does not change K; (b) why a decrease in Vshiftsthe equilibrium position toward fewer moles of gas but does notchange K; (c) why a rise in Tshifts the equilibrium position of anexothermic reaction toward reactants and also changes K;and(d) why a rise in temperature of an endothermic reaction from T1to T₂ results in K₂ being larger than K1Use the References to access important values if needed for this question. The value of K, for quinoline, C,H-N, is 6.30×10-10. Write the equation for the reaction that goes with this equilibrium constant. It is not necessary to include states such as (ag) or (1). Submit Answer Retry Entire Group No more group attempts remain
- Fill in the correct “changes” in concentration terms for the following unbalanced equations, (e.g. “+y”, “-2y”, shown in bold in the Ex.) etc, in order to establish equilibrium.NOTE: if you start with a species on the product’s side, that side must lose an amount. Const. T & P. Example: 2 SO3ó 2 SO2 + Cl2(IS balanced) “x” “x” Change: +2y -2y -y a)CH4(g) + O2(g) ó CO2(g) + H2O(g)(unbalanced) “x”“x” Change:_______________ ______ b)H2O(g) + ó H2(g) + O2(g)(unbalanced) “x” “x” Change:__________ ______An aqueous solution of acetic acid is found to havethe following equilibrium concentrations at 25 °C:[CH3COOH] = 1.65 x 10-2 M; [H+] = 5.44 x 10-4 M; and[CH3COO-] = 5.44 * 10-4 M. Calculate the equilibriumconstant Kc for the ionization of acetic acid at 25 °C. Thereaction isCH3COOH(aq) ⇌ H+(aq) + CH3COO-(aq)(a) The molar s o l u b i l it y o f PbBr2 at 25 °C i s1.0 x10-2 mol/L. Calculate Ksp. (b) If 0.0490 g of AgIO3 dissolvesper liter of solution, calculate the solubility-productconstant. (c) Calculate the pH of a saturated solution of Ca(OH)2.