Using the law of mass action, write the equilibrium expression for each of the following reactions. (a) 3 CH½(g) + 3 H½(g) 2 CI112(€) (b) CO2(g) + C(s) 2 2 CO(g) (c) CF4(g) + 2 H;O(€) = CO2(g) + 4 HF(g) (d) K2NİF6(s) + TIF4(s) 2 K,TiF,(s) + NIF2(s) + F2(g)
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- Simple acids such as formic acid, HCOOH, and acetic acid, CH3COOH, are very soluble in water; however, fatty acids such as stearic acid, CH3(CH2)16COOH, and palmitic acid, CH3(CH2)14COOH, are water-insoluble. Based on what you know about the solubility of alcohols, explain the solubility of these organic acids.The equilibrium constant, Kc , for the reaction 2 SO2 (g) + O2 (g) → 2 SO3 (g) is 6.90 x 103 . (a) What is Kc for the reaction 2 SO3 (g) → 2 SO2 (g) + O2 (g) (b) What is Kc for the reaction SO2 (g) + 1/2 O2 (g) → SO3 (g)3. (a) (b) (c) (d) Write the expression for the equilibrium constant (K) of the following reactions: Fe2+ (aq) + 2OH(aq) Fe(OH)₂ (s) CH4 (g) + 3 H2O (g) = CO (g) + 3 H₂ (g) 2 NO(g) + O₂(g) = 2 NO₂ (g) 2+ Zn(s) + Cu²+ (aq) = Zn²+ (aq) + Cu(s)
- Be sure to answer all parts. Given the value of the equilibrium constant (K) for equation (a), calculate the equilibrium constant for equation (b). 2 (a) O2(g) S,03(g) K = 8.58 × 10-9 %3D х 10 (Enter your answer in scientific notation.) (b) 302(g) 5 203(g)11) Into a 1.00 liter flask is placed 0.822 moles of SO3. At equilibrium 36.7% of the SO3 has decomposed. What is the value of the equilibrium constant? 2 SO3 (g) « 2 SO2 (g) + O2 (g)Kc = ?Be sure to answer all parts. Given the value of the equilibrium constant (K) for equation (a), calculate the equilibrium constant for equation (b). (a) O2(g) 5 K = 6.36 × 109 (b) 302(g) 5 203(g) K = X 10 (Enter your answer in scientific notation.)
- The Born-Haber process is, N2 (g) + 3 H2 (g) = 2 NH3 (g) has an equilibrium position when [N2] = 12.9 M, [H2] = 0.600 M and (NH3] =0.500 M. (a) What is the value of K? (b) If [N2] = 2.30 M, [H2] = 0.500 M and (NH3] =0.150 M, then are these concentrations at an equilibrium position? If not, then in which direction will a shift bring about equilibrium?Oxygen can be converted into ozone by the action of lightning or electric sparks: 30₂(g) 203(g) For this reaction, AH = +68 kcal/mol (+285 kJ/mol) and K = 2.68 X 10-2⁹ at 25 °C. (a) Is the reaction exothermic or endothermic? (b) Mention whether the equilibrium shifts to the left or right when Increasing pressure by decreasing volume. (c) Mention whether the equilibrium shifts to the left or right when increasing the concentration. of O3(g). (d) Mention whether the equilibrium shifts to the left or right when increasing the temperature.Interconvert K, and Kc values. Calculate Kp for the following reactions at the indicated temperature. (a) PCl3(g) + Cl₂(g)=PCI5(g) Kc = 200 at 479 K Kp = (b) NH4l(s) NH3(g) + HI(g) K = 1.34×10-³ at 651 K Kp =
- Carbon monoxide and water vapor, each at 200. Torr, were introduced into a container of volume 0.250 L. When the mixture reached equilibrium at 700 degrees Celsius, the partial pressure of CO2(g) was 88 Torr. Calculate the value of K for the equilibrium CO (g) + H2O (g)⇋ CO2(g)+H2(g).Select the reaction for which K, = Kc. 2 Na,0,(s) + 2 CO,(g) =2 Na,CO3(s) + 0,(g) 2 KCIO3 (s) = 2 KCI(s) + 30,(g) 2 H,S(g) + SO,(g)= 3 S(s) + 2 H,O(g) Br, (g) + Cl,(g) 2 BRCI(g)5) 25.0 g of HI(g) is injected into a 4.00 L reaction vessel that contains 20.0 g of I2(g). When the system comes to equilibrium at 400°C, what will be the total pressure inside the reaction vessel? 2HI(g) H2 (g) + I2(g), K 0.0156 at 400°C %3!