Part A Consider the reaction: CO(g) + 2H2(g) = CH;OH(9) What is the value of the equilibrium constant at this temperature? An equilibrium mixture of this reaction at a certain temperature was found to have Pco = 0.115 bar , PH2 = 0.118 bar and PCH OH = 0.180 bar . ? K =

The first step in the industrial synthesis of hydrogen is the reaction of steam and methane to give carbon monoxide and hydrogen at 1400 K. H2O(g) + CH4(g) ⇋ CO(g) + 3H2(g) The equilibrium constant, K, is equal to 4.7 at 1400 K. A mixture of reactants and products at 1400 K contains 0.035 M H2O, 0.050 M CH4. 0.15 M CO, and 0.20 M H2. (a) Is this reaction at equilibrium? Hint: how does your calculated ratio of products to reactants compare to the equilibrium constant noted above. (b) In which direction does the reaction proceed to reach equilibrium?

Consider the following reactions and their respective equilibrium constants: NO(g) + Br2 (9) =NOB|(9); K = 5.3 2NO(g) = N2(9)+O2 (g); K = 2.1 x 1030 Use these reactions and their equilibrium constants to predict the equilibrium constant for the following reaction: N2(9) + O2 (g) +Br2 (g) 2NOB1(g) Express your answer using two significant figures. | ? K =

Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HF (aq) + OH- (aq)F- (aq) + H2O (l)   K =

At a certain temperature, Kc = 6.0 x 10^-4 for the reaction between sulfur trioxide gas and gaseous hydrogen fluoride to produce gaseous sulfur hexafluoride and water vapour: SO3(g) + 6HF(g) = SF6(g) + 3H20(g) Calculate the equilibrium concentration of sulfur hexafluoride that would result if 1.8 mol of sulfur trioxide was mixed with 5.6 mol of hydrogen fluoride in a 2.1 L container.

The equilibrium constant for the chemical equation N,(g) + 3 H, (g) 2 NH,(g) is K, 0.356 at 197 °C. Calculate the value of the K, for the reaction at 197 °C. K.

Calculate the value of Kc.

Be sure to answer all parts. The following reactions have the indicated equilibrium constants at a particular temperature: N₂(g) + O₂(g) 2NO(g) Ke=4.3 × 10-25 2NO(g) + O₂(g) = 2NO₂(g) K=6.4 × 10⁹ Determine the value of the equilibrium constant for the following equation at the same temperature: N₂(g) +20₂(g) = 2NO₂(g) Ke= 10 (Enter your answer in scientific notation.)

An equilibrium constant of special importance in much aqueous chemistry is that of the autoionization of water: 2 H₂O (/) H3O+ (aq) + OH¯ (aq) Kw The value of this equilibrium constant at three temperatures near standard temperature is Kw(293 K) = 0.67 × 10-¹4 M² Kw(298 K) = 1.00 × 10-¹4 M² Kw(303 K) = 1.45 × 10-¹4 M² (a) Assuming that the value of AH° and AS° are constant over this narrow temperature range, determine their values (in kJ/mol and J/mol-K, respectively for the ionization equilibrium at 298 K based on this information. (Hint: You should use both the relationship between AG° and K, and the relationship between the Gibbs energy, enthalpy, and entropy in this problem. Setting up your analysis as a least-squares linear fit provides the best result.) (b) Based on the results from part (a), what would you expect the autoionization equilibrium constant to be near the freezing point of water, at T = 275 K?

Consider the following chemical equilibrium: 4 NH; (g) + 3 0, (g) =2N, (g)+6H,0 (g) Now write an equation below that shows how to calculate K, from K, for this reaction at an absolute temperature T. You can assume T is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator.