For the reaction CO(g) + 3 H2(g) H2O(g) + CH4(g), Kc = 190 at 1000 K. If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.036 M, [H2] = 0.045, [H2O] = 0.020,and [CH4] = 0.031, in which direction will a reaction occur and why? A) it is at equilibrium because Q = 190 B) toward products because Q = 4.1 C) toward reactants because Q = 0.24 D) toward products because Q = 0.38 E) toward reactants because Q = 61

21. Consider the hypothetical reaction at 355K Z(g) + R (g) D O 2Q (g) Keq = 2.71 What are the equilibrium concentrations of all the gases if all the gases have an initial concentration of 0.288 M?

8. Please don't write on a paper. I can't understand handwritten.

Danie Carbon dioxide and water react to form methane and oxygen, like this: CO2(9)+2H,O(9) → CHĄ(g)+2O¿(g) The reaction is endothermic. Suppose a mixture of CO,, H,O, CH, and O, has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation change in composition shift in equilibrium O to the right The temperature is raised. The pressure of H20 will ? O to the left O (none) O to the right The temperature is lowered. O to the left The pressure of CH4 will ? O (none) Submit Assi Continue O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center| Ac 43,203 FEB 18 PP ESS MacBook Air

At 800 K, the equilibrium constant for the reaction A2(g) = 2A(g) is Kc = 3.1 * 10-4. Assuming both forward and reverse reactions are elementary reactions,which rate constant do you expect to be larger, kf or kr?

The KP for the reactionSO2Cl2(g) ↔ SO2(g) + Cl2(g)is 2.05 at 648 K. A sample of SO2Cl2is placed in a container and heated to 648 Kwhile the total pressure is kept constant at 9.00 atm. Calculate the partialpressures of the gases at equilibrium

63) A student mixes two solutions: 10.0 mL of 0.0040 mol/L lead (II) nitrate, Pb(NO3)2 (aq), and 15.0 mL of 0.25 mol/L potassium chloride, KCI (aq). If the solubility product constant, Ksp, for lead (II) chloride, PbC12, is 1.2 x 105 at 25 °C, will a precipitate from when these two solutions are mixed? Why? ne bronsied - LoWry theory, Dut no

The equilibrium constant, Kp, for the following reaction is 1.57 at 600 K: CO(g) + Cl2(g) =CoCl2(g) Calculate the equilibrium partial pressures of all species when CO and Cl2, each at an intitial partial pressure of 1.09 atm, are introduced into an evacuated vessel at 600 K.

Initially, 1.50 M of ammonia (NH3) were placed in an empty container without any other gases at 789K. It started to decompose according to the chemical equation below: 2 NH3(g) = N₂(g) + 3 H₂(g) After equilibrium was established, it was found that there are 0.055 M of ammonia left in the same vessel. What is the equilibrium constant, Kc, for this reaction at 789 K? 3.5 28 9.8 x 103 2.4 x 10³ O4.8 x 104

Gas Initial Concentration (M) H2 0.030 I2 0.015 HI ? Samples of three gases, H2(g) , I2(g) , and HI(g) , were combined in a rigid vessel. The initial concentrations of H2(g) and I2(g) are given in the table above. (a) The original value of the reaction quotient, Qc , for the reaction of H2(g) and I2(g) to form HI(g) (before any reactions take place and before equilibrium is established), was 5.56 . On the following graph, plot the points representing the initial concentrations of all three gases. Label each point with the formula of the gas.   Equilibrium was established at a certain temperature according to the following chemical equation. H2(g)+I2(g)⇄2HI(g)ΔH°rxn=−9.4kJ/molrxn;Kc=49 After equilibrium was established, the concentration of H2(g) was 0.020M . (b) On the graph above, carefully draw three curves, one for each of the three gases, starting from the initial points you drew in part ( a ). The curves must show how the concentration of each of the three gases changed…