Tiny samples of aqueous solutions are sketched below, as if under a microscope so powerful that individual molecules could be seen. (The water molecules are not shown.) The two substances in each sample can interconvert. That is, each kind of molecule can turn into the other. The equilibrium constant K for each Interconversion equilibrium is shown below the sketch. Decide whether each solution is at equilibrium. 000 V K=9 K=- At equilibrium? At equilibrium? Oyes O no O yes O no K= K=3 At equilibrium? At equilibrium? O yes O no O yes O no

General Chemistry 4th Edition McQuarrie Rock Gallogly University presentedi The equilibrium constant for the chemical equation N,(g) + 3 H, (g) =2 NH,(g) is K, = 0.139 at 237 °C. Calculate the value of K. for the reaction at 237 °C. Ke =

Consider the following equilibrium reaction: PBr5(g) + 1/2 O2(g) = POB13(g) + Br2(g) Kc = 5.6 x 102 at 512 K Calculate K. for the reaction 2 PBr5(g) + O2(g) = 2 POBR3(g) + 2 Br2(g) at the same temperature. 24 1.1 x 103 280 5.6 x 102 O None of these 3.2 x 105

Consider the following chemical equilibrium: 4 NH, (g) +3 0, (g)=2N, (g) +6 H,Oo (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. K_ = I

19. Given the following reaction: NH.CI (s) S NH3 (g) + HCI (g) AH= +42.1 kcal Suppose the above substances in the reaction are at equilibrium at 600 K in volume V and at pressure P. State whether the partial pressure of NH3 (g) will have increased, decreased, or remained the same in order to the equilibrium to be reestablished following the disturbances of the original system. Note that some solid remains in the flask at all times. Provide a one to two sentence explanation (a) The temperature of the system is increased (b) The volume of the system is increased (c) A quantity of gaseous NH3 is added. (d) A small quantity if NH4C1 is added.

Calculating equilibrium composition from an equilibrium... 0/5 Suppose 500. mL flask is filled with 1.9 mol of H, and o0.50 mol of C1,. The following reaction becomes possible: H, (g) + Cl,(g) – 2HC1(g) The equilibrium constant K for this reaction is 3.61 at the temperature of the flask. Calculate the equilibrium molarity of H,. Round your answer to two decimal places. OM

I need to find the mols of CO, H2O, CO2, and H2 respectively within the mixture when it reaches equilibrium.

At 400 K, an equilibrium mixture of H2, 12, and HI consists of 0.065 mol H2, 0.079 mol 12, and 0.13 mol HI in a 4.50-L flask. What is the value of K, for the following equilibrium? (R= 0.0821 L atm/(K • mol)) 2HI(g) = H2(g) + 12(8) 0.29 8.2 0.039 O 26 3.4

Note:- • Do not provide handwritten solution. Maintain accuracy and quality in your answer. Take care of plagiarism. • Answer completely. • You will get up vote for sure.

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S,(g) + C(s) = CS, (g) K. = 9.40 at 900 K How many grams of CS, (g) can be prepared by heating 13.0 mol S,(g) with excess carbon in a 5.70 L reaction vessel held at 900 K until equilibrium is attained? mass of CS,(g):