You are a chemical engineer that is responsible for synthesizing a new drug. You look at a series of potential chemical reactions that will make your drug along with their respective K values. What type of K value would you be looking for and why?

The chemical equation shown is an exothermic process. 2 SO, (g) + 0,(g) 2 SO,(g) exothermic Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after decreasing the temperature. The concentration of SO, will increase. decrease. stay the same.

For the chemical equation 2SO2(g) + NO2(g) 2SO3(g) + NO(g) The equilibrium constant at a certain temperature is 5.50. At this temperature, calculate the number of moles of NO2(g) that must be added to 1.20 mol SO2(g) in order to form 0.80 mol SO3(g) at equilibrium.

True/False. Explain your answer in one sentence or less.   In an equilibrium process, the concentrations of products and of reactants are equal. The value of the equilibrium constant for a given reaction depends on the initial concentrations of reactants. Large value for equilibrium constant K means the reaction will be less complete at the equilibrium point. The concentration of a pure solid is left out of an equilibrium constant expression but a pure liquid is included.

Consider the combustion of methane (as represented by the following equation). This is the reaction that occurs for a Bunsen burner, which is a source of heat for chemical reactions in the laboratory. CH 4(9) +20 2(g) =CO2(g) + 2H 20(g) For the system at chemical equilibrium, which of the following explains what happens if the temperature is reduced? O a. The equilibrium position is shifted to the left and the value for K increases. O b. The equilibrium position is shifted to the right and the value for K increases. O c. The equilibrium position is shifted to the right and the value for K decreases. O d. The equilibrium position is shifted but the value for K stays constant. Oe. The equilibrium position is shifted to the left and the value for K decreases.

Calculating an equilibrium constant from a partial equilibrium composition

Consider the equilibrium system described by the chemical reaction below. Determine the concentration of O, at equilibrium by writing the equilibrium constant expression and solving it. Complete Parts 1-2 before submitting your answer. = 2 H₂O(g) 2 H2(g) + O̟₂(g) 1 2 NEXT At this temperature, the Kc = 2.4 × 103 and the equilibrium concentrations of H2O and H2 are 0.11 M and 0.019 M, respectively. If [x] represents the equilibrium concentration of O2, set up the equilibrium expression for Kc to solve for the concentration. Each reaction participant must be represented by one tile. Do not combine terms. Кс = 2' = 2.4 × 103 > RESET [0.11] [0.019] 2[0.11] 2[0.019] [0.11]² [0.019]² [x] [x]² [2x] [2x]²

Consider the following reaction at equilibrium. What effect will removing some SO2 have on the system? SO2(g) + NO2(g) = SO3(g) + NO(g) The pressure of SO3 will increase The equilibrium constant will decrease. No change will occur since SO2 is not included in the equilibrium expression. The pressure of NO2 will increase. The reaction will shift to decrease the pressure.

For the chemical equation SO, (g) + NO, (g) = So, (g) + NO(g) the equilibrium constant at a certain temperature is 2.70. At this temperature, calculate the number of moles of NO, (g) that must be added to 2.75 mol SO,(g) in order to form 1.10 mol SO, (g) at equilibrium. moles of NO,(g): mol

What does it mean for a chemical reaction to reach equilibrium?         The rates of the forward and reverse reactions are equal. The concentrations of the reactants and products are also equal.         The rates of the forward and reverse reactions are increasing. The concentrations of the reactants and products are equal.         The rates of the forward and reverse reactions are equal. The concentrations of the reactants and products are constant.         The rates of the forward and reverse reactions are increasing. The concentrations of the reactants and products are also increasing.