is a substance that increases the rate of reaction but has no effect on the equilibrium composition of a reaction mixture. P A Moving to another question will save this response.

Increasing the concentration of the reactants will slow down the reaction. O true O false

Consider the reaction. NaC2O2H3(s) <--- H2O ------> NaC2O2H3(aq), which is at equilibrium in an open flask in the lab at room temperature. You add more water to the equilibrium mixture. When the system reestablishes equilibrium, what has changed?  a. the concentration of NaC2H3O2(aq) does not change b. heat is produced c. the concentration of NaC2H3O2(aq) decreases d. the concentration of the water increases

Define equilibrium in terms of  a)reaction rates   -Forward reaction rate = reverse reaction rate b)changes in observable properties   -There are no observable changes c)energy and energy changes   -Energy has become stable (no longer giving off or taking in heat)

Decide whether each of the following statements is true or false.  If false, change the wording of the statement to make it true.   a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction.  d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). e) For the reaction CaCO3 (s) ↔ CaO (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.

Chapter 1 question 6: Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 50.0L tank with 4.6 mol of ammonia gas and 4.5 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 1.2 mol. Calculate the concentration equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits.

i See Periodic Table See Hin Increasing the concentration of a reactant shifts the position of chemical equilibrium towards formation of more products. What effect does adding a reactant have on the rates of the forward and reverse reactions? Choose one: O There is no effect on the forward and reverse reactions. For an equilibrium reaction, the forward and reverse rates are always equal. O Both the forward and reverse reactions speed up by the same amount. O The forward reaction speeds up immediately. As more product is made, the reverse reaction starts to speed up as the forward reaction starts to slow down until they are equal. O The forward reaction slows down initially. As the reaction proceeds, the reverse reaction slows down to meet the new forward reaction. O The forward reaction speeds up. Eventually, production of the product speeds up the reverse reaction rate to match the new forward rate. O It is impossible to say without more specific information.

K values are often written and scientific notation. If a K value has a positive power of 10 does equilibrium favor the products or reactants.

= KINETICS AND EQUILIBRIUM Setting up a reaction table Suppose a 500. mL flask is filled with 1.7 mol of N₂ and 0.10 mol of NH3. This reaction becomes possible: N₂(g) + 3H₂(g)2NH, (g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of N₂. You can leave out the M symbol for molarity. initial change equilibrium N₂ 0 0 H₂ 0 0 0 NH3 0 0 00 1/5 X

A reaction begins with a solution containing reactants but no products. When the reaction reaches equilibruim a) The enthalpies of the reactants and products are equal b) The concentrations of the reactants and products are equal c) The equilibrium constant has decreased relative to its value at the start of the reaction d) The forward and reverse rate constants are equal e) None of the above