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Where the concentrations are the concentrations at equilibrium. The Law of Mass Action for this reaction would normally be written as: That's all there is to the construction of an ICE table! This means we just add the `I` and `C` boxes:
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Notice that the equilibrium position is just the initial position plus whatever the change was. The `"E"` is going to be the position at equilibrium. If the amount of the species is increasing, the change term is position. If the amount of the species is decreasing, the change term is negative. The x term is always going to be multiplied by the coefficient of the species. Īnother way to think of it: equations express the change in a reactant in the coefficient. The same logic applies to `H_2` : since the amount of `H_2` that's produced is the `3x` the amount of `N_2`, we can express the change in `H_2` as `+3x`. Since the amount of `NH_3` that dissociates is going to be `2x` the amount of `H_2` that is produced, we can express the change in `NH_3` as `-2x` and the change in `N_2` as `+x`. This means that the `NH_3` is going to break apart to form `N_2` and `H_2`. Think of it this way: we're assuming that the reaction will proceed in the rightward direction since the `K_C` is a somewhat large value. The change term is probably the most confusing part of ICE tables. Therefore, the `x` value will be different for each species because a different amount of each species is reacting: For this reaction in particular, every `"mol"` of `N_2` that reacts must react with `3 "mol" H_2` to form `2 "mol"` of `NH_3`. Recall from stoichiometry and your understanding of chemical equations that the coefficient in front of a reactant indicates the stoichiometric amount of the reactant that reacts. Since we don't know the change, we're going to represent the change as a variable `x`. The `"C"` row stands for the change in the reaction's position. Now, we're going to fill in the `"C"` row. The only difference is, well, we're using pressure. The procedure for using pressure in ICE tables is nearly identical to that of concentration. Put those values into the `"I"` row of the table, representing the initial position.
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As a brief reminder, the units of concentration are `"moles"/"L"`. First, convert all of the values to units of concentration. For ICE tables, we use either concentration or pressure. Now, we're going to put in the initial conditions. The starting table should look something like this: Since we have 3 species, we're going to have 4 columns (one of the columns just contains the I, C, and E). ICE tables will always have 3 rows (for I,C, & E). To do this, we're going to construct an ICE table. We're given an initial starting position and want to find the final equilibrium position. Determine the equilibrium concentrations. We're going to go step by step into the construction of a basic ICE Table. The technique we're going to use is the construction of an ICE table, where "I" stands for "Initial," "C" for "Change," and "E" for "Equilibrium." In this section, we're going to go over a technique that allows us to predict the position of equilibrium. How many grams of NaNO 3 are produced when 5.3 grams of Na 2CO 3 are added to 250.0 mL of 0.So far, we've gone over the ideas of chemical equilibria and the equilibrium constant. In this module, these five steps will be used to solve the following stoichiometry problem (this problem will appear on all subsequent pages): Step 4: Determine the Change (moles) amount for one substance in
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Step 3: If any of the known information is given as a mass or Step 2: Decide what information about the problem is known and
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Any stoichiometry problem can be solved by following the same series of steps: