# At a certain temperature, 0.4211 mol of N2 and 1.701 mol of H2 are placed in a 3.50-L containerN2(g)+3H2(g) <--->2NH3(g)At equilibrium, 0.1801 mol of N2 is present. Calculate the equilibrium constant, Kc.

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At a certain temperature, 0.4211 mol of N2 and 1.701 mol of H2 are placed in a 3.50-L container

N2(g)+3H2(g) <--->2NH3(g)

At equilibrium, 0.1801 mol of N2 is present. Calculate the equilibrium constant, Kc.

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Step 1

The following reaction takes place and the initial moles of hydrogen and nitrogen are given. Also, the number of moles of nitrogen at equilibrium is given. Using the given info, let us construct the ICE table

Step 2

Now we know the number of moles of N2 at equilibrium, hence,

Number of moles of N2 at equilibrium = 0.4211 – x = 0.1801

Therefore, x = 0.241 mol

Now, let us calculate the concentration at equilibrium,

Step 3

Now using the concentrations, let us calculate the equ...

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