The equilibrium constant, K, for the following reaction is 4.33E-4 at 554 K: NH4

Question

The equilibrium constant, K, for the following reaction is 4.33E-4 at 554 K:

NH4Cl(s) NH3(g) + HCl(g)

An equilibrium mixture in a 19.6 L container at 554 K contains 0.278 mol NH4Cl(s), 2.62E-2 M NH3 and 1.65E-2 M HCl. What will be the concentrations of the two gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 10.2 L?

I am suppose to use Le Chatelier's Principle and the quadratic equation but I can figure out how to do the quadratic equation.

Explanation / Answer

The Standard Form of a Quadratic Equation looks like this: The letters a, b and c are coefficients (you know those values). They can have any value, except that a can't be 0. The letter "x" is the variable or unknown (you don't know it yet)

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