Question

A student ran the following reaction in the laboratory at 295 K:

2NO(g) + Br₂(g) <---> 2NOBr(g)

When she introduced 0.153 moles of NO(g) and 0.123 moles of Br₂(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.117 M.

Calculate the equilibrium constant, K_c, she obtained for this reaction.

K_c = ____

The equilibrium constant, K_c, for the following reaction is 6.50×10^-3 at 298K.  

2NOBr(g) <---> 2NO(g) + Br₂(g)

If an equilibrium mixture of the three gases in a 14.8 L container at 298K contains 0.393 mol of NOBr(g) and 0.416 mol of NO, the equilibrium concentration of Br₂ is ____M.

Answer 1