![]() Now, because #Q_c > K_(eq)#, the equilibrium will shift to the left, i.e. #Q_c = (_t)/(_t * _t) -> # does not use equilibrium concentrations! you should expect the equilibrium concentration of hydrogen bromide to be higher than the equilibrium concentrations of hydrogen gas and bromine gas.īefore moving on to the calculations, use the given values to calculate the reaction quotient, #Q_c#, which can be used to determine the direction in which the equilibrium will proceed when these concentrations of reactants and product are mixed together. Notice that you have #K_(eq) > 1#, which means that at this given temperature, the forward reaction will be favored, i.e. Moreover, you also know the value of the equilibrium constant, #K_(eq)#, which is said to be equal to #11.2#. The problem provides you with the initial concentrations of hydrogen gas, #"H"_2#, bromine gas, #"Br"_2#, and hydrogen bromide, #"HBr"#. the same rule still applies in terms of ICE tables?īut yes, an ICE table is what you need to use here in order to find the answer. ![]() Equilibrium constant of a reaction is used to predict the direction of the reaction, the extent of a reaction and to calculate the equilibrium concentrations.For a reverse reaction at constant temperature, the value of equilibrium constant is inverse of the equilibrium constant of the forward reaction.A dynamic equilibrium is achieved when the number of molecules remaining in the liquid becomes equal to the number of molecules leaving the liquid to become vapour.At constant temperatures, the values of equilibrium constant remain the same equilibrium constant is temperature sensitive. ![]() The number of atoms of an element should be equal on both sides.
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