A-Calculate the equilibrium concentration of IBr and I2 for the reaction 2 IBr(g) ⇄ I2 (g)...

A-Calculate the equilibrium concentration of IBr and I2 for the reaction 2 IBr(g) ⇄ I2 (g) + Br2 (g) when the initial [IBr] = 1.00 M and the concentrations of the products is initially zero. (KC = 2.50x10-3) [IBr]equilibrium = _______________ [I2]equilibrium =_______________

B- KC = 1.88x10-14 for the reaction CH3NC(g) ⇄ CH3CN(g). If the initial concentrations are [CH3NC] = 0.122 M and [CH3CN] = 0.244 M, what is the equilibrium concentration of CH3CN? [CH3CN] = _______________ M

Expert Solution

In the second part, since the value of KC is very less and hence the reaction barely moves in forward direction. So yhe concentration of the reactants and the products will not change much.

Both of them will have the same concenterations on equilibrium.

queen_honey_blossom answered 2 years ago

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