Assume that 0.320M of A(g) and 1.20M of B(g) are sealed in a reaction vessel and undergo the reaction shown below: A(g)+3B(g)2C(g) a) Based on the information provided above ONLY, fill in the ICE table below inputting x for any relative changes. Be sure to indicate the direction of change, i.e. +/. Be sure to use the proper number of significant figures. Any zeroes should be denoted as 0 . The equilibrium row should still contain the x variable. b) Determine the value of x, if there is 0.130M of A(g) remaining once the reaction reaches equilibrium. c) Based on parts a) and b), determine the value of the equilibrium constant, Kc, for the reaction