1.) shifting the reaction equilibrium to the left results in more products being formed fewer products being formed more reactants being used up no change in reactant or product concentration

The correct answer is option B. i.e. fewer products being formed.
Thus, Shifting the reaction equilibrium to the left results in fewer products. In this case, more reactants react among themselves and cause an increase in the concentration of reactants and less production of products. Thus, reactants concentration increases when equlibirum shifts towards left.

Spontaneity tell us the direction of the reaction, but not how fast it goes. gibbs free energy brings together enthalpy, entropy and temperature in one easy formula. g = h - ts. and, finally the sign of delta g is always negative for a spontaneous reaction.