You are observing a reaction and discover that the reaction vessel is warm to the touch. The reaction also results in an increase in entropy. Which statement correctly confirms whether or not the reaction is spontaneous and explains why?

A)The reaction is exothermic (- $\Delta$ H)as demonstrated by the warm reaction vessel and entropy is increased (+ $\Delta$ S). The reaction has a negative $\Delta$ G and is, therefore, spontaneous.
B)The reaction is exothermic (+ $\Delta$ H)as demonstrated by the warm reaction vessel and entropy is increased (+ $\Delta$ S). The reaction therefore has a negative $\Delta$ G and is, therefore, spontaneous.
C)The reaction is exothermic (+ $\Delta$ H)as demonstrated by the warm reaction vessel and entropy is increased (- $\Delta$ S). The reaction has a positive $\Delta$ G and is, therefore, spontaneous.
D)The reaction is endothermic (- $\Delta$ H)as demonstrated by the warm reaction vessel and entropy is increased (- $\Delta$ S). The reaction has a positive $\Delta$ G and is, therefore, spontaneous.