1. The problem statement, all variables and given/known data Use the following Bronsted-Lowry reaction to answer the following question: HMo(aq) + H2O(l) ⇔ H3O+(aq) + Mo–(aq) The best description of this equilibrium is that: A. Products are favoured. B. Reactants are favoured. C. The reaction is quantitative. D. The reaction is non spontaneous. 2. Relevant equations N / A 3. The attempt at a solution The above reaction shows a system at equilibrium, with both forward and reverse reaction occurring at the same rate. If a reverse reaction is occurring, the reaction is not quantitative. Answer C is not correct. Answer D is not correct. Methyl orange indicators are commonly used in laboratories. If the reaction to form a system at equilibrium containing methyl orange were non spontaneous, the indicator simply wouldn't work unless certain conditions such as high temperatures or the use of a catalyst were met. I cannot determine if products or reactants are favoured within the system. I would like to say that because a solution of methyl orange is ideal for testing a range of acidic pH values, the solution of methyl orange itself is acidic. However, this may easily be incorrect. If not, would the solution being acidic indicate that products are favoured? Some acidic solutions favour the formation of reactants: there doesn't seem to be a correlation between the two concepts. How can I go about approaching this question? Please keep your answers restricted to a high school level education, as that is the level of the course I am completing. Thank you, Eric.