You read a reversible reaction from left to right in the forward direction. This direction shows which of these occurring?

a) the reactants forming a product
b) the product decomposing to form reactants
c) both a and b occurring
d) b occurring, followed by a
e) none of the above

I think the answer is a) but I'm not 100% sure. In this reaction, it is at equilibrium, which also means that both a and b are occurring.

You are correct, A.

You are partially correct. The correct answer is c) both a and b occurring.

When a reversible reaction is at equilibrium, it means that the forward reaction (reactants forming a product) and the reverse reaction (product decomposing to form reactants) are occurring at the same rate. Therefore, both processes are happening concurrently.

To determine the answer to this question, let's first review the concept of a reversible reaction. In a reversible reaction, the reactants can form products, and the products can also reverse back to reform the reactants. This means that both forward and backward reactions are occurring simultaneously.

When you read a reversible reaction from left to right in the forward direction, you are indicating the reaction in which the reactants are forming a product. This means that option a) is correct.

However, it is also important to note that in a reversible reaction at equilibrium, both the forward and backward reactions are occurring at the same rate, resulting in no net change in the concentration of reactants and products. This indicates that option c) is also correct, as both a) and b) are occurring simultaneously.

So, to answer the question accurately, the correct choice is c) both a and b occurring.