Answer:
Choice B, C, and D.
Explanation:
Choice A is not true in general. Here's a way to think about that. Consider a very special equilibrium where the concentration of reactants and products are indeed equal. When one of the external factors (such as temperature) changes, the equilibrium will shift towards either side of the reaction. More products will be converted to reactants, or vice versa. Either way, in the new equilibrium, the concentration of the reactants and products will not be equal any more.
Choice B should be considered with choice C and D in mind.
Choice C is indeed correct. The reaction rate would not be zero unless all the reactants were used up or taken out of the system. That's not what happens in an equilibrium. Instead, when reaction rate is plotted against time, the graph for reactions in both directions will eventually flat out at a non-zero value.
Choice D explains why even though choice C is correct, the concentration of a system at equilibrium stays the same. At the equilibrium, reactions in both directions are still happening. However, during the time it takes for the forward reaction use up some reactant particles, the reverse reaction would have produced these particles again. On a large scale, there would be no observable change to the concentration of each species in the equilibrium. Therefore, choice B is also correct.
Answer:
43.7
Explanation:
mole is equal mass concentration/ moler mass of MgCl²
When water molecules align with each other, a weak bond is established between the negatively charged oxygen atom<span> of one water molecule and the positively charged </span>hydrogen atoms<span> of a neighboring water molecule. The weak bond that often forms between </span>hydrogen atoms<span> and neighboring atoms is the hydrogen bond.</span>
