For the reaction, state if the reaction is quantitative, or, if not, state whether products or reactants are favoured at equilibrium.

1. 100 mL of 0.1 mol/L nitric acid reacts with 100 mL of 0.1 mol/L ammonium hydrogen carbonate

My question is how do I know if it is quantitive or not. and if its not how do I know if it is favoured at equilibrium? Can u please help asap...I need to hand this in today.

The equation is the key. Write the equation and balance it.
HNO3 + NH4HCO3 ==> H2CO3 + NH4NO3.

The H2CO3 is not stable and continues as follows:
H2CO3(aq) ==> H2O(l) + CO2(g) so that the overall reaction is

HNO3(aq) + NH4HCO3(s) ==> H2O(l) + CO2(g) + NH4NO3(aq)

A reaction goes to completion if
a. a precipitate is formed.
b. a gas is formed (and escapes;i.e., it isn't in a closed system).
c. a slightly ionized substance is formed.

Does this help?

Thanks!

To determine if the reaction is quantitative or not, you can look at the balanced chemical equation. In this case, the balanced chemical equation for the reaction is:

HNO3(aq) + NH4HCO3(s) -> H2O(l) + CO2(g) + NH4NO3(aq)

Here, the reactants are nitric acid (HNO3) and ammonium hydrogen carbonate (NH4HCO3), and the products are water (H2O), carbon dioxide (CO2), and ammonium nitrate (NH4NO3).

To determine if the reaction is quantitative, you need to consider what happens to the products and reactants at equilibrium. If the reaction is quantitative, it means that it goes to completion, meaning that all of the reactants are consumed and converted into products. In this case, if the reaction is quantitative, it means that all of the nitric acid and ammonium hydrogen carbonate are converted into water, carbon dioxide, and ammonium nitrate.

On the other hand, if the reaction is not quantitative, it means that there is an equilibrium established between the reactants and products. In this case, it means that not all of the reactants are converted into products and there is a mixture of reactants and products present at equilibrium.

To determine if the products or reactants are favored at equilibrium, you need to consider the reaction conditions and the nature of the substances involved. Generally, a reaction is favored towards the products if the products have a lower energy state or are more stable compared to the reactants. In this case, you can look at the nature of the substances involved in the reaction. Water (H2O) and ammonium nitrate (NH4NO3) are both soluble in water, which means they will exist in the aqueous phase and will not form a precipitate. Carbon dioxide (CO2) is a gas, which means it will escape from the reaction system. On the other hand, ammonium hydrogen carbonate (NH4HCO3) is a solid, which means it will remain in the reaction system.

Based on this information, you can conclude that the reaction is not quantitative because not all of the reactants are converted into products. At equilibrium, the products (H2O, CO2, NH4NO3) will be favored over the reactants (NH4HCO3, HNO3), but there will still be a mixture of reactants and products present.