assuming the reaction goes to completion, determine the final concentration of NH4Cl in the calorimeter.
NH4Cl(s)+ H2O(l)-> NH4Cl(aq)
concentration of NH4Cl is 1.00M
its specific heat is 3.93 and density is g/ml.
note: the exact same question was asked for a previous problem with the equation of:
NH3(aq) +HCl(aq) -> NH4Cl(aq)
So how do I differentiate between the two, what do i do differently?
I recommend you repost as a new question and type the exact question. You've omitted the density from this post and I suspect a number of other essentials.
This post states the concn of NH4Cl solution is 1.00 M
i dokt know
haaalllppppp
To determine the final concentration of NH4Cl in the calorimeter, you need to consider the balanced chemical equation and the stoichiometry of the reaction. In this case, assuming the reaction goes to completion, we can assume that all of the NH4Cl(s) is converted to NH4Cl(aq).
Given that the concentration of NH4Cl is 1.00 M, it means that in 1 liter (1000 ml) of solution, there is 1.00 mole of NH4Cl. However, we need to find the concentration (in M) in the calorimeter.
To differentiate between the two equations (NH3(aq) + HCl(aq) -> NH4Cl(aq) and NH4Cl(s) + H2O(l) -> NH4Cl(aq)), you need to focus on the reactants involved. In this case, you are given that NH4Cl is initially in solid form (NH4Cl(s)) and it reacts with water (H2O(l)) to form NH4Cl in aqueous form (NH4Cl(aq)).
To calculate the final concentration of NH4Cl in the calorimeter, you need to determine the volume of the solution. From the provided information, the density of NH4Cl is given but the volume of the solution is not mentioned. Without the volume of the solution, we cannot determine the final concentration of NH4Cl in the calorimeter.
So, to answer your question, you need to provide the volume of the solution in order to determine the final concentration of NH4Cl.