In an adiabatic coffee cup, a 75mL of 1.0M HCl and 50mL of 1.0M HaOH were neutralize. The initial temperature is 22.1 C and the final temperature is 26.3 C. What is the enthalpy?
S=4.18g/JC and the heat capacity of the adiabatic coffee
To calculate the enthalpy change (ΔH) of the reaction, we can use the formula:
ΔH = q / moles
where q is the heat absorbed or released by the reaction, and moles is the number of moles of the limiting reactant.
First, we need to determine the limiting reactant, which is the one that is completely consumed and determines the amount of heat released or absorbed by the reaction. In this case, HCl and NaOH react in a 1:1 ratio, so we can compare the number of moles of each reactant.
1. Convert the volumes of solutions to moles using the molarity (M) and volume (V) relationship:
moles of HCl = Molarity of HCl x Volume of HCl
= 1.0M x 0.075L
= 0.075 moles
moles of NaOH = Molarity of NaOH x Volume of NaOH
= 1.0M x 0.050L
= 0.050 moles
Based on the stoichiometry, we can see that there are fewer moles of NaOH than HCl, so NaOH is the limiting reactant.
2. Calculate the heat absorbed or released by the reaction (q).
q = mcΔT
where m is the mass of the solution, c is the specific heat capacity, and ΔT is the change in temperature.
Since we know the volume of the solution and the density, we can calculate the mass of the solution:
mass = volume x density
Given the volume of the solution is 125 mL and the density of the solution is not provided, we cannot directly calculate the mass of the solution. So, we need additional information or assumptions about the density or specific heat capacity of the solution.
Without the density, we cannot directly determine the mass and, subsequently, the heat capacity of the adiabatic coffee cup. Therefore, we cannot accurately determine the enthalpy change (ΔH) without this missing information.