A calorimeter contains 16.0 of water at 15.0. When 1.60 of (a substance with a molar mass of 58.0 ) is added, it dissolves via the reaction



and the temperature of the solution increases to 27.5.
Calculate the enthalpy change, , for this reaction per mole of .

Assume that the specific heat and density of the resulting solution are equal to those of water [4.18 and 1.00 ] and that no heat is lost to the calorimeter itself, nor to the surroundings.

1. You need to learn how to spell chemistry.

2. You need to redo this post. 16.0 what of water. 15.0 what T. 1.60 what of substance. No reaction is given.

To calculate the enthalpy change (∆H) for this reaction per mole of HCl, you can use the equation:

∆H = q / n

Where:
∆H is the enthalpy change
q is the heat absorbed or released by the reaction
n is the number of moles of HCl

First, calculate the heat absorbed or released by the reaction using the equation:

q = mc∆T

Where:
m is the mass of water in the calorimeter (16.0 g)
c is the specific heat capacity of water (4.18 J/g°C)
∆T is the change in temperature of the solution (27.5°C - 15.0°C)

Substituting the values into the equation:

q = 16.0 g × 4.18 J/g°C × (27.5°C - 15.0°C)

Calculate the value of q.

Next, calculate the number of moles of HCl using its mass and molar mass:

n = m / M

Where:
m is the mass of HCl (1.60 g)
M is the molar mass of HCl (58.0 g/mol)

Substituting the values into the equation:

n = 1.60 g / 58.0 g/mol

Calculate the value of n.

Finally, substitute the calculated values of q and n into the equation for ∆H:

∆H = q / n

Calculate the value of ∆H.

Now you have calculated the enthalpy change (∆H) for this reaction per mole of HCl.