To calculate the enthalpy change (螖H) for the reaction, you'll need to use the equation:
q = m 路 C 路 螖T
where:
q is the heat absorbed or released by the reaction,
m is the mass of the solution,
C is the specific heat capacity of the solution, and
螖T is the change in temperature.
First, calculate the heat absorbed or released by the reaction (q) using the equation:
q = m1 路 C1 路 螖T1 + m2 路 C2 路 螖T2
where:
m1 is the mass of the HI solution,
m2 is the mass of the KOH solution,
C1 is the specific heat capacity of the HI solution, and
C2 is the specific heat capacity of the KOH solution.
Given:
m1 = 65.0 g
m2 = 84.0 g
C1 = C2 = 4.184 J/g(掳C)
螖T1 = 螖T2 = (final temperature - initial temperature)
In this case, the initial temperature for both solutions is 18.46 掳C, and the final temperature is 21.96 掳C.
Now you can calculate 螖T1 and 螖T2:
螖T1 = 21.96 掳C - 18.46 掳C = 3.50 掳C
螖T2 = 21.96 掳C - 18.46 掳C = 3.50 掳C
Substituting the values into the equation for q:
q = (65.0 g) 路 (4.184 J/g(掳C)) 路 (3.50 掳C) + (84.0 g) 路 (4.184 J/g(掳C)) 路 (3.50 掳C)
Calculate the value of q, the heat absorbed or released by the reaction.
Next, we need to convert q to moles of HI. First, calculate the number of moles of HI using the given mass and molar mass of HI (127.91 g/mol). The number of moles can be calculated using the equation:
moles of HI = mass of HI / molar mass of HI
Once you have the moles of HI, you can calculate the enthalpy change (螖H) for the reaction using the equation:
螖H = q / moles of HI
Substitute the calculated values into the equation to find the enthalpy change for the reaction.