You can mix 100.mL of 1.0 M HCl with 100 mL of 1.0 NaOH, both at 25 degree Celcius. The temperature of your calorimeter rises by 5.98 degree C, and its heat capacity is 100 J/degre C. How much energy is released per mol of H2O formed?
My answer: 6x10^6 J per mol H2O
Ok, you will make .1 mole of H2O
you have 200ml of water heating 5.99C
Heat released=mass*c*deltaTemp
=200*100J/C*5.98C
heat released per mole
= heatreleased/.1 J/mole
Unless I made an error, your answer is wrong.
To calculate the energy released per mole of H2O formed, we need to use the formula:
q = m * C * ΔT
Where:
q is the heat released (in joules),
m is the mass of the solution (in grams),
C is the specific heat capacity of the solution (in joules per gram per degree Celsius), and
ΔT is the change in temperature (in degrees Celsius).
First, let's calculate the mass of the solution. Since we are adding 100 mL of 1.0 M HCl to 100 mL of 1.0 M NaOH, the total volume of the solution is 200 mL. We can convert this to grams using the density of water, which is 1 g/mL.
mass = volume * density = 200 mL * 1 g/mL = 200 g
Next, we use the specific heat capacity of the calorimeter to calculate the heat released. The heat capacity, C, is given as 100 J/°C.
q = mass * C * ΔT = 200 g * 100 J/g°C * 5.98 °C = 119,600 J
Finally, we need to convert the energy released to kilojoules and determine the number of moles of H2O formed. To convert J to kJ, divide by 1000:
q = 119,600 J / 1000 = 119.6 kJ
The balanced equation for the reaction between HCl and NaOH is:
HCl + NaOH → H2O + NaCl
From the balanced equation, we can see that 1 mole of H2O is formed for every 1 mole of HCl.
Therefore, the energy released per mole of H2O formed is equal to the energy released, so:
Energy released per mole of H2O formed = 119.6 kJ
Hence, the correct answer is 119.6 kJ per mole of H2O formed.