The molar heat of solution of NaOH is -445.1KJ/mol. In a certain experiment,5g of NaOH is completely dissolved in 1L of H2O at 20°C in foam cup calorimeter. Assuming no heat loss , Tf= 33.2°C, verify?

To verify the temperature change, we can use the equation:

q = m × C × ΔT

where:
q = heat gained or lost by the solution (in J)
m = mass of the solution (in g)
C = specific heat capacity of the solution (in J/g°C)
ΔT = change in temperature (in °C)

First, let's calculate the heat gained or lost by the solution:

q = -445.1 kJ/mol × (5 g / 40.0 g/mol)
q = -55.6375 kJ

Since 1 kJ = 1000 J, we have:

q = -55.6375 kJ × 1000 J/kJ
q = -55637.5 J

Next, let's calculate the specific heat capacity of the solution. Since it is a mixture of water and NaOH, we can assume the specific heat capacity of the solution is the same as that of water, which is 4.18 J/g°C.

Now, we can rearrange the equation to solve for ΔT:

ΔT = q / (m × C)
ΔT = -55637.5 J / (1000 g × 4.18 J/g°C)
ΔT ≈ -13.3 °C

Since the initial temperature is 20°C, the final temperature is:

Tf = 20°C + (-13.3°C)
Tf ≈ 6.7°C

However, the given final temperature is Tf = 33.2°C, which does not match the calculated value. Therefore, there seems to be an error in the calculation or assumption made.