When 2.0 g of solid NaOH (∆Hsoln = -445.1kJ/mol) dissolves in 10L of water, how much heat is released?
445.1 kJ
44.51 kJ
22.26 kJ
11.13 kJ***
No. Show your work and I'll find the error.
22.25
To find the amount of heat released when 2.0 g of solid NaOH dissolves in 10L of water, we need to use the given enthalpy of solution (∆Hsoln) for NaOH.
First, we need to determine the number of moles of NaOH by dividing the given mass (2.0 g) by the molar mass of NaOH. The molar mass of NaOH is calculated by adding the atomic masses of its constituent elements: sodium (Na) with a molar mass of 22.99 g/mol, oxygen (O) with a molar mass of 16.00 g/mol, and hydrogen (H) with a molar mass of 1.01 g/mol.
The molar mass of NaOH = 22.99 g/mol + 16.00 g/mol + 1.01 g/mol = 40.00 g/mol
Now we can calculate the number of moles of NaOH:
Number of moles = mass / molar mass = 2.0 g / 40.00 g/mol = 0.05 mol
The enthalpy change (∆H) for the given amount of NaOH is given as -445.1 kJ/mol. To find the total heat released, we can multiply the number of moles by the enthalpy change (∆H).
Total heat released = number of moles × ∆H = 0.05 mol × -445.1 kJ/mol
Multiplying these values will give us the answer:
Total heat released = -22.255 kJ ≈ -22.26 kJ
Therefore, the correct answer is 22.26 kJ, which indicates that 11.13 kJ is not the correct answer.