200 mL of 0.2 M HCl is mixed with 300 mL of 0.1 M NaOH. The molar heat of neutralization of this reaction is $$-$$57.1 kJ. The increase in temperature in $$^\circ$$C of the system on mixing is x $$\times$$ 10$$-$$2. The value of x is ___________. (Nearest integer)
[Given : Specific heat of water = 4.18 J g$$-$$1 K$$-$$1, Density of water = 1.00 g cm$$-$$3]
[Assume no volume change on mixing)
Your Input ________
Answer
Correct Answer is 82
Explanation
$$\Rightarrow$$ Millimoles of HCl = 200 $$\times$$ 0.2 = 40
$$\Rightarrow$$ Millimoles of NaOH = 300 $$\times$$ 0.1 = 30
For water $$\Delta$$vap H = 41 kJ mol$$-$$1 at 373 K and 1 bar pressure. Assuming that water vapour is an ideal gas that occupies a much larger volume than liquid water, the internal energy change during evaporation of water is ___________ kJ mol$$-$$1