Answer:
Explanation:
Molal freezing point depression constant of butanol Kf = 8.37⁰C /m
ΔTf = Kf x m , m is no of moles of solute per kg of solvent .
mol weight of butanol = 70 g
235.1 g of butanol = 235.1 / 70 = 3.3585 moles
3.3585 moles of butanol dissolved in 4.14 kg of water .
ΔTf = 8.37 x 3.3585 / 4.14
= 6.79⁰C
Depression in freezing point = 6.79
freezing point of solution = - 6.79⁰C .
2Mg+O₂⇒2MgO
It can be a combustion reaction, or it can be a combination reaction
Answer: -64.1 kJ.
Explanation:
According to first law of thermodynamics:
=Change in internal energy
q = heat absorbed or released
w = work done or by the system
w = work done by the system=
{Work is done by the system is negative as the final volume is greater than initial volume}
w = -855 Joules = 0.855 kJ (1kJ=1000J)
q = -65.0 kJ {Heat released by the system is negative}

Thus the change internal energy (ΔE) for a system that is giving off 65.0 kJ of heat and is performing 855 J of work on the surroundings is -64.1 kJ.
I would say D would be the answer