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Airida [17]
3 years ago
13

The specific heat of ethanol is 2.44 J/g ֯C. How many kJ of energy are required to heat 50.0 grams of ethanol from -20 ֯C to 68

֯C? (heat equation)
Chemistry
1 answer:
Aliun [14]3 years ago
5 0

Answer:

Heat energy required (Q) = 10.736 KJ

Explanation:

Given:

Specific heat of ethanol (C) = 2.44 J/g °C

Mass of ethanol (M) = 50 gram

Initial temperature (T1) = -20°C

Final temperature (T1) = 68°C

Find:

Heat energy required (Q) = ?

Computation:

Change in temperature (ΔT) = 68°C - (-20°C)

Change in temperature (ΔT) = 88°C

Heat energy required (Q) = mC(ΔT)

Heat energy required (Q) = (50)(2.44)(88)

Heat energy required (Q) = 10,736 J

Heat energy required (Q) = 10.736 KJ

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Answer:

\Delta G =-103.95kJ

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Hello there!

In this case, since the thermodynamic definition of the Gibbs free energy for a change process is:

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It is possible to plug in the given H, T and S with consistent units, to obtain the correct G as shown below:

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Answer:

<u>STEP I</u>

This is the balanced equation for the given reaction:-

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____________________________

\\

\mathfrak{\underline{\green{ Why\: KOH \:has\:  been\: taken\: as\: aqueous ?}}}

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[Alkali metal hydroxides are the only halides soluble in water ]

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