Ethanol (1) has a specific heat of 2.443/9-°C and mercury's is 0.14 J/g. C. Which substance is the easier one to warm to a higher temperature? Why?

The specific Heat of any material is the heat absorbed or evolved by the material to raise or fall it's temperature by 1°C per unit mass of the material.

The heat absorbed or evolved (Q) is directly proportional to the mass of substance(m) and rise or fall of temp(∆T)

The general formula for specific heat is,

[tex] \sf \: \: \: \: \: s = \frac{Q}{\Delta T} [/tex]

Where s is specific heat,
Q is the Heat absorbed or evolved
& ∆T is change is temp.

Now coming to your question,

The specific heat of ethanol is 2.443 J/g °C

& specific heat of mercury is 0.14 J/g ° C

The definition states that, if the specific heat would be more, more amount of heat will be required for per unit change in temperature and the corresponding substance will be difficult to warm. Similarly, substance with high specific heat won't warm as fast as substance with less specific heat.

Hence mercury will be easier to warm up compared to ethanol, and this could a reason to why Mercury is the only metal liquid at room temperature, because it have less specific heat!

[tex] \small \sf Answer \rightarrow Mercury \: is \: easier \: to \: warm \: to \: a \: high \: temperature.[/tex]

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