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The specific heat of glass is 0.840 J/g*°C, the specific heat of water is 4.184 J/g*°C and the specific heat of iron is 0.450 J/g*°C. Identify the correct statement.

Water requires the most energy to increase its temperature followed by glass and then iron.

Water requires the most energy to increase its temperature followed by iron and then glass.

Glass requires the most energy to increase its temperature followed by iron and then water.

Respuesta :

water requires the most energy to increase its temperature followed by glass and then iron

Answer:

Water requires the most energy to increase its temperature followed by glass and then iron.

Step-by-step explanation:

We know that the heat energy is given by:

Q=m×c×Δt where Q represents the heat energy, m represents the mass, c represents the specific heat and Δt represents the change in temperature.

" This means that the energy is directly proportional to specific heat. i.e. more the specific heat more energy will be required to increase the temperature "

Here we are given:

  • The specific heat of glass is 0.840 J/g*°C
  • the specific heat of water is 4.184 J/g*°C
  • and the specific heat of iron is 0.450 J/g*°C.

As water has highest specific heat hence water requires maximum energy followed by glass and then by iron.

Hence, first option is true.

Water requires the most energy to increase its temperature followed by glass and then iron.

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