The specific heat of fat is 0.45 cal/(g ⋅ °C) (1.9 J/g °C) and the density of fat is 0.94 g/cm³. How much energy (in calories and joules) is needed to heat 10 cm³ of fat from room temperature (25 °C) to its melting point (35 °C)?

Question

Accepted Answer

Hello everyone today, we have a falling problem. A certain butter has a specific heat of 0.488 calories per gram Celsius and its density is 0.9 11 g per centimeter cubed, calculate the amount of energy in cows and in jewels required to make a 219.5 centimeter cubed block of butter initially at 10 degrees Celsius. The melting point of butter is 40 degrees Celsius. So the first thing we need to do is we need to find the mass in grams. So what we're going to do is we're going to take the energy or the volume of this block of butter, which is 219.5 centim cubed. We're gonna multiply by the density and this density was given to us as 0.911 g per one centimeter cube centimeter cubes cancels out. We're left with 199.96 g. And so now we can find out the heat in calories. So the heat in calories. We're going to take our heat formula which is Q. Or heat is equal to the mass times our specific heat capacity times. To change the temperature. Our mass we found was 199.96 g. Our specific heat capacity was said to be 0.488 calories per grams Celsius. And then our change of temperature, our final temperature was 40°C in which we melted the butter and our initial temperature was 10°C. And this gives us 2.9 times 10 to the third calories. Next we can find the heat in jewels. And so to do that, We're going to use the same formula. The heat is equal to the mass times specific heat capacity times to change the temperature, we have our mass, which is 199.96. We have the specific heat capacity in terms of jewels, which was two point oh four jewels per gram's degrees Celsius. And then of course our final temperature of 40 degrees Celsius minus our initial temperature 10 degrees Celsius, giving us 1.2 times 10 to the fourth jewels. And so with that we have our answer in calories and in jewels. Overall, I hope this helped and until next time.

The specific heat of fat is 0.45 cal/(g ⋅ °C) (1.9 J/g °C) and the density of fat is 0.94 g/cm³. How much energy (in calories and joules) is needed to heat 10 cm³ of fat from room temperature (25 °C) to its melting point (35 °C)?

Verified video answer for a similar problem:

Key Concepts

Specific Heat Capacity

Density

Energy Calculation

The specific heat of fat is 0.45 cal/(g ⋅ °C) (1.9 J/g °C) and the density of fat is 0.94 g/cm3. How much energy (in calories and joules) is needed to heat 10 cm3 of fat from room temperature (25 °C) to its melting point (35 °C)?

Verified video answer for a similar problem:

Key Concepts

Specific Heat Capacity

Density

Energy Calculation

The specific heat of fat is 0.45 cal/(g ⋅ °C) (1.9 J/g °C) and the density of fat is 0.94 g/cm³. How much energy (in calories and joules) is needed to heat 10 cm³ of fat from room temperature (25 °C) to its melting point (35 °C)?