Calculate the amount of heat required to raise the tempera- ture of 250.0 g (approximately 1 cup) of hot chocolate from 25.0 °C to 80.0 °C. Assume hot chocolate has the same spe-cific heat as water 34.18 J>1g °C24.

Video transcript

Hello everyone today. We have the following question determine the energy needed to heat 400 ml of coffee from 30°C to 90°C. Use the density and specific heat of water. So first we're going to recall what the density Of H 20. Or water is. That's going to be one g per mil a leader. And this is going to be found in a reference text. And the specific heat of our water is going to be 4.18 jules per gram Celsius. And so with this we can now solve for our heat heat energy. So solve for heat energy. That's going to be equal to Q. Or our heat equal to. We're gonna use our density From our 400 ml. We're going to multiply that by our density of water which is which is going to be equal to our one g per one miller leader. That's how we're gonna get our grams are mass. They're gonna multiply by our specific heat capacity which is 4. Jules per gC. And they were going to multiply by our change in our temperature which is going from 90°C to 30°C. It wasn't mentioned earlier but our formula for specific heat capacity is our mass times our specific heat capacity times the change in our temperature. And that is how we derive the following equation. We are then going to get 100,320 jewels. However, we need to determine the energy in terms of killer jewels. So we can simply just multiply this by the conversion factor that one kill a jewel is equal to 10 to the third jewels are units of joules will cancel up. That will be left with a final answer of 100. kg joules of energy needed to heat that amount of coffee from 30 degrees Celsius to 90 degrees Celsius Overall, I hope that this helped, and until next time.