To find the amount of heat needed to raise the temperature of 500g of water from 30°C to 35°C, we can use the formula:
\[ \text{Heat} = \text{mass} \times \text{specific heat capacity} \times \Delta T \]
where:
- mass = 500g
- specific heat capacity of water = 4.2 J/g°C
- \( \Delta T \) (change in temperature) = final temperature - initial temperature
Given:
- initial temperature = 30°C
- final temperature = 35°C
Calculating \( \Delta T \):
\[ \Delta T = 35°C - 30°C = 5°C \]
Now, plug the values into the formula:
\[ \text{Heat} = 500g \times 4.2 J/g°C \times 5°C \]
\[ \text{Heat} = 500g \times 4.2 J/g°C \times 5 \]
\[ \text{Heat} = 500g \times 21 J \]
\[ \text{Heat} = 10500 J \]
Therefore, the amount of heat needed to raise the temperature of 500g of water from 30°C to 35°C is 10500 Joules.
