How much heat is needed to increase the temperature of 100.00g of water by 1.0 degree celsius? By 10.0 degrees celsius? By 20.0 degrees celsius?
q = mass water x specific heat water x delta T.
To calculate the heat needed to increase the temperature of a substance, we use the specific heat capacity formula:
q = m * c * ΔT
Where:
q = heat (in Joules)
m = mass of the substance (in grams)
c = specific heat capacity of the substance (in J/g°C)
ΔT = change in temperature (in °C)
In the case of water, the specific heat capacity (c) is 4.18 J/g°C. So, let's substitute the given values into the formula for each question:
1. To increase the temperature of 100.00g of water by 1.0 °C:
q = 100.00g * 4.18 J/g°C * 1.0 °C
q = 418.0 Joules
Therefore, 418.0 Joules of heat are needed.
2. To increase the temperature of 100.00g of water by 10.0 °C:
q = 100.00g * 4.18 J/g°C * 10.0 °C
q = 4180 Joules
Therefore, 4180 Joules of heat are needed.
3. To increase the temperature of 100.00g of water by 20.0 °C:
q = 100.00g * 4.18 J/g°C * 20.0 °C
q = 8360 Joules
Therefore, 8360 Joules of heat are needed.