How much heat is required to raise the temperature of 500 g of water from 25°C t

How much heat is required to raise the temperature of 500 g of water from 25°C to 75°C? (2020)

How much heat is required to raise the temperature of 500 g of water from 25°C to 75°C? (2020)

Step 1: Identify the mass of water. In this case, it is 500 grams.
Step 2: Identify the specific heat capacity of water. It is 4.2 Joules per gram per degree Celsius (J/g°C).
Step 3: Determine the initial temperature of the water, which is 25°C.
Step 4: Determine the final temperature of the water, which is 75°C.
Step 5: Calculate the change in temperature (ΔT) by subtracting the initial temperature from the final temperature: ΔT = 75°C - 25°C = 50°C.
Step 6: Use the formula Q = mcΔT to calculate the heat required. Here, Q is the heat, m is the mass (500 g), c is the specific heat capacity (4.2 J/g°C), and ΔT is the change in temperature (50°C).
Step 7: Plug in the values: Q = 500 g * 4.2 J/g°C * 50°C.
Step 8: Calculate the result: Q = 500 * 4.2 * 50 = 10000 Joules.

Specific Heat Capacity – The amount of heat required to raise the temperature of a unit mass of a substance by one degree Celsius.
Heat Transfer Calculation – Using the formula Q = mcΔT to calculate the heat energy required for temperature changes.
Unit Consistency – Ensuring that all units in the calculation are consistent, particularly mass in grams and temperature in degrees Celsius.