Question

4. How many J of energy are needed to raise the temperature of 165 g of water from 10.55°C to 47.32°C?

Answer 1

To find out how many Joules of energy are required to raise the temperature of 165 g of water from 10.55°C to 47.32°C, the specific heat capacity of water (4.184 J/g°C) is multiplied by the mass and the temperature change, yielding approximately 25.34 kJ.

Step-by-step explanation:

To calculate how many Joules (J) of energy are needed to raise the temperature of 165 g of water from 10.55°C to 47.32°C, we utilize the formula for heat energy: Q = mcΔT, where Q is the heat energy in Joules, m is the mass of the water in grams, c is the specific heat capacity of water, and ΔT is the change in temperature in degrees Celsius.

The specific heat capacity of water is a constant, 4.184 J/g°C. The mass of the water (m) is given as 165 g, and the change in temperature (ΔT) can be calculated as the final temperature minus the initial temperature, which is 47.32°C - 10.55°C = 36.77°C.

By substituting these values into the formula, we get: Q = (165 g) × (4.184 J/g°C) × (36.77°C) which gives us the total energy required to heat the water under the given conditions.

Thus, the calculation is: Q = 165 × 4.184 × 36.77 = 25337.596 J or approximately 25.34 kJ.

Answer 2

Q = 25360.269 j

Step-by-step explanation:

Given data:

Mass = 165 g

Initial temperature = 10.55 °C

Final temperature = 47.32°C

Energy absorbed = ?

Solution:

Formula:

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

ΔT = T2 - T1

ΔT = 47.32°C - 10.55 °C

ΔT = 36.77 °C

Q = m.c. ΔT

Q = 165 g . 4.18 j/g.°C . 36.77 °C

Q = 25360.269 j