Question

Calculate the amount of heat, in Joules, needed to raise 34.0g of water from 55.0°C to 76.0*C. The specific heat of water is 4.18 J/gºC.

Answer 1

The amount of heat needed to raise 34.0g of water from 55.0°C to 76.0°C is 2958.24 Joules.

Step-by-step explanation:

To calculate the amount of heat needed to raise the temperature of water, we can use the formula Q = mcΔT, where Q is the heat, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.

In this case, we are given the mass of water (34.0g), the specific heat of water (4.18 J/gºC), and the change in temperature (76.0°C - 55.0°C = 21.0°C).

Substituting these values into the formula, we have Q = (34.0g)(4.18 J/gºC)(21.0°C) = 2958.24 J.

Therefore, the amount of heat needed to raise 34.0g of water from 55.0°C to 76.0°C is 2958.24 Joules.

Answer 2

2984.52J

Step-by-step explanation:

Using the formula: Q = m × c × ∆T

Where;

Q = amount of heat (in Joules)

m = mass (in grams)

c = specific heat capacity (J/g°C)

∆T = change in temperature (°C)

Based on the information provided in the question;

m = 34.0g

c = 4.18 J/gºC.

Initial temperature = 55.0°C

Final temperature = 76.0°C

Hence, Q = m × c × ∆T

Q = 34 × 4.18 × (76 - 55)

Q = 142.12 × 21

Q = 2984.52J

Therefore, 2984.52J is the amount of heat, in Joules, needed to raise 34.0g of the water.