Answer :
Answer:
8.0 × 10⁴ J
Explanation:
Step 1: Given data
- Specific heat of water (c): 4,186 J/kg.°C
- Mass of water (m): 1.2 kg
- Initial temperature: 23 °C
- Final temperature: 39 °C
Step 2: Calculate the change in the temperature
ΔT = 39 °C - 23 °C = 16 °C
Step 3: Calculate the heat required (Q)
We will use the following expression.
Q = c × m × ΔT
Q = 4,186 J/kg.°C × 1.2 kg × 16 °C
Q = 8.0 × 10⁴ J
Final answer:
The quantity of heat required to increase the temperature of 1.2 kg of water from 23 °C to 39 °C, given the specific heat of water used (4,186 J/kg∙°C), is approximately 80,467.2 Joules.
Explanation:
The heat required to change a material's temperature can be found using the formula: q = mcΔT, where q is the heat energy, m is the mass of the material, c is the material's specific heat, and ΔT is the change in temperature. Given that the specific heat (c) of water is 4,186 J/kg∙°C, the mass (m) of the water is 1.2 kg, and the temperature change (ΔT) is from 23 °C to 39 °C (a change of 16 °C), we can use the formula to find the required heat.
Substituting the given values into the formula: q = 1.2 kg * 4,186 J/kg∙°C * 16 °C. Calculating this gives an answer of approximately 80,467.2 Joules. Hence, this quantity of heat is required to increase the temperature of the water from 23 °C to 39 °C.
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