Question

How much energy must be transferred to raise the temperature of a cup of coffee (250 mL) from 20.5 °C ( 293.7 K) to 95.6 °C ( 368.8 K)? Assume that water and coffee have the same density (1.00 g/ mL), and specific heat capacity ( 4.184 J/ g · K).

Answer 1

To calculate the energy required to raise the temperature of the coffee, use the equation q = m * c * ΔT, where q is the energy transferred, m is the mass of the coffee, c is the specific heat capacity of water, and ΔT is the change in temperature. Apply the equation step-by-step to find the answer.

Step-by-step explanation:

To calculate the amount of energy required to raise the temperature of the coffee, we can use the equation:

q = m * c * ΔT

where q is the energy transferred, m is the mass of the coffee, c is the specific heat capacity of water, and ΔT is the change in temperature. Here's the step-by-step calculation:

1. Convert the volume of the coffee to mass by multiplying it by the density: m = 250 mL * 1.00 g/mL = 250 g
2. Calculate the change in temperature: ΔT = 95.6 °C - 20.5 °C = 75.1 °C
3. Plug the values into the equation: q = 250 g * 4.184 J/g·K * 75.1 °C = 784,670 J

Therefore, the amount of energy required to raise the temperature of the cup of coffee is 784,670 J.