How much energy must be transferred to raise the temperature of a cup of coffee (250 ml) from 20.5∘C to 95.6∘C Assume that water and coffee has same density (1 g/ml) and specific heat capacity 4.148 J/g/k .

c=qmdtq=c×m×dt =4.148×(250)×(95.6−20.5) =1037×75.1=77878.7J

How much energy must be transferred to raise the temperature of a cup of coffee (250 ml) from 20.5∘C to 95.6∘C Assume that water and coffee has same density (1 g/ml) and specific heat capacity 4.148 J/g/k .

c=qmdtq=c×m×dt =4.148×(250)×(95.6−20.5) =1037×75.1=77878.7J

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How much energy must be transferred to raise the temperature of a cup of coffee (250 ml) from ${20.5}^{\circ} C to {95.6}^{\circ} C$ Assume that water and coffee has same density (1 g/ml) and specific heat capacity 4.148 J/g/k .

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7.9 J

790 KJ

77,878.7 J

79 J

answer is B.

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Detailed Solution

$c = \frac{q}{mdt}$

$q = c \times m \times dt$

$\begin{aligned} = 4.148 \times (250) \times (95.6 - 20.5) \end{aligned}$

$\begin{array}{r} = 1037 \times 75.1 = 77878.7 J \end{array}$

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How much energy must be transferred to raise the temperature of a cup of coffee (250 ml) from 20.5∘C to 95.6∘C Assume that water and coffee has same density (1 g/ml) and specific heat capacity 4.148 J/g/k .

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How much energy must be transferred to raise the temperature of a cup of coffee (250 ml) from ${20.5}^{\circ} C to {95.6}^{\circ} C$ Assume that water and coffee has same density (1 g/ml) and specific heat capacity 4.148 J/g/k .