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Komok [63]
3 years ago
6

How much heat is required to warm 1.40 l of water from 20.0 ∘c to 100.0 ∘c? (assume a density of 1.0g/ml for the water.)?

Physics
1 answer:
marta [7]3 years ago
3 0
The water density is 
d=1.0 g/mL = 1000 g/L
And the mass of 1.40 L of water is
m=dV=(1000 g/L)(1.40 L)=1400 g

The amount of heat needed to increase the temperature of the water by \Delta T is given by
Q=m C_s \Delta T
where m is the water mass, C_s = 4.18 J/g ^{\circ}C is the water specific heat capacity and 
\Delta T=100.0 ^{\circ}C-20.0 ^{\circ}C = 80.0^{\circ}C 
is the increase in temperature. If we substitute these numbers into the equation, we find
Q=(1400 g)(4.18 J/g^{\circ}C)(80.0^{\circ}C)=4.68 \cdot 10^5 J
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Let's analyze the force on the chair.

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Let's analyze the forces on the student.

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Learn more here: brainly.com/question/18117041

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