You accidentally drop a book out of the window of a tall building. Assuming
2 answers:
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The change in the player's internal energy is -491.6 kJ. The number of nutritional calories is -117.44 kCal
For this process to take place, some of the basketball player's perspiration must escape from the skin. This is because sweating relies on a physical phenomenon known as the heat of vaporization.
The heat of vaporization refers to the amount of heat required to convert 1g of a liquid into a vapor without causing the liquid's temperature to increase.
From the given information,
- the work done on the basketball is dW = 2.43 × 10⁵ J
The amount of heat loss is represented by dQ.
where;
- dQ = -mL
∴
Using the first law of thermodynamics:b
dU = dQ - dW
dU = -mL - dW
dU = -(0.110 kg × 2.26 × 10⁶ J/kg - 2.43 × 10⁵ J)
dU = -491.6 × 10³ J
dU = -491.6 kJ
The number of nutritional calories the player has converted to work and heat can be determined by using the relation:
dU = -117.44 kcal
Learn more about first law of thermodynamics here:
Answer:
Explanation:
Take at look to the picture I attached you, using Kirchhoff's current law we get:
This is a separable first order differential equation, let's solve it step by step:
Express the equation this way:
integrate both sides, the left side will be integrated from an initial voltage v to a final voltage V, and the right side from an initial time 0 to a final time t:
Evaluating the integrals:
natural logarithm to both sides in order to isolate V:
Where the term RC is called time constant and is given by:
Answer:
Explanation:
The quantity of heat required to raise the temperature of a substance by one degree Celsius is called the specific heat capacity.
Q = Heat absorbed= 16.7 kJ = 16700 J (1kJ=1000J)
m= mass of benzene = 225 g
c = specific heat capacity = 1.74 J/gK
Initial temperature of the water = = 20.0°C = 293 k
Final temperature of the water = = ?
Change in temperature ,
Putting in the values, we get:
The final temperature will be