Answer:
2730.304 KJ
Explanation:
How much heat is required to convert 0.8 kg of ice at -35°C into steam at 100 C?
Given that:
mass of ice (m) = 0.8 kg = 800 g
Initial temperature () = -35°C = 238 K
final temperature ()= 100°C = 373 K
Specific heat of ice () = 2.108 J/g.K
Specific heat of water () = 4.18 J/g.K
Latent heat of fusion () = 334 J/g.
Latent heat of vaporization () = 2230 J/g.
Total heat (Q) required to increase the temperature of ice from the initial temperature of 238K to final temperature of 373 K is given by the equation:
The area of a square is given by:
A = s²
A is the square's area
s is the length of one of the square's sides
Let us take the derivative of both sides of the equation with respect to time t in order to determine a formula for finding the rate of change of the square's area over time:
d[A]/dt = d[s²]/dt
The chain rule says to take the derivative of s² with respect to s then multiply the result by ds/dt
dA/dt = 2s(ds/dt)
A) Given values:
s = 14m
ds/dt = 3m/s
Plug in these values and solve for dA/dt:
dA/dt = 2(14)(3)
dA/dt = 84m²/s
B) Given values:
s = 25m
ds/dt = 3m/s
Plug in these values and solve for dA/dt:
dA/dt = 2(25)(3)
dA/dt = 150m²/s
Answer:
The correct option is B
Explanation:
Although, it is common knowledge that in an electric field, unlike charges attract and like charges repel. However, to build up an electric potential, a positive charge is brought close to another positive charge - this causes work done to be changed to electric potential energy and stored in the electric field.
It should however be noted that when a negative charge is moved away from a positive charge, the negative charge gains electric potential energy.
Find the screenshots in the attachment for complete solution. Follow the sequence