The specific heat of copper is 0.42J/g°C. How much energy is required to heat a 275g sample of copper from 25.2°C to 75.8°C?

Q = 5844.3 j

Explanation:

Given data:

Specific heat of copper = 0.42 j/g.°C

Mass of sample = 275 g

Initial temperature = 25.2°C

Final temperature = 75.8°C

Energy required = ?

Solution:

Formula:

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

ΔT = 75.8°C - 25.2°C

ΔT = 50.6°C

Q = 275 g × 0.42 j/g.°C ×  50.6°C

Q = 5844.3 j

d: the voltage of the secondary coil is less than that of the primary coil.

im not suree sorry if wrong

the dependant variable is spilled water

the independent is the heat