How much energy is needed to raise 20.0g H2O from 10.0oC to 75.0oC. The specific heat of water is 4.18 J/gC.

to get the heat released or absorbed,

Q = mc(T2-T1)
where
m = mass of substance (units in g)
c = specific heat capacity (units in J/g-K)
T2 = final temperature
T1 = initial temperature
*note: units of temp doesn't matter if it's in degree Celsius or Kelvin, as long as T1 and T2 have the same units (since it's difference in temperature or delta,T)
**note: if Q is (-), heat is released and if (+), heat is absorbed

substituting,
Q = (20.0)(4.18)(75-10)
Q = 5434 J

hope this helps~ :)

To calculate the amount of energy needed to raise the temperature of a substance, we use the formula:

q = m * c * ΔT

Where:
q is the amount of energy required
m is the mass of the substance
c is the specific heat capacity of the substance
ΔT is the change in temperature

In this case, we have:
m = 20.0g (mass of water)
c = 4.18 J/g°C (specific heat of water)
ΔT = 75.0°C - 10.0°C = 65.0°C (change in temperature)

Now we can substitute these values into the formula and calculate:

q = 20.0g * 4.18 J/g°C * 65.0°C
q = 5417 J

Therefore, the amount of energy needed to raise 20.0g of water from 10.0°C to 75.0°C is 5417 J.