The specific heat of zinc is 0.096 cal/(g °C). Determine the energy required to raise the temperature of 26.1 g of zinc from room temperature (20.0 °C) to 150 °C.
(Sp Heat)(Change in Temp)(Mass)=
To determine the energy required to raise the temperature of zinc from 20.0 °C to 150 °C, we need to use the specific heat formula:
q = m * c * ΔT
Where:
q = energy (in calories)
m = mass of the substance (in grams)
c = specific heat (in cal/(g °C))
ΔT = change in temperature (in °C)
Given:
m = 26.1 g
c = 0.096 cal/(g °C)
ΔT = 150 °C - 20.0 °C = 130 °C
Plugging the values into the formula:
q = 26.1 g * 0.096 cal/(g °C) * 130 °C
Simplifying:
q = 320.376 cal
Therefore, it would require 320.376 calories of energy to raise the temperature of 26.1 g of zinc from 20.0 °C to 150 °C.
To determine the energy required to raise the temperature of zinc, we can use the formula:
Q = mcΔT,
where Q is the energy change or heat, m is the mass of the substance, c is the specific heat, and ΔT is the change in temperature.
In this case, we are given:
- The mass of zinc (m) = 26.1 g,
- The specific heat of zinc (c) = 0.096 cal/(g °C),
- The initial temperature (T1) = 20.0 °C, and
- The final temperature (T2) = 150 °C.
First, let's calculate the change in temperature:
ΔT = T2 - T1
ΔT = 150 °C - 20.0 °C
ΔT = 130.0 °C
Now, we can calculate the heat energy needed:
Q = mcΔT
Q = (26.1 g)(0.096 cal/(g °C))(130.0 °C)
To find the answer, we'll perform the calculation:
Q = (26.1 g)(0.096 cal/(g °C))(130.0 °C)
Q ≈ 327.888 cal
Therefore, it would require approximately 327.888 calories of energy to raise the temperature of 26.1 grams of zinc from 20.0 °C to 150 °C.