How much heat (in cal) is necessary to heat 27.0 mL of octane (s= 0.526 cal/g ®C ; d = o.703 g/mL ) from 50.6 ®C to 67.2 ®C?
I understand the Delta T is = 16.6®C
But I don’t know what d stands for (density) or how to apply to the formula.
Use density to convert mL octane to grams octane. mass = volume x density.
Then q = heat needed = mass octane x specific heat octane x delta T.
To calculate the heat required to heat a substance, you can use the formula:
Q = m * s * ΔT
Where:
Q is the heat (in calories),
m is the mass of the substance (in grams),
s is the specific heat capacity of the substance (in cal/g °C), and
ΔT is the change in temperature (in °C).
In this case, you were given the volume of octane instead of its mass. To find the mass, you can use the equation:
m = d * V
Where:
m is the mass (in grams),
d is the density of octane (in g/mL), and
V is the volume of octane (in mL).
Given:
V = 27.0 mL
d = 0.703 g/mL
s = 0.526 cal/g °C
ΔT = 16.6 °C
Now, let's calculate the mass of octane:
m = d * V
m = 0.703 g/mL * 27.0 mL
m = 18.981 g
Now that we have the mass, we can calculate the heat required:
Q = m * s * ΔT
Q = 18.981 g * 0.526 cal/g °C * 16.6 °C
Q ≈ 165.342 cal
Therefore, approximately 165.342 calories of heat is necessary to heat 27.0 mL of octane from 50.6 °C to 67.2 °C.
To calculate the amount of heat necessary to heat a substance, you need to use the formula:
q = m * s * ΔT
In this formula:
- q represents the amount of heat energy required (in calories).
- m represents the mass of the substance (in grams).
- s represents the specific heat capacity of the substance (in cal/g · °C).
- ΔT represents the change in temperature (in °C).
In this case, you are given the specific heat capacity (s) and the change in temperature (ΔT), but you need to find the mass (m) of the octane.
To determine the mass (m), you can use the density (d) of the octane, which is given as 0.703 g/mL. The volume (V) of the octane is also given as 27.0 mL.
To find the mass, you can use the formula:
m = d * V
Let's substitute these values into the formula:
m = 0.703 g/mL * 27.0 mL
m = 18.981 g
Now that you have the mass (m) of the octane, you can proceed with calculating the amount of heat (q) required using the specific heat capacity (s) and the change in temperature (ΔT).
q = m * s * ΔT
q = 18.981 g * 0.526 cal/g · °C * 16.6 °C
q ≈ 169.62 cal
Therefore, approximately 169.62 calories of heat energy are necessary to heat 27.0 mL of octane from 50.6 °C to 67.2 °C.