the specific heat of aluminum is 0.900 J/g degrees celsius. how much energy is required to heat 45.0g of aluminum from 20.0 degrees celsius to 50.0 degrees celsius.
a. 2840 J
b. 810 J
c. 1220 J
d. 2030 J
love how no 1 answered this lol
q = mass x specific heat x delta T.
To calculate the amount of energy required to heat a substance, you can use the formula:
q = m * c * ΔT
Where:
q is the energy (in joules),
m is the mass of the substance (in grams),
c is the specific heat capacity (in J/g °C),
ΔT is the change in temperature (in °C).
In this case:
m = 45.0 g
c = 0.900 J/g °C
ΔT = 50.0 °C - 20.0 °C = 30.0 °C
Now, substitute these values into the formula:
q = 45.0 g * 0.900 J/g °C * 30.0 °C
q = 1215 J
Therefore, the amount of energy required to heat 45.0 g of aluminum from 20.0 °C to 50.0 °C is 1215 J. However, none of the answer options provided matches this value exactly. The closest option is 1220 J, so the correct answer would be:
c. 1220 J
To find the amount of energy required to heat the aluminum, we need to use the formula:
q = m * c * ΔT
where:
- q represents the energy
- m is the mass of the substance (in grams)
- c is the specific heat capacity of the substance (in J/g°C)
- ΔT is the change in temperature (in °C)
In this case, the mass of aluminum (m) is 45.0 g, the specific heat capacity of aluminum (c) is 0.900 J/g°C, and the change in temperature (ΔT) is 50.0°C - 20.0°C = 30.0°C.
Now, let's plug in the values into the formula:
q = 45.0 g * 0.900 J/g°C * 30.0°C
q ≈ 1215 J
The energy required to heat 45.0 g of aluminum from 20.0°C to 50.0°C is approximately 1215 J.
Since none of the provided answer choices exactly matches 1215 J, the closest option is:
c. 1220 J