The molar heat capacity of silver is 25.35
J/mol⋅
∘
C
. How much energy would it take to raise the temperature of 12.0
g
of silver by 18.6
∘
C
q = mass x heat capacity x delta T
To find the amount of energy required to raise the temperature of a given amount of substance, we 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 molar heat capacity of the substance (in J/mol⋅°C)
- ΔT is the change in temperature (in °C)
In this case, we have:
- m = 12.0 g (mass of silver)
- C = 25.35 J/mol⋅°C (molar heat capacity of silver)
- ΔT = 18.6 °C (change in temperature)
First, let's convert the mass of silver from grams to moles:
- moles of silver = mass / molar mass
The molar mass of silver (Ag) is 107.87 g/mol. Therefore:
- moles of silver = 12.0 g / 107.87 g/mol
Now, we can calculate the energy:
- q = (12.0 g / 107.87 g/mol) * 25.35 J/mol⋅°C * 18.6 °C
By performing this calculation, we find the amount of energy required to raise the temperature of 12.0 g of silver by 18.6 °C.