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 14.6 degrees Celsius?
q = mass x specific heat x delta T
4626.375
To calculate the amount of energy required to raise the temperature of a specific amount of 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 molar heat capacity of the substance (in J/mol*C)
ΔT is the change in temperature (in degrees Celsius)
First, we need to convert the mass of silver from grams to moles using its molar mass. The molar mass of silver (Ag) is 107.87 g/mol.
mass of silver (g) = 12.0 g
molar mass of silver (Ag) = 107.87 g/mol
moles of silver (mol) = mass of silver (g) / molar mass of silver (Ag)
moles of silver (mol) = 12.0 g / 107.87 g/mol
Now, we can calculate the energy required using the given values:
C (molar heat capacity of silver) = 25.35 J/mol*C
ΔT (change in temperature) = 14.6 degrees Celsius
q = m * C * ΔT
q = moles of silver (mol) * C (J/mol*C) * ΔT (C)
Substituting the values:
q = (12.0 g / 107.87 g/mol) * 25.35 J/mol*C * 14.6 C
Now, let's calculate the value:
q = (0.1113 mol) * 25.35 J/mol*C * 14.6 C
q ≈ 43.33 J
Therefore, it would require approximately 43.33 joules of energy to raise the temperature of 12.0 grams of silver by 14.6 degrees Celsius.