calculate the quantity of energgy required to heat 1.00 mol of aluminum from 25 degrees to its normal melting point of658 degrees
To calculate the quantity of energy required to heat 1.00 mol of aluminum from 25°C to its normal melting point of 658°C, you need to use the equation:
Q = mcΔT
Where:
Q = quantity of heat energy
m = mass of the substance (in this case, 1.00 mol of aluminum)
c = specific heat capacity of the substance (for aluminum, it's 0.897 J/g°C)
ΔT = change in temperature (658°C - 25°C)
First, let's convert the temperature change from Celsius to Kelvin by adding 273.15 to each value:
ΔT = (658 + 273.15) - (25 + 273.15)
ΔT = 931.15 - 298.15
ΔT = 633 K
Now we need to convert the mass of aluminum from moles to grams. The molar mass of aluminum is 26.98 g/mol.
Mass of aluminum = 1.00 mol aluminum × 26.98 g/mol
Mass of aluminum = 26.98 g
Now we have all the values needed to calculate the quantity of energy.
Q = (26.98 g) × (0.897 J/g°C) × (633 K)
Q = 16,447.074 J
Therefore, the quantity of energy required to heat 1.00 mol of aluminum from 25°C to 658°C is approximately 16,447.074 joules.
q1 = mass Al x specific heat Al x (Tfinal-Tinitial).
Tf = 658
Ti = 25