Lithium metal is a highly reactive metal that oxidizes instantly in water or air. Given the data below, calculate the energy required to heat 10.0 g of Li from 150.0 °C to 200.0 °C.

Molar heat capacity (solid) = 3.58 J/°C • mol
Molar heat capacity (liquid) = 4.379 J/°C • mol
Melting point = 180.5 °C
Boiling point = 1342 °C
Heat of fusion = 3.00 kJ/mol
Heat of vaporization = 147.1 kJ/mol

The melting point of Li is 180.5.

q1 = heat to raise T of solid from 150 to 181.
q1 = mass Li x specific heat solid Li x (Tfinal-Tinitial). Note: Tf is 181; Ti is 150.

q2 = heat to melt Li at 180.5.
q2 = mass Li x heat fusion.

q3 = heat to raise T of liquid Li from 180.5 to 200.0
q3 = mass Li x specific heat liquid Li x (Tfinal-Tinitial). Note: Tf = 200; Ti = 180.5.

Total Q = q1 + q2 + q3.

To calculate the energy required to heat 10.0 g of Li from 150.0 °C to 200.0 °C, we need to consider the different energy changes that occur during the process.

First, we need to determine if lithium is in a solid or liquid state at the initial and final temperatures given. Since the melting point of lithium is 180.5 °C and the initial temperature is below the melting point (150.0 °C < 180.5 °C), we can assume that lithium is in the solid state at the initial temperature.

Next, we need to calculate the energy required to heat lithium from the initial temperature to its melting point. We can use the molar heat capacity of the solid:

q1 = m * C1 * ΔT1

where:
q1 is the heat transferred
m is the mass of lithium (10.0 g)
C1 is the molar heat capacity of solid lithium (3.58 J/°C • mol)
ΔT1 is the change in temperature (melting point - initial temperature)

Calculating q1:

ΔT1 = 180.5 °C - 150.0 °C = 30.5 °C

q1 = (10.0 g) * (1 mol / 6.941 g) * (3.58 J/°C • mol) * (30.5 °C) = X Joules

Next, we need to calculate the energy required to melt the solid lithium at its melting point. We can use the heat of fusion:

q2 = m * ΔHf

where:
q2 is the heat transferred
m is the mass of lithium (10.0 g)
ΔHf is the heat of fusion of lithium (3.00 kJ/mol)

Calculating q2:

q2 = (10.0 g) * (1 mol / 6.941 g) * (3.00 kJ/mol) * 1000 J/kJ = Y Joules

Next, we need to calculate the energy required to heat the molten lithium from its melting point to the final temperature. We can use the molar heat capacity of the liquid:

q3 = m * C2 * ΔT2

where:
q3 is the heat transferred
m is the mass of lithium (10.0 g)
C2 is the molar heat capacity of liquid lithium (4.379 J/°C • mol)
ΔT2 is the change in temperature (final temperature - melting point)

Calculating q3:

ΔT2 = 200.0 °C - 180.5 °C = 19.5 °C

q3 = (10.0 g) * (1 mol / 6.941 g) * (4.379 J/°C • mol) * (19.5 °C) = Z Joules

Finally, we can calculate the total energy required by summing up the individual energies:

Total energy = q1 + q2 + q3 = X + Y + Z Joules

Note: This calculation assumes the specific heat capacity and the heat of fusion/vaporization remain constant over the given temperature range.