Calculate the heat released when 4.260 L Cl2 with a density of 2.46 g/L at 25°C reacts with an excess of sodium metal to form solid sodium chloride at 25°C.

Cl2 + 2Na --> 2NaCl

Use density to calculate grams Cl2 used.
Then used heat rxn x (g Cl2 used/molar mass Cl2).
You will need to look up the heat rxn for NaCl from Na and Cl2.

To calculate the heat released during a reaction, you need to use the equation:

q = m * c * ΔT

Where:
q = heat released or absorbed (in joules or calories)
m = mass of the substance (in grams)
c = specific heat capacity of the substance (in J/g·°C or cal/g·°C)
ΔT = change in temperature (in °C)

First, we need to find the mass of chlorine gas (Cl2) that reacts. This can be calculated using the density and volume given:

Density = mass/volume

Rearranging the equation, we get:

Mass = density * volume

Mass = 2.46 g/L * 4.260 L = 10.4696 g

Now that we have the mass of Cl2, we can calculate the heat released. We need the specific heat capacity of chlorine gas, which can be found in reference books or online sources. For simplicity, let's assume the specific heat capacity of Cl2 is 0.479 J/g·°C.

ΔT = final temperature - initial temperature

As both the reactants and products are at the same temperature (25°C), ΔT = 0.

Therefore, the heat released during the reaction is:

q = mass * c * ΔT
q = 10.4696 g * 0.479 J/g·°C * 0
q = 0 Joules (since ΔT = 0)

Thus, no heat is released during this reaction as both reactants and products are at the same temperature.