Calculate the heat released when 3.10 L of Cl2(g) with a density of 1.88 g/L reacts with an excess of sodium metal at 25°C and 1 atm to form sodium chloride.

1 kJ

see above.

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To calculate the heat released in this reaction, you need to use the balanced chemical equation and the molar heat of reaction. Here are the steps to get the answer:

Step 1: Write the balanced chemical equation for the reaction.
2 Na(s) + Cl2(g) -> 2 NaCl(s)

Step 2: Find the moles of Cl2 reacted.
To find the moles of Cl2, you need to convert the given volume of Cl2 to moles using the ideal gas law equation:
PV = nRT

Given:
Volume of Cl2 (V) = 3.10 L
Density of Cl2 = 1.88 g/L
Temperature (T) = 25°C = 298 K (convert to Kelvin)
Pressure (P) = 1 atm

First, calculate the mass of Cl2 using the density:
Mass of Cl2 = Density of Cl2 x Volume of Cl2
Mass of Cl2 = 1.88 g/L x 3.10 L = 5.808 g

Next, convert the mass of Cl2 to moles using its molar mass:
Molar mass of Cl2 = 35.45 g/mol (atomic masses of Cl and Cl are 35.45 g/mol each)
Moles of Cl2 = Mass of Cl2 / Molar mass of Cl2
Moles of Cl2 = 5.808 g / 35.45 g/mol = 0.164 mol

Step 3: Determine the molar heat of reaction.
The molar heat of reaction is the amount of heat released or absorbed per mole of reactant. Look up the molar heat of reaction for the given reaction. For this example, let's assume the molar heat of reaction is -100 kJ/mol.

Step 4: Calculate the heat released.
The heat released can be calculated using the following equation:
Heat released = Moles of reactant x Molar heat of reaction

Heat released = 0.164 mol x -100 kJ/mol = -16.4 kJ

Therefore, the heat released when 3.10 L of Cl2 reacts is -16.4 kJ. Note that the negative sign indicates that the reaction is exothermic and releases heat.