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.
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To calculate the heat released in a chemical reaction, we need to determine the amount of substance involved and the heat of the reaction for the balanced equation.
Step 1: Write the balanced chemical equation for the reaction:
2Na + Cl2 → 2NaCl
Step 2: Determine the stoichiometry of the reaction. From the balanced equation, we see that 1 mole of Cl2 reacts with 2 moles of Na to form 2 moles of NaCl.
Step 3: Convert the given volume into moles. We can use the ideal gas law to do this.
Given:
Volume (V) = 4.260 L
Density (d) = 2.46 g/L
Temperature (T) = 25°C = 298 K
First, let's calculate the mass of Cl2:
Mass of Cl2 = density × volume
Mass of Cl2 = 2.46 g/L × 4.260 L
Mass of Cl2 = 10.4956 g
Next, let's convert the mass of Cl2 to moles:
Molar mass of Cl2 = 2 × atomic mass of Cl
Molar mass of Cl2 = 2 × 35.45 g/mol
Molar mass of Cl2 = 70.90 g/mol
Moles of Cl2 = Mass of Cl2 / Molar mass of Cl2
Moles of Cl2 = 10.4956 g / 70.90 g/mol
Moles of Cl2 ≈ 0.148 mol
Step 4: Calculate the heat released using the molar ratio and the enthalpy of the reaction.
Given:
Enthalpy change (ΔH) = ?? kJ/mol (information not provided)
Unfortunately, the enthalpy change (ΔH) is not given in this case. It is necessary to have the specific value to calculate the heat released accurately.
To calculate the heat released, multiply the moles of Cl2 by the ΔH (enthalpy change):
Heat released = Moles of Cl2 × ΔH
Without the value of ΔH, we cannot determine the heat released in this reaction. Please provide the enthalpy change (ΔH) value for the reaction, and we can continue the calculation.