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Calculate the heat released when 4. 0 x 103 mL of Cl2 (g) with a density of 1. 88 g/L react with an excess of sodium metal at 25°C and 1 atm to form sodium chloride



Answer :

mickymike92

The heat released from the reaction is -87.11 kJ.

What is the mass of the chlorine gas reacting?

The mass of chlorine gas reacting is calculated from the formula below:

  • mass = density * volume

volume of chlorine = 4.0 x 10³ mL or 4 L

density = 1.88 g/L

Mass of chlorine gas = 4 * 1.88 = 7.52 g

The moles of chlorine reacting is:

moles of chlorine reacting = mass / molar mass

moles of chlorine = 7.52 / 71 = 0.106 moles

Equation of reaction: Cl₂ (g) + 2 Na (s) → 2 NaCl (s)

Heat of reaction, ΔHrxn = ΔHproducts - ΔHreactants

ΔHrxn = (2 {ΔHf NaCl}) - ({ΔHf Cl₂} + 2 * {ΔHf Na})

ΔHrxn = (2 * {-410.9 kJ/mol}) - ({0 kJ/mol} + 2 * {0 kJ/mol})

ΔHrxn = -821.8 kJ/mol

Hence;

Heat released = -821.8 kJ/mol * 0.106 moles

Heat released = -87.11 kJ

Learn more about the heat of reaction at: https://brainly.com/question/11631046

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