5 public questions tagged with this topic.
Δ U = q + w. Here, q = -500 J (heat released), w = -300 J (work done by system), so Δ U = -500 - 300 = -800 J.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: First Law of Thermodynamics and Enthalpy and Internal Energy
Moles = 39 / 78 = 0.5 mol, heat released = 0.5 × 3267.6 = 1633.8 kJ.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: First Law of Thermodynamics and Enthalpy and Internal Energy
Moles of CH₄ = 8 / 16 = 0.5 mol. Heat released = 0.5 × 890 = 445 kJ.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: First Law of Thermodynamics and Enthalpy and Internal Energy
Moles = 60 / 46 = 1.304 mol, heat released = 1.304 × 1366.7 = 1782.2 kJ.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: First Law of Thermodynamics and Enthalpy and Internal Energy
Moles of C = 12 / 12 = 1 mol. Heat released = 1 × 393.5 = 393.5 kJ.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: Bond Enthalpy and Entropy and Spontaneity
