A student pours 60.0 mL of 1.50 M nitric acid into 140.0 mL of 0.500 M potassium hydroxide solution in an insulated cup with a lid. Both start at the same temperature, and the mixture warms by 4.54 K. The cup itself takes up 48 J for each kelvin. The solutions have a density of 1.00 g mL⁻¹ and a specific heat of 4.18 J g⁻¹ K⁻¹. What is the size of the enthalpy of neutralisation, in kJ mol⁻¹ of water formed, to the nearest integer?

ChemistryMediumHigh School (11–12)Chemical Thermodynamics › Enthalpy and Hess's Law JEE Main

A student pours $60.0\ \text{mL}$ of $1.50\ \text{M}$ nitric acid into $140.0\ \text{mL}$ of $0.500\ \text{M}$ potassium hydroxide solution in an insulated cup with a lid. Both start at the same temperature, and the mixture warms by $4.54\ \text{K}$ . The cup itself takes up $48\ \text{J}$ for each kelvin. The solutions have a density of $1.00\ \text{g mL}^{-1}$ and a specific heat of $4.18\ \text{J g}^{-1}\ \text{K}^{-1}$ . What is the size of the enthalpy of neutralisation, in $\text{kJ mol}^{-1}$ of water formed, to the nearest integer?

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← Silver oxide decomposes on heating: 2 Ag₂O(s) → 4 Ag(s) + O₂(g). The standard enthalpy of formation of Ag₂O(s) is -31.05 kJ mol⁻¹. The standard molar entropies are Ag(s) 42.55, O₂(g) 205.1 and Ag₂O(s) 121.3 J K⁻¹ mol⁻¹. Taking Δ H° and Δ S° as constant, above what temperature is the decomposition spontaneous under standard conditions?The standard enthalpies of combustion are: ethyne, C₂H₂(g), -1300 kJ mol⁻¹; graphite, -393.5 kJ mol⁻¹; hydrogen, -285.8 kJ mol⁻¹ (the water formed is liquid). What is the standard enthalpy of formation of ethyne, 2 C(graphite) + H₂(g) → C₂H₂(g)? →

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