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Chemistry Practical Class 12 Enthalpy of dissolution of copper sulphate or potassium nitrate Viva Questions with Answers

Q1. What is the Enthalpy of Copper Sulphate or Potassium Nitrate Dissolution?

Answer. The molar heat of a solution, also known as the enthalpy of solution, is defined as the amount of heat taken in or emitted while a mole of a solution is dissolved in any solvent, most commonly water. This molar heat is denoted by ΔH and measured in kJ/mol in both popular and academic terms.

Q2. Which Thermodynamic Law governs the entire experiment?

Answer. This experiment follows a well-known thermodynamic law, the law of energy conservation. According to thermodynamics proposed law of conservation of energy, the sum of all enthalpy exchanges must equal zero. As a result, the following equation is used in every heat-related reaction.

ΔH1 + ΔH2 + … + ΔHn = 0

Q3. How to Determine the Type of Reaction Based on the Sign of Enthalpy of Copper Sulphate or Potassium Nitrate Dissolution?

Answer. ΔH is positive if the reaction is exothermic and heat is released during solution formation, and negative if the reaction is endothermic and heat is absorbed.

Q4. What is the weight of copper sulphate in grams?

Answer. Copper sulphate has an equivalent weight of approximately 80 g/mol.

Q5. What is the enthalpy of dissociation?

Answer. The amount of energy required during an endothermic process to break a chemical bond and produce two separated atoms, each with one electron from the first mutual pair, is referred to as the Bond Dissociation Enthalpy.

Q6. What is meant by the term, calorimeter constant?

Answer. A calorimeter constant (abbreviated Ccal) is a constant that quantifies a calorimeter’s heat capacity. It can be calculated by applying a known amount of heat to the calorimeter and measuring the resulting temperature change.

Q7. Why is Δsol H for some substances negative while for others it is positive?

Answer. The total amount of heat absorbed or released when two substances combine to form a solution is referred to as the enthalpy of solutions. This sum can be positive or negative.

Q8. How does Δsol H vary with temperature?

Answer. When the temperature rises, so does the number of molecular interactions. When the number of interactions increases, so does the system’s internal energy.

According to the equation H = U+PV, as temperature rises, the internal energy (U) increases, and so does the h.

C = q/ΔT

Q9. Will the enthalpy change for dissolution of the same amount of anhydrous copper sulphate and hydrated copper sulphate in the same amount of water be the same or different? Explain.

Answer. No, in the case of anhydrous copper sulphate, the enthalpy change will correspond to both the dissolution and hydration processes, resulting in enthalpy of hydration plus enthalpy of solution.

Q10. How will the solubility of copper sulphate and potassium nitrate be affected on increasing the temperature?

Answer. Since the dissolution of copper sulphate and potassium nitrate in water is an endothermic process, the solubility of copper sulphate and potassium nitrate in water will increase with increasing temperature.

Q11. Is the dissolution of hydrated copper sulphate an exothermic or endothermic process?

Answer. The dissolution of hydrated copper sulphate is an Endothermic process.

Q12. What is the difference between an endothermic and an exothermic reaction?

Answer. Endothermic reactions use chemical reaction bonds to attract and store energy. An exothermic reaction sheds heat energy as it progresses, which means it radiates heat while it is happening.

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