📚NCERT Questions — CBSE11

Calculate the enthalpy change on freezing of 1.0 mol of water at 10.0°C to ice at -10.0°C. Given: Δ_fus H = 6.03 kJ mol⁻¹ at 0°C, C_p[H₂O(l)] = 75.3 J mol⁻¹ K⁻¹, C_p[H₂O(s)] = 36.8 J mol⁻¹ K⁻¹.

What is lattice enthalpy?

According to IUPAC conventions in chemical thermodynamics, when work is done ON the system, what is the sign of w_ad and its effect on internal energy?

The standard enthalpy change for the decomposition of CaCO₃(s) into CaO(s) and CO₂(g) is +178.3 kJ mol⁻¹. What does this value indicate about the process?

Why does a bare proton (H+) not exist freely in aqueous solutions?

Which of the following statements correctly describes the relationship between bond order, bond enthalpy, and bond length?

The number of angular nodes for any orbital is equal to its:

Which of the following metals reacts with cold water to displace hydrogen?

For a salt to dissolve in a solvent, what must be true about its solvation enthalpy compared to its lattice enthalpy?

For the reaction H₂(g) + ½O₂(g) → H₂O(l), what is the relationship between ΔH and ΔU?