Home
Class 11
CHEMISTRY
Calculate the entropy change in surround...

Calculate the entropy change in surroundings when `1.00` mol of `H_(2)O(l)` is formed under standard conditions, `Delta_(r )H^(Θ) = -286 kJ mol^(-1)`.

Text Solution

Verified by Experts

The standard enthalpy of formation of water at 298 K = `-286 kJ "mol"^(-1)`
The reaction is exothermic so heat gained by surroundings, `DeltaH_(surr) = 286.0 kJ "mol"^(-1)`
`DeltaS_(sur) = (286.0 xx 10^(3)J "mol"^(-1))/(298 K) `
` = 959.73J K^(-1)`
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    MODERN PUBLICATION|Exercise Practice Problems|65 Videos

  • THERMODYNAMICS

    MODERN PUBLICATION|Exercise Advanced Level Problems|15 Videos

  • STRUCTURE OF ATOM

    MODERN PUBLICATION|Exercise Unit Practice Test|13 Videos

Similar Questions

Explore conceptually related problems

Calculate the entropy change for vaporization of 1mol of liquid water to stem at 100^(@)C , if Delta_(V)H = 40.8 kJ mol^(-1) .

Calculate the entropy change of n-hexane when 1 mole of it evaporates at 341.7 K (Delta_(vap) H = 29.0 kJ "mol"^(-1)) .

Calculate the entropy change of n -hexae when 1mol of it evaporates at 341.7K (Delta_(vap)H^(Theta) = 290.0 kJ mol^(-1))

The dissolution of 1 mol e of NaOH_((s)) in 100 mol e of H_(2)O_((l)) give rise to evolution of heat equal to -42.34kJ . However if 1 mol e of NaOH_((s)) is dissolved in 1000 mol e of H_(2)O_((l)) , the heat given out is 42.76kJ . What would be enthalpy change when 900 mole of H_(2)O_((l)) are added to a solution containing 1 mole of NaOH_((s)) in 100 mole of H_(2)O ?