Molar enthalpy change for melting of ice is 6 kJ / mol. Then the internal energy change (in k J / mol ) when 1 mole of water is converted into ice at 1 atm at 0° C is Empty QImg

Question

Molar enthalpy change for melting of ice is 6 kJ / mol. Then the internal energy change (in k J / mol ) when 1 mole of water is converted into ice at 1 atm at 0° C is Empty QImg (A) RT/1000 (B) 6 (C) 6-(RT/1000) (D) 6+(RT/1000)

Tardigrade Admin · Accepted Answer

Given, Δ H=6 kJ / mol Δ U=? H2 O(l) Ice(s) ∵ Δ H=Δ U+Δ ng R T Here, Δ ng=0 ∴ Δ H=Δ U ⇒ Δ U=6 kJ / mol

Q. Molar enthalpy change for melting of ice is $6 k J / m o l$ . Then the internal energy change (in $k J / m o l$ ) when $1$ mole of water is converted into ice at $1$ atm at $0^{\circ} C$ is Empty QImg

RT/1000

6

6-(RT/1000)

6+(RT/1000)

Given, $Δ H = 6 k J / m o l$
$Δ U = ?$
$H_{2} O (l) I ce (s)$
$∵ Δ H = Δ U + Δ n_{g} RT$
Here, $Δ n_{g} = 0$
$∴ Δ H = Δ U$
$\Rightarrow Δ U = 6 k J / m o l$

Q. Molar enthalpy change for melting of ice is 6kJ/mol. Then the internal energy change (in kJ/mol ) when 1 mole of water is converted into ice at 1 atm at 0∘C is Empty QImg

RT/1000

6

6-(RT/1000)

6+(RT/1000)

Given, ΔH=6kJ/mol ΔU=? H2​O(l)Ice(s) ∵ΔH=ΔU+Δng​RT Here, Δng​=0 ∴ΔH=ΔU ⇒ΔU=6kJ/mol

Q. Molar enthalpy change for melting of ice is $6 k J / m o l$ . Then the internal energy change (in $k J / m o l$ ) when $1$ mole of water is converted into ice at $1$ atm at $0^{\circ} C$ is Empty QImg

Given, $Δ H = 6 k J / m o l$
$Δ U = ?$
$H_{2} O (l) I ce (s)$
$∵ Δ H = Δ U + Δ n_{g} RT$
Here, $Δ n_{g} = 0$
$∴ Δ H = Δ U$
$\Rightarrow Δ U = 6 k J / m o l$