SATHEE: Chemical Thermodynamics Question 399

Chemical Thermodynamics Question 399

Question: $Δ H_{f}^{0}$ of water is $- 285.8 k J m o l^{- 1}$ . If enthalpy of neutralisation of monoacidic strong base is $- 57.3 k J m o l^{- 1}$ . $Δ H_{f}^{0}$ of $O H^{-}$ ion will be

Options:

A) $- 114.25 k J, m o l^{- 1}$

B) $114.25 k J m o l^{- 1}$

C) $228.5 k J, m o l^{- 1}$

D) $- 228.5 k J m o l^{- 1}$

Show Answer

Answer:

Correct Answer: D

Solution:

$H_{2} (g) + \frac{1}{2} O_{2} (g) \overset{}{\to} H_{2} O (l);$

$Δ H = - 285.8 k J$ …. (i) $H^{+} (a q) + O H^{-} (a q) \overset{}{\to} H_{2} O (l);$

$Δ H = - 57.3 k J$ …. (ii) $\frac{1}{2} H_{2} (g) + a q \overset{}{\to} H^{+} {(a q)}^{+} e^{-}; Δ H = 0$ (by convention) …. (iii) (ii) - (iii) gives, $\frac{1}{2} H_{2} (g) + \frac{1}{2} O_{2} (g) + e^{-} + a q \overset{}{\to} O H^{-} (a q)$

$Δ H = - 285.8 + 57.3 = - 228.5 k J$

Chemical Thermodynamics Question 399

Question: $Δ H_{f}^{0}$ of water is $- 285.8 k J m o l^{- 1}$ . If enthalpy of neutralisation of monoacidic strong base is $- 57.3 k J m o l^{- 1}$ . $Δ H_{f}^{0}$ of $O H^{-}$ ion will be

Options:

Answer:

Solution:

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Chemical Thermodynamics Question 399

Question: ΔHf0 of water is −285.8kJmol−1 . If enthalpy of neutralisation of monoacidic strong base is −57.3kJmol−1 . ΔHf0 of OH− ion will be

Options:

Answer:

Solution:

Engineering Preparation

Medical Preparation

NCERT Books & Solutions

Important Resources

Other Resources

Syllabus

Test Platform

Sample Mock Test

Mentorship

NCERT Exercise Video Solution

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Question: $Δ H_{f}^{0}$ of water is $- 285.8 k J m o l^{- 1}$ . If enthalpy of neutralisation of monoacidic strong base is $- 57.3 k J m o l^{- 1}$ . $Δ H_{f}^{0}$ of $O H^{-}$ ion will be