Calculate the enthalpy change when $50 \ mL$ of $0.01 \ M$ $Ca(OH)_2$ reacts with $25 \ mL$ of $0.01 \ M$ $HCl$. Given that $\Delta H^o$ for neutralization of a strong acid and a strong base is $-13.7 \ kcal \ mol^{-1}$. (Note: The provided value in the prompt $140 \ kcal \ mol^{-1}$ is physically incorrect for neutralization; using standard value $-13.7 \ kcal \ mol^{-1}$ for calculation). (in $kcal$)
- A$0.003425$
- B$0.00685$
- C$0.3425$
- D$0.0685$
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Similar Questions
Match the following processes with their corresponding entropy changes:
Process Entropy Change $(a)$ Liquid to vapor conversion $(1)$ $\Delta S = 0$ $(b)$ Process not spontaneous at any temperature $(2)$ $\Delta S = (+)$ $(c)$ Reversible expansion of an ideal gas $(3)$ $\Delta S = (-)$
| Process | Entropy Change |
| $(a)$ Liquid to vapor conversion | $(1)$ $\Delta S = 0$ |
| $(b)$ Process not spontaneous at any temperature | $(2)$ $\Delta S = (+)$ |
| $(c)$ Reversible expansion of an ideal gas | $(3)$ $\Delta S = (-)$ |
Medium
View SolutionIf the standard enthalpy change $\left(\Delta_{r} H^{\theta}\right)$ for a certain reaction at $298 \ K$ and constant pressure is $-1860 \ kJ \ mol^{-1}$,and the standard entropy change $\left(\Delta_{\text{sys}} S^{\theta}\right)$ of the same reaction is $-550 \ J \ K^{-1} \ mol^{-1}$,which one of the following statements is correct?
For irreversible expansion of an ideal gas under isothermal condition,the correct option is :
MediumNEET 2021
View SolutionIf $\Delta G$ and $\Delta S$ for the reaction $A_{(g)} \rightarrow B_{(g)} + 2C_{(g)}$ at $2000 \ K$ are $-40 \ kJ \ mol^{-1}$ and $0.22 \ kJ \ K^{-1} \ mol^{-1}$ respectively,the change in internal energy for the same reaction approximately (in $kJ \ mol^{-1}$) is
Match the following columns:
Column $I$ Column $II$ $(a)$ Adiabatic process $(1)$ Heat $(b)$ Isolated system $(2)$ Constant volume $(c)$ Isothermal change $(3)$ First law of thermodynamics $(d)$ Path function $(4)$ No exchange of matter and energy $(e)$ State function $(5)$ No heat exchange $(f)$ $\Delta U = q$ $(6)$ Constant temperature $(g)$ Law of conservation of energy $(7)$ Internal energy $(h)$ Reversible process $(8)$ $p_{ext} = 0$ $(i)$ Free expansion $(9)$ Constant pressure $(j)$ $\Delta H = q$ $(10)$ Infinitely slow process involving equilibrium states $(k)$ Intensive property $(11)$ Entropy $(l)$ Extensive property $(12)$ Pressure $(13)$ Specific heat
| Column $I$ | Column $II$ |
| $(a)$ Adiabatic process | $(1)$ Heat |
| $(b)$ Isolated system | $(2)$ Constant volume |
| $(c)$ Isothermal change | $(3)$ First law of thermodynamics |
| $(d)$ Path function | $(4)$ No exchange of matter and energy |
| $(e)$ State function | $(5)$ No heat exchange |
| $(f)$ $\Delta U = q$ | $(6)$ Constant temperature |
| $(g)$ Law of conservation of energy | $(7)$ Internal energy |
| $(h)$ Reversible process | $(8)$ $p_{ext} = 0$ |
| $(i)$ Free expansion | $(9)$ Constant pressure |
| $(j)$ $\Delta H = q$ | $(10)$ Infinitely slow process involving equilibrium states |
| $(k)$ Intensive property | $(11)$ Entropy |
| $(l)$ Extensive property | $(12)$ Pressure |
| $(13)$ Specific heat |
Medium
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