If 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?
- A$\left(\Delta_{\text{sys}} S^{\theta}\right) + \Delta_{\text{surr}} S^{\theta} = -7692 \ J \ mol^{-1} \ K^{-1}$,the reaction is spontaneous
- B$\left(\Delta_{\text{sys}} S^{\theta}\right) + \Delta_{\text{surr}} S^{\theta} = -5692 \ J \ mol^{-1} \ K^{-1}$,the reaction is non-spontaneous
- C$\left(\Delta_{\text{sys}} S^{\theta}\right) + \Delta_{\text{surr}} S^{\theta} = +5692 \ J \ mol^{-1} \ K^{-1}$,the reaction is spontaneous
- D$\left(\Delta_{\text{sys}} S^{\theta}\right) + \Delta_{\text{surr}} S^{\theta} = +7692 \ J \ mol^{-1} \ K^{-1}$,the reaction is non-spontaneous
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Similar Questions
When $1 \ g$ of $NH_4NO_3$ is decomposed in a bomb calorimeter,the temperature of the calorimeter increases by $6.12 \ K$. If the heat capacity of the system is $1.23 \ kJ/K$,the molar enthalpy of decomposition of $NH_4NO_3$ is ........ $kJ/mol$.
Medium
View SolutionMatch the following terms in Column-$I$ with their corresponding descriptions in Column-$II$:
Column-$I$ Column-$II$ $(a)$ Adiabatic process $(1)$ Heat $(b)$ Isolated system $(2)$ At 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 $(9)$ At constant pressure $(j)$ $\Delta H = q$ $(10)$ Infinitely slow process involving multiple 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 | $(2)$ At 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 | $(9)$ At constant pressure |
| $(j)$ $\Delta H = q$ | $(10)$ Infinitely slow process involving multiple equilibrium states |
| $(k)$ Intensive property | $(11)$ Entropy |
| $(l)$ Extensive property | $(12)$ Pressure,$(13)$ Specific heat |
Medium
View SolutionWhat is the value of $\Delta S_{\text{total}}$ for the following reaction at $300 \ K$:
$Fe_{2}O_{3(s)} + 3CO_{(g)} \longrightarrow 2Fe_{(s)} + 3CO_{2(g)}$
$\Delta H^{\circ} = -25 \ kJ, \Delta S^{\circ} = 15 \ J \ K^{-1}$ (in $J \ K^{-1}$)
$Fe_{2}O_{3(s)} + 3CO_{(g)} \longrightarrow 2Fe_{(s)} + 3CO_{2(g)}$
$\Delta H^{\circ} = -25 \ kJ, \Delta S^{\circ} = 15 \ J \ K^{-1}$ (in $J \ K^{-1}$)
DifficultMHT CET 2020
View SolutionThe enthalpy change on freezing of $1 \ mol$ of water at $5 \ ^\circ C$ to ice at $-5 \ ^\circ C$ is ..... $kJ \ mol^{-1}$.
(Given $\Delta _{fus}H = 6 \ kJ \ mol^{-1}$ at $0 \ ^\circ C$,
$C_p(H_2O, l) = 75.3 \ J \ mol^{-1} \ K^{-1}$,
$C_p(H_2O, s) = 36.8 \ J \ mol^{-1} \ K^{-1}$)
(Given $\Delta _{fus}H = 6 \ kJ \ mol^{-1}$ at $0 \ ^\circ C$,
$C_p(H_2O, l) = 75.3 \ J \ mol^{-1} \ K^{-1}$,
$C_p(H_2O, s) = 36.8 \ J \ mol^{-1} \ K^{-1}$)
DifficultJEE MAIN 2017
View SolutionFor the reaction $2Cl_{(s)} \to Cl_{2(s)}$,the signs of $\Delta H$ and $\Delta S$ respectively are
Medium
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