$A$ system of $100 \ kg$ mass undergoes a process in which its specific entropy increases from $0.3 \ kJ \ kg^{-1} \ K^{-1}$ to $0.4 \ kJ \ kg^{-1} \ K^{-1}$. At the same time,the entropy of the surrounding decreases from $80 \ kJ \ K^{-1}$ to $75 \ kJ \ K^{-1}$. Find the $(\Delta S)_{universe}$ in $kJ \ K^{-1}$.

  • A
    $0$
  • B
    $5$
  • C
    $10$
  • D
    $15$

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Similar Questions

What will be $\Delta S$ for the reaction: $2A + 3B \to 4C + 5D$ (in $J \ K^{-1}$)?
Given:
$\Delta S_A^o = 100 \ J \ mol^{-1} \ K^{-1}$
$\Delta S_B^o = 120 \ J \ mol^{-1} \ K^{-1}$
$\Delta S_C^o = 200 \ J \ mol^{-1} \ K^{-1}$
$\Delta S_D^o = 150 \ J \ mol^{-1} \ K^{-1}$

For the conversion $C$ (graphite) $\to C$ (diamond),the $\Delta S$ is:

The enthalpy change for the transition of liquid water to steam,$\Delta H_{vap} = 37.3 \ kJ \ mol^{-1}$ at $373 \ K$. The entropy change for the process is......$J \ mol^{-1} K^{-1}$.

For the reaction $MgCO_3(s) \rightarrow MgO(s) + CO_2(g)$,the value of $\Delta S$ is:

The second law of thermodynamics states that in a cyclic process:

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