Match the conditions and the temperature for the 'fusion' process of $H_2O_{(s)}$ at $1 \ atm$ pressure.
Condition Temperature $(1)$. Spontaneous $(p)$. $273 \ K$ $(2)$. At equilibrium $(q)$. $260 \ K$ $(3)$. Non-spontaneous $(r)$. $280 \ K$
| Condition | Temperature |
|---|---|
| $(1)$. Spontaneous | $(p)$. $273 \ K$ |
| $(2)$. At equilibrium | $(q)$. $260 \ K$ |
| $(3)$. Non-spontaneous | $(r)$. $280 \ K$ |
- A$1 \to r, \ 2 \to p, \ 3 \to q$
- B$1 \to q, \ 2 \to p, \ 3 \to r$
- C$1 \to r, \ 2 \to q, \ 3 \to p$
- D$1 \to p, \ 2 \to q, \ 3 \to r$
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The quantity of heat (in $J$) required to raise the temperature of $1.0 \, kg$ of ethanol from $293.45 \, K$ to the boiling point and then change the liquid to vapor at that temperature is closest to
[Given,boiling point of ethanol $351.45 \, K$. Specific heat capacity of liquid ethanol $2.44 \, J \, g^{-1} \, K^{-1}$. Latent heat of vaporisation of ethanol $855 \, J \, g^{-1}$ ]
[Given,boiling point of ethanol $351.45 \, K$. Specific heat capacity of liquid ethanol $2.44 \, J \, g^{-1} \, K^{-1}$. Latent heat of vaporisation of ethanol $855 \, J \, g^{-1}$ ]
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View SolutionMatch the transformations in column $I$ with appropriate options in column $II$.
Column $I$ Column $II$ $A$. $CO_{2(s)} \rightarrow CO_{2(g)}$ $p$. phase transition $B$. $CaCO_{3(s)} \rightarrow CaO_{(s)} + CO_{2(g)}$ $q$. allotropic change $C$. $2H_{(g)} \rightarrow H_{2(g)}$ $r$. $\Delta H$ is positive $D$. $P_{(\text{white, solid})} \rightarrow P_{(\text{red, solid})}$ $s$. $\Delta S$ is positive $t$. $\Delta S$ is negative
| Column $I$ | Column $II$ |
| $A$. $CO_{2(s)} \rightarrow CO_{2(g)}$ | $p$. phase transition |
| $B$. $CaCO_{3(s)} \rightarrow CaO_{(s)} + CO_{2(g)}$ | $q$. allotropic change |
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| $t$. $\Delta S$ is negative |
DifficultIIT 2011
View Solution$A$ sample of gas is compressed from an initial volume of $2V_0$ to $V_0$ using three different processes.
First: Using reversible isothermal.
Second: Using reversible adiabatic.
Third: Using irreversible adiabatic under a constant external pressure.
Then
First: Using reversible isothermal.
Second: Using reversible adiabatic.
Third: Using irreversible adiabatic under a constant external pressure.
Then
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View SolutionFor the reaction $A_{(g)} + 2B_{(g)} \to 2C_{(g)} + 3D_{(g)}$,the value of $\Delta E$ at $27\ ^oC$ is $19.0\ kcal$. The value of $\Delta H$ for the reaction would be.......$kcal$ $(R = 2.0\ cal\ K^{-1} mol^{-1})$
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$NH_2CN_{(s)} + \frac{3}{2}O_{2_{(g)}} \to N_{2_{(g)}} + CO_{2_{(g)}} + H_2O_{(l)}$
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