(A) The fusion process is $H_2O_{(s)} \rightleftharpoons H_2O_{(l)}$.At $1 \ atm$ pressure,the melting point of ice is $273 \ K$.At $T = 273 \ K$,the

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$1 \to r, \ 2 \to p, \ 3 \to q$

(A) The fusion process is $H_2O_{(s)} \rightleftharpoons H_2O_{(l)}$.At $1 \ atm$ pressure,the melting point of ice is $273 \ K$.At $T = 273 \ K$,the system is at equilibrium $(2 \to p)$.For $T > 273 \ K$ (e.g.,$280 \ K$),the process is spontaneous $(1 \to r)$.For $T Therefore,the correct matching is $1 \to r, \ 2 \to p, \ 3 \to q$.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Medium

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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Mix Examples-Thermodynamics and Thermochemistry

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DifficultAIIMS 2000

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Consider the $P-V$ (pressure-volume) diagram given below,where an ideal gas is reversibly converted from state $X$ to state $Y$. Among the following,which is the correct $T-S$ (temperature-entropy) diagram corresponding to this process?

DifficultKVPY 2021

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Following data is known about the melting of a compound $AB$: $\Delta H = 9.2 \ kJ \ mol^{-1}$,$\Delta S = 0.008 \ kJ \ K^{-1} \ mol^{-1}$. Its melting point is:

MediumAIIMS 2000

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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 $(r)$. $280 \ K$

Similar Questions

Enthalpy of neutralisation of acetic acid by $NaOH$ is $-50.6 \ kJ/mol$ and the heat of neutralisation of a strong acid with a strong base is $-55.9 \ kJ/mol$. What is the value of $\Delta H$ for the ionisation of $CH_3COOH$ in $kJ/mol$?

For a certain thermochemical reaction $M \rightarrow N$ at $T = 400 \ K$,$\Delta H^{\ominus} = 77.2 \ kJ \ mol^{-1}$ and $\Delta S = 122 \ J \ K^{-1} \ mol^{-1}$,the value of $\log K$ is $ . . . . . . \times 10^{-1}$.

Consider the $P-V$ (pressure-volume) diagram given below,where an ideal gas is reversibly converted from state $X$ to state $Y$. Among the following,which is the correct $T-S$ (temperature-entropy) diagram corresponding to this process?

Following data is known about the melting of a compound $AB$: $\Delta H = 9.2 \ kJ \ mol^{-1}$,$\Delta S = 0.008 \ kJ \ K^{-1} \ mol^{-1}$. Its melting point is:

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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 $(r)$. $280 \ K$