1988-6-b-ii-td
Criterion of a chemical equilibrium is that the total Gibbs free energy change is:
1997-1-21-td The equilibrium constant \(K\) for a chemical reaction depends on
1997-1-22-td The decomposition of \(A\) into \(B\) is represented by the exothermic reaction \( A \rightleftharpoons B\). To achieve maximum decomposition, it is desirable to carry out the reaction
2002-1-9-td
The extent of reaction is
2004-7-td
For an ideal gas mixture undergoing a reversible gaseous phase chemical reaction, the equilibrium constant
2006-32-td For a reversible exothermic gas phase reaction, \(A+B\rightleftharpoons C\), the equilibrium conversion will increase with
2012-9-td For an exothermic reversible reaction, which one of the following correctly describes the dependence of the equilibrium constant (\(K\)) with temperature (\(T\)) and pressure (\(P\))?
2014-7-td Match the following:
Group 1
Group 2
P.
\(\displaystyle \left (\frac {\partial G}{\partial n_i} \right )_{T,P,n_{j\ne i}} \)
I
Arrhenius equation
Q.
\(\displaystyle \left (\frac {\partial G}{\partial n_i} \right )_{S,V,n_{j\ne i}} \)
II.
Reaction equilibrium constant
R.
\(\displaystyle \exp \left (\frac {-\Delta G^\circ _{\text {reaction}}}{RT} \right ) \)
III.
Chemical potential
S.
\(\displaystyle \sum (n_i d\mu _i)_{T,P = 0}\)
IV.
Gibbs-Duhem equation
MT-2007-66-td Enthalpy of formation at 298 K, \(\Delta H_f^\circ \) of CO2 and PbO are -393 kJ/mol and -220 kJ/mol, respectively. The enthalpy change for the reaction 2PbO + C \(\rightarrow \) 2Pb + CO2 is
2013-5-td A gaseous system contains H2, I2, and HI, which participate in the gas-phase reaction: \( 2\text{HI} \rightleftharpoons \text{H$_2$} + \text{I$_2$}\). At a state of reaction equilibrium, the number of thermodynamic degrees
of freedom is ____________
1997-25-td Ethanol is manufactured by the vapor phase hydration of ethylene according to the reaction: \[ \ce {C2H4(g)} + \ce {H2O(g)} \rightleftharpoons \ce {C2H5OH(g)} \] The reactor operates at 400 K and 2 bar and the feed is a gas mixture of ethylene and steam
in the mole ratio 1:3. The equilibrium constant is 0.25. Estimate the composition (mol%) of the equilibrium mixture. (ii) % of \(\ce {C2H4}\)
Assume ideal gas behaviour and take \(f_i^\circ \) = 1 bar, where \(f_i^\circ \) is the standard state fugacity of component \(i\).
(i) % of \(\ce {C2H5OH}\)
{#1}
{#2}
1998-23-td The reaction \(\ce {N2} + \ce {O2} \rightleftharpoons 2\ce {NO}\) takes place in the gas phase at 2700\(^\circ \)C and 2025 kPa. The reaction mixture initially comprises 15 mole% oxygen, 77 mole% nitrogen and the rest inerts. The standard Gibb’s free
energy change for the reaction is 113.83 kJ/mol at this temperature. Assuming ideal gas behaviour, calculate the composition (in %) of all species at equilibrium. (ii) \(\ce {O2}\) (iii) \(\ce {NO}\) (iv) inerts
(i) \(\ce {N2}\)
{#1}
{#2}
{#3}
{#4}
1996-2-10-td Given \[ 3\ce {H2} + \ce {CO} = \ce {CH4} + \ce {H2O} \quad K_p = 10^{1.84} \] and \[ 4\ce {H2} + \ce {CO2} = \ce {CH4} + 2\ce {H2O} \quad K_p = 10^{1.17} \] the \(K_p\) for the reaction \[ \ce {CO} + \ce {H2O} = \ce {CO2} + \ce {H2} \] is
2000-2-06-td At a given temperature, \(K_1, K_2\) and \(K_3\) are the equilibrium constants for the following reaction 1, 2, 3 respectively: \( \begin{align*} \text{CH$_4$(g)} + \text{H$_2$O(g)} &\rightleftharpoons \text{CO(g)} + 3 \text{H$_2$(g)} & (1) \\ \text{CO(g)} + \text{H$_2$O(g)} &\rightleftharpoons \text{CO$_2$(g)} + \text{H$_2$(g)} & (2) \\ \text{CH$_4$(g)} + 2\text{H$_2$O(g)}
&\rightleftharpoons \text{CO$_2$(g)} + 4 \text{H$_2$(g)} & (3) \end{align*} \) Then \(K_1, K_2\) and \(K_3\) are related as
2007-34-td Vapor phase hydration of C2H4 to ethanol by the following reaction \[ \text {C}_2\text {H}_4\text {(g)} + \text {H}_2\text {O}\text {(g)} \rightleftharpoons \text {C}_2\text {H}_5\text {OH} \text {(g)} \] attains equilibrium at 400
K and 3 bar. The standard Gibbs free energy change of reaction at these conditions is \(\Delta G^\circ =4000\) J/mol. For 2 moles of an equimolar feed of ethylene and steam, the equation in terms of the extent of reaction \(\varepsilon \) (in mols)
at equilibrium is
2008-36-td The standard Gibbs free energy change and enthalpy change at 25oC for the liquid phase reaction \[ \text {CH}_3\text {COOH}\text {(l)} + \text {C}_2\text {H}_5\text {OH}\text {(l)} \rightarrow \text {CH}_3\text {COOC}_2\text {H}_5\text {(l)}
+ \text {H}_2\text {O}\text {(l)} \] are given as \(\Delta G^\circ _{298} = -4650\) J/mol and \(\Delta H^\circ _{298} = -3640\) J/mol. If the solution is ideal and enthalpy change is assumed to be constant, the equilibrium constant at 95oC
is
MT-2011-32-td Given: \[ \begin {align*} 2\text {Cu}\text {(s)} + 0.5\text {O}_2\text {(g)} &= \text {Cu}_2\text {O}\text {(s)} \quad \quad \Delta G^\circ = -162200+69.24T, \quad J \\ 2\text {Cu}\text {(l)} + 0.5\text {O}_2\text {(g)} &= \text {Cu}_2\text {O}\text
{(s)} \quad \quad \Delta G^\circ = -188300+88.48T, \quad J \end {align*} \] The molar free energy change at 1300 K for the transformation of solid Cu to liquid Cu will be
MT-2012-35-td The reduction of FeO with CO gas in co-current flow is given by the following equation: \[ \text {FeO} + \text {CO} = \text {Fe} + \text {CO}_2 \quad \quad \Delta G^\circ = 8120 \text { J at 1173 K} \] The ratio of \(\bar {P}_{\text {CO}}/\bar {P}_{\text
{CO}_2}\) for this reaction at 1173 K is
1991-17-i-td Calculate the fraction of pure ethane that would dehydrogenate at 750 K and 5 atm, if the following reaction goes to equilibrium \[ \ce {C2H6(g)} \rightleftharpoons \ce {C2H4(g)} + \ce {H2(g)} \] \(\Delta G^{\circ }\) for the reaction at 750 K = 42.576
kJ. Assume ideal gas behaviour.
1994-10-td Ethanol can be prepared by the following vapor phase reaction from ethylene: \[ \ce {C2H4(g)} + \ce {H2O(g)} \rightleftharpoons \ce {C2H5OH(g)} \] The value of \(\Delta G^\circ \) for the above reaction at 1 atm and 125\(^\circ \)C is 5040 J. Calculate
the conversion obtained if an isothermal reactor operating at 125\(^\circ \)C and 2 atm is fed with a mixture containing 50 mol% ethylene and 50 mol% steam. Assume that equilibrium is reached at the exit of the reactor and gases behave ideally.
0200-9-td Compute the equilibrium mole fraction of each of the species in the gas phase reaction \(\ce{CO2}\) + \(\ce{H2}\) = \(\ce{CO}\) + \(\ce{H2O}\) at 1000 K and at (a) 1 atm total pressure, and (b) at 500 atm total pressure. The reaction equilibrium constant \(K\) = 0.693 at 1000 K. Standard state is pure gases at 1000 K and 1 atm pressure. Initially there are
equal amounts of \(\ce{CO2}\) and \(\ce{H2}\) present. The fugacity coefficients at 500 atm pressure for the species are:
For \(\ce{CO2}\)
0.99
\(\ce{H2}\)
1.15
\(\ce{CO}\)
1.08
\(\ce{H2O}\)
0.86.
1988-6-a-v-td
Activity of a component in solution is defined as the ratio of its --------------- to its ---------------
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