1
JEE Main 2016 (Online) 9th April Morning Slot
MCQ (Single Correct Answer)
+4
-1
Change Language
For the reaction,
A(g) + B(g) $$ \to $$ C(g) + D(g), $$\Delta $$Ho and $$\Delta $$So are, respectively, − 29.8 kJ mol−1 and −0.100 kJ K−1 mol−1 at 298 K. The equilibrium constant for the reaction at 298 K is :
A
1.0 $$ \times $$ 10$$-$$10
B
1.0 $$ \times $$ 1010
C
10
D
1
2
JEE Main 2016 (Offline)
MCQ (Single Correct Answer)
+4
-1
Change Language
The heats of combustion of carbon and carbon monoxide are –393.5 and –283.5 kJ mol–1, respectively. The heat of formation (in kJ) of carbon monoxide per mole is :
A
676.5
B
-676.5
C
–110
D
110.5
3
JEE Main 2015 (Offline)
MCQ (Single Correct Answer)
+4
-1
Change Language
The following reaction is performed at 298 K
2NO(g) + O2 (g) $$\leftrightharpoons$$ 2NO2 (g)
The standard free energy of formation of NO(g) is 86.6 kJ/mol at 298 K. What is the standard free energy of formation of NO2(g) at 298 K? (KP = 1.6 × 1012)
A
86600 + R(298) ln(1.6 $$\times$$ 1012)
B
86600 - $$ln (1.6 \times 10^{12}) \over R (298)$$
C
0.5[2×86,600 – R(298) ln(1.6×1012)]
D
R(298) ln(1.6×1012) – 86600
4
JEE Main 2014 (Offline)
MCQ (Single Correct Answer)
+4
-1
For complete combustion of ethanol, C2H5OH(l) + 3O2(g) $$\to$$ 2CO2(g) + 3H2O(l) the amount of heat produced as measured in bomb calorimeter, is 1364.47 kJ mol–1 at 25oC. Assuming ideality the Enthalpy of combustion, $$\Delta _CH$$, for the reaction will be : (R = 8.314 kJ mol–1)
A
–1460.50 kJ mol–1
B
– 1350.50 kJ mol–1
C
– 1366.95 kJ mol–1
D
– 1361.95 kJ mol–1
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