Two moles of an ideal gas is heated at a constant pressure of one atmosphere from 27$°$C to 127$°$C. If ${\mathrm{C}}_{\mathrm{v}, \mathrm{m}}=20+{10}^{-2} \mathrm{T} {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1},$ then q and $△\mathrm{U}$ for the process are respectively:

1.  6362.8 J, 4700 J

2.  3037.2 J, 4700 J

3.  7062.8 J, 5400 J

4.  3181.4 J, 2350 J

Calculate ${△}_{\mathrm{f}}\mathrm{H}°$ (in kJ/mol) for ${\mathrm{Cr}}_2{\mathrm{O}}_3$ from the ${△}_{\mathrm{r}}\mathrm{G}°$ and the $\mathrm{S}°$ values provided at 27$°$C

$4\mathrm{Cr}\left(\mathrm{s}\right)+3{\mathrm{O}}_2\left(\mathrm{g}\right)$ $\to$ $2{\mathrm{Cr}}_2{\mathrm{O}}_3\left(\mathrm{s}\right);$ $$
${△}_{\mathrm{r}}\mathrm{G}°=-2093.4$ $\mathrm{kJ}/\mathrm{mol}$

$\mathrm{S}°\left(\mathrm{J}/\mathrm{K}\right)$ $\mathrm{mol}$ $:$ $\mathrm{S}°\left(\mathrm{Cr},\right)$ $\mathrm{s}=24;$ $$
$\mathrm{S}°\left({\mathrm{O}}_2,\right)$ $\mathrm{g}=205;$ $$ $$ $\mathrm{S}°\left({\mathrm{Cr}}_2{\mathrm{O}}_3,\right)$ $\mathrm{s}=81$

1.  -2258.1 kJ/mol

2.  -1129.05 kJ/mol

3.  -964.35 kJ/mol

4.  None of the above

The standard heat of combustion of propane is –2220.1 kJ mol^–1. The standard heat of vaporisation of liquid water is 44.0 kJ mol^–1. The enthalpy change for the reaction is–

C₃H₈ (g) + 5O₂ (g) $\to$ 3CO₂ (g) + 4H₂O(g)

Consider the following reaction,

S + O₂ $\to$ SO₂,  $∆$H = – 298.2 kJ mole^–1

SO₂ + 1/2 O₂ $\to$  SO₃, $∆$H = – 98.7kJ mole^–1

SO₃ + H₂O $\to$ H₂SO₄ , $∆$H = – 130.2 kJ mole^–1

H₂ + 1/2 O₂ $\to$ H₂O, $∆$H = – 287.3 kJ mole^–1

the enthalpy of formation of H₂SO₄ at 298 K will be–

2.1 g of Fe combines with S evolving 3.77 kJ. The heat of formation of FeS in kJ/mole is–

The bond energy of H—H and Cl-Cl is 430 kJ mol^-1 and 240 kJ mol^-1 respectively
and ΔH_f for HCl is -90 kJ mol^-1. The bond enthalpy of HCl is:

1. 290 $kJ$ $mo{l}^{-1}$

2. 380 $kJ$ $mo{l}^{-1}$

3. 425 $kJ$ $mo{l}^{-1}$

4. 245 $kJ$ $mo{l}^{-1}$

The values of ΔH and ΔS for the given reaction are 170 kJ and 170 JK^-1, respectively.
C_(graphite) + CO₂(g)→2CO(g) 
This reaction will be spontaneous at:

1. 710 K
2. 910 K
3. 1110 K
4. 510 K

From the following bond energies:
H—H bond energy: 431.37 kJ mol^-1 
C=C bond energy: 606.10 kJ mol^-1 
C—C bond energy: 336.49 kJ mol^-1 
C—H bond energy: 410.50 kJ mol^-1 
Enthalpy for the reaction, 

will be:

Pairs correctly represent intensive property among the following is:

1. Entropy, Gibb’s energy

2. Enthalpy, Heat capacity

3. Electrode potential, Vapour pressure

4. Resistance, Conductance