In a reversible isothermal process, the change in internal energy is

• zero 

• positive

• negative

• None of these

Based on the following thermochemical equations

H₂O (g) + C(s) → CO (g) + H₂ (g); $∆$H = 131 kJ

CO (g) + $\frac{1}{2}$ O₂(g) → CO₂ (g); $∆$H = -282 kJ

H₂ (g) + $\frac{1}{2}$O₂ (g) → H₂O (g); $∆$H =-242 kJ

C (s) + O₂ (g) → CO₂ (g); $∆$H = X kJ

the value of X will be

• -393 kJ

• -655 kJ

• +393 kJ

• +655 kJ

Which of the following relationships is correct?

• $\mathrm{k}=\frac{\mathrm{T}∆\mathrm{S}°-∆\mathrm{H}°}{\mathrm{RT}}$

• $\mathrm{k}=\frac{∆\mathrm{H}°-\mathrm{T}∆\mathrm{S}°}{\mathrm{RT}}$

• $\ln k=\frac{∆\mathrm{H}°-\mathrm{T}∆\mathrm{S}°}{\mathrm{RT}}$

• $\ln \mathrm{k}=\frac{\mathrm{T}∆\mathrm{S}°-∆\mathrm{H}°}{\mathrm{RT}}$

464.

Which of the following represents the first law of thermodynamics?

• $∆$U = q + W

• $∆$U = p . $∆$V

• $∆\mathrm{U} = ∆\mathrm{H} + \mathrm{P}.∆\mathrm{V}$

• $∆$H = q + W

Heat of neutralization of HCl and NaOH is

• -13.7 kcal

• -13.7 J

• -13.7 kJ

• None of these

Which is true for a cyclic process?

• ΔE= 0

• ΔE= q- W

• q =W

• All of these

When solid melts, there will be

• a decrease in enthalphy

• a decrease in free energy

• a decrease in entropy

• all the above factors remain constant

To convert 94 g of ice at 0°C into 94g of vapour at 100° C, the quantity of coal (90% carbon) required is : (ΔH_c of carbon = -94 k cal mol^-1);latent heat of fusion = + 80 cal per gm; latent heat ofvaporisation=+ 540 cal per gm; specificheat of water = 1 cal per gm per °C).

• 94g

• 80g

• 9.4g

• 9.6 g

When 1 M H₂SO₄ is completely neutralized by NaOH, the heat liberated is 114.64 kJ. What is the enthalpy of neutralization?

• + 114.64 kJ

• -114.64 kJ

• -57.32 kJ

• + 57.32 kJ

What is the free energy change $∆$G when 10 moles of water at 100°C and 1 atm pressure is converted into steam at 100° C and 1 atm pressure?

• 540 cal

• -9800 cal

• 9800 cal

• 0 cal