Thermodynamics ...

How much energy is needed to convert $$100\ g$$ of ice at $$263\ K$$ to liquid water at a temperature of $$283\ K$$?
$${C}_{ice}=0.49\ cal/({g}^{o}C)$$
$${C}_{water}=1.00\ cal/({g}^{o}C)$$
$$\Delta {H}_{fus}= 79.8\ cal/{g}$$
$$\Delta {H}_{vap}=540\ cal/g$$

For a reaction to be spontaneous, the sign on delta G should be :

Which of the following is most likely to produce a spontaneous reaction?

If the gibbs free energy is negative than reaction will be?

An ideal mono-atomic gas of given mass is heated at constant pressure. In this process, the fraction of supplied energy used for the increase of the internal energy of the gas is

$$Mg(s) \rightarrow \rightarrow \rightarrow Mg^{2+}$$ ; Energy = A KJ/mol.
$$Cl_{2}(g) \rightarrow \rightarrow \rightarrow 2Cl^{-}$$ ; Energy = B KJ/mol.
What is the $$\triangle H_{f}$$ of $$MgCl_{2}$$ if lattice enthalpy involved is C KJ/mol ?

For $$A\rightarrow B,\, \Delta H=4\,\text{kcal mol}^{-1}$$, $$\Delta S=10 \,\text{cal mol}^{-1}K^{-1}$$. Reaction is spontaneous when temperature is:

For spontaneity of cell, which is correct?

The process is spontaneous at the given temperature, if:

Consider the below diagram of heat transfer and work transfer for a system. What will be the first law equation for the below system?