Thermodynamics ...

For $$Ag, \overline {C_{P}} (JK^{-1}mol^{-1})$$ is given by $$24 + 0.006\ T$$. If temperature of $$3\ mol$$ of silver is raised from $$27^{\circ}C$$ to its melting point $$927^{\circ}C$$ under $$1$$ atm pressure then $$\triangle H$$ is equal to:

For a certain reaction the change in enthalpy and change in entropy are $$40.63\ kJ\ ,ol\ KJ^{-1}$$. What is the value of $$\triangle G$$ at $$27^{\circ}C$$ and indicate whether the reaction is spontaneous.

The heat capacity of a bomb calorimeter is $$300\ J/K$$. When $$0.16\ gm$$ of methane was burnt in this calorimeter the temperature rose by $$3^{\circ}C$$. The value of $$\triangle U$$ per mole will be

The heat change during the reaction $$24g\ C$$ and $$128g\ S$$ following the change: 

$$NX$$ is produced by the following step of reactions:

Stearic acid $$\left[ C{ H }_{ 3 }\ { \left( C{ H }_{ 2 } \right)  }_{ 16 }\ C{ O }_{ 2 }H \right]$$ is a fatty acid, the part of fat that stores most of the energy. $$1.0\ g$$ of stearic acid was burned in a bomb calorimeter. The bomb had a heat capacity of $$652\ J/ C$$. If the temperature of $$500\ g $$ water $$\left( c=4.18J/g\ C \right)$$ rose from $$25.0$$ to $$39.3 C$$, how much heat was released when the strearic acid burned? $$[Given\ { C }_{ p }\left( { H }_{ 0 }O \right) =4.18\ { J }/{ g }\ C]$$

If an electron is moving in an orbit with total energy $$U = -\dfrac {e^{2}}{r} r$$ is radius of the orbit then find the speed of the electron.

$${E}^{o}$$ of an electrode half reaction is related to $$\Delta { G }^{ o }$$ by the equation, $${ E }^{ o }=-\Delta { G }^{ o }/nF$$. If the amount of $${Ag}^{+}$$ in the half reaction, $${ Ag }^{ + }+{ e }^{ - }\longrightarrow Ag$$ is tripled then:

Heat of reaction for the equation, $$A(s) + B(g) \rightarrow 2C(g)$$ is $$40\ kJ$$ at $$300\ K$$ at constant volume. Hence, heat of reaction at constant pressure and at $$300\ K$$ is___________.

On the basis of the following thermochemical data
$${ H }_{ 2 }{ O }_{ (g) }\longrightarrow { H }_{ (aq) }^{ + }+{ OH }_{ (aq) }^{ - };\Delta H=57.32kJ\quad $$
$${H}_{2(g)}+\cfrac{1}{2}{O}_{2(g)}\longrightarrow{ H }_{ 2 }{ O }_{ (l) };\Delta H=-286.2kJ$$
The value of enthalpy of formation of $${OH}^{-}$$ ion at $${ 25 }^{ o }C$$ is: