Class 11th

We cannot universally say that negative enthalpy is the cause for spontaneity in chemical reactions. Though it is commonly seen in spontaneous reactions that heat releases or follows the exothermic definition, some spontaneous reactions can also absorb heat. They can be endothermic in nature. With that, we get a positive value for enthalpy change. So the better approach is to look into entropy and Gibbs Energy. These two quantities can define or tell us that a chemical process is spontaneous when the total entropy change is positive and when the Gibbs energy change is negative. 

This can be a little confusing when we already know the equation from the First Law of Thermodynamics (delta U = q + W) has internal energy as a state function. Work (W) and heat (q) are dependent on the path entirely, but internal energy is only concerned with initial and final states. We can consider the example of work done for an extremely slow or quick process of a gas expanding. The work done for slow work will be different from that of a faster one, but their initial and final states won't have any effect. 

${\left(C_v\right)}_{mix}=\left(\frac{2*\frac{3}{2}+6*\frac{5}{2}}{2+6}\right)R$

$=\frac{\left(3+15\right)R}{8}=\frac{9}{4}R$

Kindly go through the solution

HBrO₂ has least existence

Kindly go through the solution

NO is a neutral oxide.

            E =   $\frac{Stress}{Strain}$

As temperature increases, strain increases

Elasticity decreases

10 M = 11 V

Þ  1V =   $\frac{10}{11}$ * 5 mm

Þ  LC = |M – V|

      =   $\frac{5}{11}$ mm