For an exothermic reaction, what effect will increasing the temperature have on the equilibrium? (a) there will be a shift toward the products. (b) there will be a shift toward the reactants. (c) there will not be a shift in equilibrium. (d) not enough information is given.

Option (B) is the correct answer.

Explanation:

According to Le Chatelier's principle, any disturbance caused in the equilibrium reaction will shift the equilibrium in a direction that oppose the change or disturbance.

As the given reaction is exothermic in nature. So, when we increase the temperature then more heat will be releasing on product side. Therefore, equilibrium will shift in a direction where there will be less heat or low temperature.

Hence, equilibrium will shift in the backward direction.

Thus, we can conclude that for an exothermic reaction, increasing the temperature on the equilibrium will be a shift toward the reactants.

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.