During neutralization of 1 mol HCl by NaOH increases the temperature of solution by 5°C. What would be the increase in temperature if 2 mol HCl is neutralised by NaOHa)5°C b) 10°C c)20°C d)2.5°C

To determine the increase in temperature when 2 moles of HCl are neutralized by NaOH, we first need to understand the concept of neutralization and how it relates to temperature change. In a neutralization reaction, an acid reacts with a base to produce water and a salt, releasing heat in the process. This heat release is known as the enthalpy of neutralization.

Understanding the Reaction

When 1 mole of HCl is neutralized by NaOH, the temperature of the solution increases by 5°C. This indicates that the reaction is exothermic, meaning it releases heat. The amount of heat released is proportional to the number of moles of acid and base involved in the reaction.

Proportionality of Temperature Change

The temperature change is directly related to the amount of acid being neutralized. If 1 mole of HCl results in a 5°C increase, then we can infer that doubling the amount of HCl to 2 moles will also double the heat released, leading to a greater temperature increase.

Calculating the Temperature Increase

Let’s break it down:

• 1 mole of HCl → 5°C increase
• 2 moles of HCl → 2 × 5°C = 10°C increase

Thus, when 2 moles of HCl are neutralized by NaOH, the expected increase in temperature would be 10°C.

Final Answer

Based on the calculations and the principles of thermodynamics involved in neutralization reactions, the correct answer is 10°C, which corresponds to option b) 10°C.