Q1: Conversion achieved in HNO₃ synthesis with the use of platinum catalyst is about 95-97%. The rate of formation of nitrogen dioxide from the oxidation of nitric acid is favoured by

ANS:C - increasing the temperature.

The rate of formation of nitrogen dioxide (NO2) from the oxidation of nitric acid (HNO3) is favored by increasing the temperature. In the synthesis of nitric acid, one of the steps involves the oxidation of nitric oxide (NO) to nitrogen dioxide (NO2). This reaction is typically carried out at high temperatures, and it is catalyzed by a platinum catalyst. The reaction can be represented as follows: 2 NO+O2→2 NO22 NO+O2​→2 NO2​ By increasing the temperature, the kinetic energy of the molecules increases, leading to more frequent and energetic collisions between reactant molecules. This results in a higher rate of reaction and facilitates the conversion of nitric oxide to nitrogen dioxide. Therefore, increasing the temperature favors the forward reaction, leading to a higher rate of formation of nitrogen dioxide. Decreasing the pressure or temperature would generally have the opposite effect, as these changes would reduce the kinetic energy of the molecules and decrease the likelihood of successful collisions. Therefore, decreasing the pressure or temperature would not favor the rate of formation of nitrogen dioxide.