An environmental chemist got an idea that two serious pollutants (CO and NO) of the automobile exhaust can be converted to less harmful gases CO₂ and N2. The reaction is CO(g) + NO(g) CO2(g) + 2 N2(g). ΔΗ° = ?The enthalpy of this reaction as calculated from the following date isCO(g) + 1/2 O2(g)CO2(g). ΔΗ° = -283kJ/molCO(g) + O2(g) 2NO2(g). ΔΗ° = 180.6kJ/mol

Explanation

Let's calculate the enthalpy of the given reaction using Hess's Law. We'll use the enthalpies of the provided reactions to find the enthalpy change for the desired reaction.The given reactions are:CO(g) + 0.5 O2(g) → CO2(g) with ΔHo = -283 kJ/molCO(g) + O2(g) → 2NO2(g) with ΔHo = 180.6 kJ/molWe want to find the enthalpy change for the reaction: CO(g) + NO(g) → CO2(g) + 0.5 N2(g)Let's break down the desired reaction into steps:CO(g) + 0.5 O2(g) → CO2(g) (Given reaction 1)2NO2(g) → 2NO(g) + O2(g) (Reverse of given reaction 2)Now, let's apply Hess's Law. The enthalpy change for the desired reaction is the sum of the enthalpies of the individual steps:CO(g) + NO(g) → CO2(g) + 0.5 N2(g) (Desired reaction)ΔHo = ΔHo1 (from reaction 1) + ΔHo2 (from reverse of reaction 2)ΔHo = (-283 kJ/mol) + (-180.6 kJ/mol)ΔHo = -463.6 kJ/molTherefore, the enthalpy change for the given reaction is approximately -463.6 kJ/mol.Among the provided options, the closest value to this is -400.0 kJ (option d). However, it's not an exact match, so we may need to consider more precise values or potential rounding errors.Keep in mind that these values are approximate due to the precision of the given enthalpies and any rounding during calculations. Therefore, option d (-400.0 kJ) is the best choice based on the available options.