6. A student is determining the enthalpy of solution for ammonium nitrate by adding ammonium nitrate to a calorimeter and measuring the temperature change. The accepted value is AH = 25.7 kJ/mol. sol'n A student, not paying attention, adds 1.5g of ammonium nitrate instead of 1.0g. When they perform their calculations, they use 1.0g as the mass. Will their calculation result in an answer that is higher than the accepted value or lower? Explain.

For the denitrification [microbiological conversion of nitrite/nitrate (N-containing contaminants) to nitrogen gas (harmless end product)] to be more effective, an external carbon source (e.g., methanol) is frequently added for denitrifiers (denitrifying microorganisms) during the reaction. The following chemical reaction is for when methanol is added for this purpose. Calculate how much (concentration) of methanol (in mg/L) needs to be added to completely convert 30 mg/L of NO3--N to N2 gas. 0.1667 CH3OH + 0.1343 NO3- + 0.1343 H+ ↔ 0.0143 C5H7O2N + 0.06 N2 + 0.3505 H2O + 0.0952 CO2

at of Reaction The heat of reaction, AH, is the amount of heat absorbed or released uring a chemical reaction. It is calculated as the difference in energy of the products and the reactants. gure Energy diagram B Progress of reaction Type here to search D < 1 of 1 O II CD Label the energy diagram (Eigure 1) by matching each term to the appropriate letter from the graph. Drag each item to the appropriate bin. View Available Hint(s) Submit energy of heat of products reaction B energy of reactants activation energy D Reset Help 3

Heating solid ammonium nitrate enhances its reversible decomposition into dinitrogen monoxide and water vapour. a)  Write a balanced chemical equation with physical states for the reaction just described. b)  Write the law of mass action (aka equilibrium expression) consistent with the equation you wrote in (a).