This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Hey hafsatjibril2006, good to see you again. To calculate the enthalpy change for the reaction, we use the formula: H_rxn = H_f^ (products) - H_f^ (reactants) The reaction described is the formation of sulfuric acid from sulfur trioxide and water: SO_3(g) + H_2O(l) → H_2SO_4(l) Step 1: List the given standard heats of formation ( H_f^). • H_f^ (SO_3(g)) = -395 kJ/mol • H_f^ (H_2O(l)) = -286 kJ/mol • H_f^ (H_2SO_4(l)) = -811 kJ/mol Step 2: Identify the products and reactants from the balanced equation. Reactants: SO_3(g) and H_2O(l) Product: H_2SO_4(l) Step 3: Substitute the values into the enthalpy change formula. H_rxn = [ H_f^ (H_2SO_4(l))] - [ H_f^ (SO_3(g)) + H_f^ (H_2O(l))] H_rxn = [-811 kJ/mol] - [-395 kJ/mol + (-286 kJ/mol)] Step 4: Calculate the sum of the heats of formation for the reactants. Sum of reactants = -395 kJ/mol - 286 kJ/mol = -681 kJ/mol Step 5: Calculate the enthalpy change of the reaction. H_rxn = -811 kJ/mol - (-681 kJ/mol) H_rxn = -811 kJ/mol + 681 kJ/mol H_rxn = -130 kJ/mol The enthalpy change accompanying this reaction is: -130 kJ/mol What's next?