Question

D Question 6 1 pts Given the balanced chemical equation: Ba(NO3)2(aq)+ Na2SO4(aq) BaSO4(s) + 2 NaNO3(aq) ons A 0.30 L of 0.15 M Ba(NO3)2(aq) is mixed with excess Na2SO4(aq) to make 200.0 g of solution in a coffee-cup calorimeter and allowed to react completely. The temperature of the solution rises from 23.5 °C to 24.9 °C. Answer the question in each step to find ΔHrxn for this reaction. Csson-4.18 J/g °C Stirrer sources Cover Step 1: The reaction is I Select ) temperature increases. The heat absorbed by the solution (asoln) is cover because the solution m Matrix I Select ] Reaction mixture Step2: The heat associated with the reaction (grml is I Select ] Step 3: Use qrxn and the stoichiometric relations in the balanced chemical equation to calculate ΔΗΧη. ΔΗΧη IS [ Select ] Previous Next

Answer 1

Given balanced chemical equation: Ba(NO_3)_2(aq) + No_2 So_4(aq) rightarrow BaSO_4(s) + 2 NaNO_3(aq) Molar mass 261.33 mol 142 g/mol A 0.30 L of 0.15 m Ba(NO_3) (aq) is mixed with excess Na_2SO_4CO make 200 g of solution in a coffee cup calorimeter & allowed to rest completely The temp of the solution rises from 23.5 degree to 24.9 degree Answer the question in each step to find delta H_times n \or this reaction. C_s, soln = 4.18 J/g degree C Step I The reaction is exothermic because the solution temperature increases Step II Heat(q_r times n) associated with is given by m times c times delta T where m is mass of reaction mixture C is specific heat capacity of water delta T is change in temp of solution \r\n since 200g of mixture is produced, so by law conservation of mass. Mass of reactant solution = 200 g T_final = 24.9 degree, T_initial = 23.4 degree C Hence q_r times n = mass of