A sample of solid acetylsalicylic acid (C₂H804) that weighs 0.9205 g is burned in an excess of oxygen to CO₂(9) and H₂O(

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A Sample Of Solid Acetylsalicylic Acid C H804 That Weighs 0 9205 G Is Burned In An Excess Of Oxygen To Co 9 And H O 1 (31.96 KiB) Viewed 12 times

A sample of solid acetylsalicylic acid (C₂H804) that weighs 0.9205 g is burned in an excess of oxygen to CO₂(9) and H₂O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.130 °C. The heat capacity of the calorimeter and its contents is known to be 9.285x10³ JK¹. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. + Based on this experiment: (b) Assuming that a is approximately equal to AE, calculate the standard enthalpy change for the combustion of 1.000 mol of acetylsalicylic acid to CO₂(g) and H₂O(₂). k3 mol + kJ mol Ignition wires heat sample Water Stirrer Thermometer Sample Burning Steel dish sample bomb Insulated outside chamber Combustion (bomb) calorimeter. (c) Calculate the standard enthalpy of formation per mole of acetylsalicylic acid, using the following for the standard enthalpies of formation of CO₂(9) and H₂O(₂). AH H₂0 (₂) -285.83 k3 mol¹; AH CO₂(0) -393.51 kJ mol-1