Question

Thermometer A sample of solid bianthracene (C28H18) that weighs 0.5254 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.190 °C. The heat capacity of the calorimeter and its contents is known to be 9.405x103 JK. Ignition wires heat sample Stirrer (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank. Water Based on this experiment: (b) Assuming that AHⓇ is approximately equal to AE, calculate the standard enthalpy change for the combustion of 1.000 mol of bianthracene to CO2(g) and H2O(). Insulated outside chamber Sample dish Burning sample Steel bomb kJ mol-1 Combustion (bomb) calorimeter. (c) Calculate the standard enthalpy of formation per mole of bianthracene, using the following for the standard enthalpies of formation of CO2(g) and H2000). AH, H20 (2) =-285.83 kJ mol!; AH; CO2(g) = -393.51 kJ mol"!

Answer 1

balanced chemical equalin;- a) 2 C23 H 1 s 650, c) 56 co c18 H2 molusdr sHis o 5254/35 -3 -1.484x10 7. 405 x1ox (2 10) 20 596 5 - 20 51/0.00144 .596 AH - 388 xO -393-51 18x- 28583) - 2918-5-2 CHir 389.4 - 20530 - 20530