# A sample of solid biphenyl (C12H10) that weighs 0.4800 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 2.100°C. The heat capacity of the calorimeter and its contents is known to be 9.273×103 J K-1.(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.Based on this experiment:(b) Assuming that ΔH° is approximately equal to ΔE, calculate the standard enthalpy change for the combustion of 1.000 mol of biphenyl to CO2(g) and H2O(). c) Calculate the standard enthalpy of formation per mole of biphenyl, using the following for the standard enthalpies of formation of CO2(g) and H2O().ΔHf° H2O () = -285.83 kJ mol-1 ;   ΔHf° CO2(g) = -393.51 kJ mol-1

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A sample of solid biphenyl (C12H10) that weighs 0.4800 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 2.100°C. The heat capacity of the calorimeter and its contents is known to be 9.273×103 J K-1.

(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.

Based on this experiment:

(b) Assuming that ΔH° is approximately equal to ΔE, calculate the standard enthalpy change for the combustion of 1.000 mol of biphenyl to CO2(g) and H2O().

c) Calculate the standard enthalpy of formation per mole of biphenyl, using the following for the standard enthalpies of formation of CO2(g) and H2O().
ΔHf° H2O () = -285.83 kJ mol-1 ;   ΔHf° CO2(g) = -393.51 kJ mol-1

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Step 1

(a) The balance the chemical equation for the combustion reaction is given

Step 2

(b) Standard enthalpy change for t...

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