When exactly one mole of chrysene, C18H12(s) is burned at 25°C in a calorimeter, ΔE = -8942.6 kJ. When any hydrocarbon like chrysene is burned completely, the products are CO2 and H2O. (a) Write and balance the chemical equation for the combustion reaction of chrysene. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) (b) Determine the value of ΔH per mole for the combustion of chrysene at 298 K (25°C).   kJ/mol (c) When 1.1112 g of chrysene C18H12(s), was burned in a bomb, the temperature rose from 21.82°C to 25.28°C. What is the heat capacity of this calorimeter?   kJ/°C

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When exactly one mole of chrysene, C18H12(s) is burned at 25°C in a calorimeter, ΔE = -8942.6 kJ. When any hydrocarbon like chrysene is burned completely, the products are CO2 and H2O.

(a) Write and balance the chemical equation for the combustion reaction of chrysene. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.)

(b) Determine the value of ΔH per mole for the combustion of chrysene at 298 K (25°C).
  kJ/mol

(c) When 1.1112 g of chrysene C18H12(s), was burned in a bomb, the temperature rose from 21.82°C to 25.28°C. What is the heat capacity of this calorimeter?
  kJ/°C
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