At 1 atm, how much energy is required to heat 51.0 g H2O(s) at −24.0 ∘C to H2O(g) at 159.0 ∘C? Use the heat transfer constants found in this table.   q = _____________ kJ

For a particular isomer of C8H18, the combustion reaction produces 5104.1 kJ of heat per mole of C8H18(g)consumed, under standard conditions.   C8H18(g)+25/2O2(g)⟶8CO2(g)+9H2O(g)  Δ?∘rxn=−5104.1 kJ/mol What is the standard enthalpy of formation of this isomer of C8H18(g)?

Given the following thermochemical equations: C2H29) + 5 02(9) 2C02(g) + H201) AH° = -1229.5 kJ AH° = -393.5 kJ C(6) + 02(g) → C02(g) 1 H2(9) +5 02(9) → H20) AH° = -285.5 kJ 2 Calculate the enthalpy (in kJ) for this reaction: 206) + H2(g) → C,H2(9)

Calculate the energy required to heat 0.30kg of graphite from −4.8°C to 13.1°C . Assume the specific heat capacity of graphite under these conditions is 0.710J·g−1K−1 . Be sure your answer has the correct number of significant digits.

Part III: Determine the molar enthalpy change for reaction 3 using Hess’s law          HCl(aq)  +  NH3(aq) ®  NH4Cl(aq)         DH3 = A. In the space below, show all calculation set-ups to determine the molar heat of enthalpy, in kJ/mol HCl, of reaction 3 (DH3). For full credit, all numerical answers must be rounded off to correct sig figs and with proper units