Given the thermochemical equations X2+3Y2⟶2XY3.       Δ?1=−340 kJ    X2+2Z2⟶2XZ2        Δ?2=−190 kJ   2Y2+Z2⟶2Y2Z         Δ?3=−250 kJ   Calculate the change in enthalpy for the reaction. 4 XY3+7 Z2⟶6 Y2Z+4 XZ2

Using the table of standard formation enthalpies that you'll find under the ALEKS Data tab, calculate the reaction enthalpy of this reaction under standard conditions: 2 HNO₂(g) + O₂(g) →2 HNO3(g) Round your answer to the nearest kJ. ៣ kJ x10 X

Calcium acetate, Ca(CH3COO)2 has a molar mass of 158.17 g/mol. In a constant pressure calorimeter, 44.2 g of Ca(CH3COO)2 is dissolved in 861g of water at 25.00 °C. The heat produced by the solution was determined to be 15kJ. What is the final temperature of the solution? q= - msAT SH20 = 4.184 29.0 °C O 18.4 °C O 64.6 °C O 33.8 °C O 3.96 °C O 21.0 °C

55. Does the standard enthalpy of formation of H2O(g) differ from ΔH° for the reaction 2H2(g)+O2(g)⟶2H2O(g)?

Calculate the change internal energy (AE or AU) for a system that is gaining 65.0 kJ of heat and has 855 J of work performed on it by the surroundings. Be mindful of units and signs. 65.9 kJ O -64.1 kJ O -65.9 kJ -65.0 kJ O 64.1 kJ

If a system has 5.00×102 kcal5.00×102 kcal of work done to it, and releases 5.00×102 kJ5.00×102 kJ of heat into its surroundings, what is the change in internal energy (Δ? or Δ?)(ΔE or ΔU) of the system?

why is heat a path function when enthalpy is a state function? ( H = q + w)

to calculate the true enthalpies of these reactions by the Hess’ law, as: ΔH°(rxn) = Σ[ν × ΔHf°(product)] – Σ[ν × ΔHf°(reactant)] for: Mg(s) + ½O2(g) → MgO(s)