15. Using the standard enthalpies of formation for the chemicals involved, calculate the enthalpy change for the following reaction. (Note: Show the math clearly and provide units in your setup) (AH, Values in kJ/mol are as follows: NO, +32, H,0 -286, HNO, -207, NO +90) 3NO2(e) + H,O O 2HNO3(aq) + NO) (1)

Find the enthalpy of reaction for the equation: H2SO4laq) + 2NAOH(aq)-Na,SO,(aq) + 2H20(), AH=? Using the following equations whose enthalpy is known (please round your answer to the tenths place): H2(g) + S(s) + 202(g) – H2SO,(aq), AH= -907.5 kJ Na(s)+ ½H2(g) + ½O2{g) – NaOH(aq), AH= -469.6 kJ 2Na(s) + S(s) + 20,(g) – Na,SOal(aq). AH= -1387.1 kJ H2(8) + ½O2(g) – H2O(1). AH= -285.8 kJ AH= kJ.

Use Hess’s law to calculate the enthalpy change for the reaction WO3(s) + 3H2(g) —> W(s) +3H2O(g) from the following data: 2W(s) + 3O2(g) —> 2 WO3(s) H=-1685.4 2H2(g) + O2(g) —> 2H2O(g) H=-477.84

The standard molar enthalpy of formation for oxygen gas, ?2(?), is zero. The enthalpy of formation for atomic oxygen, ?(?), is +250??/???. Why is there a difference in these values?

Can you help me with this?

（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g)     ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A?   （2）Consider the reaction: C (s) + O2 (g) → CO2 (g)     ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?

Please don't provide handwritten solution ....

Sulfur dioxide, SO, (g), can react with oxygen to produce sulfur trioxide, SO, (g), by the reaction 2 SO, (g) + 0,(g) → 2 SO,(g) The standard enthalpies of formation for SO,(g) and SO, (g) are AH; [SO,() = -296.8 kJ/mol AH; SO,( = -395.7 kJ/mol Calculate the amount of energy in the form of heat that is produced when a volume of 4.10 L of SO, (g) is converted to 4.10 L of SO, (g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C. Assume ideal gas behavior. kJ AL = 18.249 incbrcect