Calculate the enthalpy of formation of 1 mole SO2(g) from the standard enthalpy changes of the following reactions: 280;(g) 25(s) + 30,(g) S(s) + O2(8) 2S0,(g) +0,(g) → 2S0,(g) → SO,(8) AH°. rxn 1 = +196 kJ AHrxn 2 = -790 kJ AH°xn 3=?

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Using the standard enthalpies of formation, what is the standard enthalpy of reaction? CO(g) + H,O(g) –→ CO,(g) + H,(g) AHân = kJ

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7.Using the following standard enthalpies of reaction4NH3(g) + 7 O2(g) 4 NO2(g) + 6 H2O(l)H ̊rxn= -1395 kJN2(g) + 2 O22 NO2(g)H ̊rxn= +67.4 kJFind the standard enthalpy of reaction for the equation:2N2(g) + 6 H2O(l) 4 NH3(g) + 3 O2(g)   Based on your work above, determine the standard enthalpy of reaction for the following equation:N2(g) + 3 H2O(l) 2 NH3(g) + 3/2 O2(g)

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, HNO3 -207, NO +90) 3NO2(8) + H,Oy O 2HNO3(aq) + NO(g) (g),

（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?

Given the following enthalpy change values for the reactions below: A + B → 2C; AH = -485.1 kJ mol-¹ C + 2D + E +F; AH = 251.4 kJ mol-¹ ½E + G +H; AH = 471.1 kJ mol-¹ Calculate A,H for the following reaction (in kJ mol-¹) using Hess's Law: A + B + 4D + 4G → 4H + 2F Answer:

The standard heat of formation, AH;, is defined as the enthalpy change for the formation of one mole of Part B substance from its constituent elements in their standard states. Thus, elements in their standard states have AH: = 0. Heat of formation values can be used The combustion of ethene, C2H4, occurs via the reaction to calculate the enthalpy change of any reaction. C2H4 (g) + 302 (g)→2CO2(g) + 2H20(g) Consider, for example, the reaction with heat of formation values given by the following table: 2NΟ (5) + Ο, (s) 2ΝO, (g) ΔΗρ (kJ/mol) Substance with heat of formation values given by the following table: C2H4 (g) 52.47 CO2 (g) -393.5 Substance (kJ/mol) H2O(g) -241.8 NO(g) 90.2 Calculate the enthalpy for the combustion of ethene. 02 (g) Express your answer to four significant figures and include the appropriate units. NO2(g) 33.2 • View Available Hint(s) Then the heat of formation for the overall reaction is ΔΗ ΔΗ (products) -ΔΗ; (reactants ) [2(90.2) + 0] HA ? 2(33.2) -114 kJ/mol…