Sulfur dioxide reacts with oxygen to produce sulfur trioxide. Thermodynamic Data Substance ΔfH∘ (kJ mol−1) ΔfG∘ (kJ mol−1) S∘ (J mol−1 K−1) Sulfur dioxide −296.8 −300.2 248.2 Oxygen 0 0 205.1 Sulfur trioxide −395.7 −371.1 256.8   Calculate the enthalpy change of the reaction. Calculate the entropy change of the reaction. Calculate the free energy change of the reaction at 230.0 ∘C.

What is the enthalpy change for the first reaction? CH4(g) + 1/2O2(g) → CH3OH(g) ΔH =  CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)  ΔH = -806.5 CH3OH(l) + 3/2 O2 → CO2(g) + 2H2O(g)  ΔH = -676.7

Ethanol can be made from the fermentation of crops and has been used as a fuel additive to gasoline.         C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(g)C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(g)   Part B Calculate ΔrH∘ (The standard enthalpy of formation of liquid ethanol is −277.6 kJmol−1, of gaseous carbon dioxide is −393.5 kJmol−1, and of gaseous water is −241.8 kJmol−1.) Express your answer in kilojoules per mole to one decimal place.

Calculate ΔHrxn for the reaction: 7 C (s) + 8 H2 (g) → C7H16 (g) The following reactions and associated ΔHrxn values are may likely be helpful to you: Reaction A: C7H16(g) + 11 O2 (g) → 7 CO2 (g) + 8 H2O (g) ΔHrxn = -4817 kJ Reaction B: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ Reaction C: 2 H2 (g) + O2 (g) → 2 H2O (g) ΔHrxn = -483.6 kJ

Compound ΔHf (kj/mol) C2H5OH(i) -277.6 H2O(i) -285.8 H2O(g) -241.8 CO2(g) -393.5 CO(g) -110.5 H2O2(i) -187.6 C3H8(g) -103.8 What is the ΔH for the following reaction? C2H5OH(i) + 3O2 (g) --> 2CO2(g) + 3H2O(i)

Methanol (CH3OH) can be used as the fuel in a "canned heat" container that is used to keep food hot on a buffet table.  The combustion of methanol can be described by the following BALANCED thermochemical equation: 2 CH3OH(l)  +  3 O2(g)  →  2 CO2(g)  +  4 H2O(g)   ΔH° = –1199 kJ Calculate the enthalpy change, in kilojoules, when 151.3 g of methanol is burned via this reaction?

Compound ΔHf,ΔHf, (kJ/mol)(kJ/mol) Al2O3(s)Al2O3(s) −− 1675.7 CO(g)CO(g) −−110.5 Al(s)Al(s) 0 CO2(g)CO2(g) −−393.5 Use standard enthalpies of formation in the table above to determine ΔHorxnΔHrxno for the reaction: Al2O3(s)+3CO(g)→2Al(s)+3CO2(g)

How much heat must be removed from a 90.5 g sample of benzene (M = 78.11 g mol-1) to cool the sample from 305 K to 215 K?  The following physical data may be useful.ΔfusH = 9.8 kJ mol-1ΔvapH = 30.8 kJ mol-1Cs(l) = 1.73 J g-1 K-1Cs(s) = 1.51 J g-1 K-1Cs(g) = 82.4 J g-1 K-1 Tm = 279.0 KTb = 353.3 K Note: The word 'removed' in the question already accounts for the negative sign involved in the heat transfer.   Express your answer to three significant figures.

A chemist measures the enthalpy change AH during the following reaction: 2 KCl(s) + 302(g) →2 KClO3(s) AH=78. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction ΔΗ ㅁ x10 2K C103 (s) → 2KC1(s) + 302(g) KCIO, (s)-KCI(s) + 0,(s) 3 KCI(s)+0, (g)KCIO, (s) kJ kJ 1 5

Given the following reaction: 2NO (g) + O2 (g) → 2NO2 (g)           ΔrH0 = - 114.1 kJ/mol Calculate the enthalpy change when 1.25 g of NO gas is converted completely converted to NO2 gas. Enter your answer to 2 decimal places.