enthalpy

Which equation would correctly calculate the enthalpy for the reaction: 2H2 + O2(g) → 2H2O(g)? - ΔΗq(H2o) – (ΔΗq(02) + ΔΗq(H2)) a. ΔΗ = b. ΔΗ = ΔΗ;(H2O) C. ΔΗ = 2ΔΗ,(H2O) d. ΔΗ = 2Hg(H2o) + 2ΔΗ,ap(H2O) e. ΔΗ = 2Hg(H20) – 2ΔΗvap(120)

Please don't provide handwritten solution

Using the information in the table below, calculate the heat of released from the following reaction in kJ per g of  NO. ( Mw. Of NO = 30.01 g/mol).                 4NH3(g)   +  5O2 (g)                6H2O(g)  +  4 NO(g)   NH3 H2O NO Hfº (kJ/mol) - 46.1 -241.8 + 90.3

04) (g Calculate the volume of air at 30°C and 1.00 atm that is needed to burn completely 10.0 grams of propane. Assume that air is 21.0 percent O₂ by volume. The heat of combustion of propane is -2,220.1 kJ/molrxn. Calculate the heat of formati of propane given that AHO of H₂0(1) = -285.3 kJ/mol and AHO of CO2(g) = -393.5 kJ/ f AH-[(3•Co₂) + (4•H₂0)]-[C3H8 + 5(0₂)] [ F)+(4(-285.3)]-[AH C3H5] [200

Consider the following reaction: CH4 (9) + 20, (g) → CO2(g) + 2H,0(1) AH=-891 kJ a. Calculate the enthalpy change if 2.59 g methane is burned in excess oxygen. Enthalpy change = kJ b. Calculate the enthalpy change if 3.04 × 10° L methane gas at 737 torr and 25°C is burned in excess oxygen. Enthalpy change = kJ

For a particular isomer of Cg H₁g, the combustion reaction produces 5108.7 kJ of heat per mole of C, H₁g (g) consumed, under standard conditions. 25 Cg H18 (8) + O₂(g) →→→ 8 CO₂(g) + 9 H₂O(g) What is the standard enthalpy of formation of this isomer of Cg H₁g (g)? AH; = $ V T B MacBook Air Y H & 7 8 AH-5108.7 kJ/mol 18 N M K 1 38 kJ/mol

Consider the following equation:  CH4 + 02 -> H2O + CO2 +890 kJ 1. Balance the Equation 2. How much heat is released when 5.50L of oxygen is reacted with methane at STP? 1 mole of oxygen will occupy 22.4L at STP (standard temperature and pressure (0 degrees celsius) and standard pressure (1atm)).

Q4: Calculate the enthalpy of the reactions below: 1. H;Om + CO2 (aq) - H,CO3 (aa) 2. H;POalag) + 3OH, → 3H;0m + POaloa) 3. C;Ha (a) + 302 () → 2H,06) + 2CO2 (9) AHP of H,CO3 (oa) is -699.65 kJ/mole

Sucrose, C12 Hzm011, is common table sugar. The enthalpy change at 25°C and 1 atm for the complete burning of 3 mol of sucrose in oxygen to give CO:(9) and H3O(1) is - 1.692 x 10' kJ. From this and from data given below: AH; (H2O(1)) =-285.8 kJ/mol AH(CO2(9) = -393.5 kJ/mol AH (02(9)) = 0 kJ/mol Calculate the standard enthalpy of formation of sucrose. AH; - k]/mol