How much heat (in kJ) is needed to convert 10.0 grams of C2F6(m) at -100.05"c to C2F6(1) at -100.05 c? O 1) 37.1 kJ 0.195 kJ O 3) 2.69 KJ O 4) 16.15 kJ 5) 1.11 kJ
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- What is the standard heat of formation of C2H4 H2+1/2O2>H2O. -242kj/mol 2C+3H2+1/2O2>C2H5OH. -273kj/mol C2H4+H20>C2H5OH. -88kj/mol 2C+2H2>C2H4C(s) + O2(g) -> CO2(g) CH4(g) -> C(s) + 2 H2(g) ∆Hrxn= +74.6 kJ/mol H2(g) + ½ O2(g) ->H2O(l) ∆Hrxn = −285.8 kJ/mol CH4(g) + 2 O2(g) -> CO2(g) + 2 H2O(l) ∆Hrxn = −890.5 kJ/mol 4) Let’s calculate heat of combustion for propane, C3H8, at thermodynamic standard state – first, we need the balanced chemical equation: C3H8(g) + O2(g) -> CO2(g) + H20(l) Use some of the reactions above and the reaction below for the formation of propane (C3H8) to determine the heat of combustion for propane (i.e DH for balanced equation you wrote above). C3H8(g) -> 3 C(s) + 4 H2(g) ΔHrxn = +103.9 kJ/molCombustion: C2H6(g)+O2(g)--->(heat)_____________ do not include heat in your answer
- Calculate the heat of hydrogenation of ethane, C2H4 given the following thermochemical equations: 2 C(graphite) + 3 H2 (g) —> C2H6 (g) ΔHf= - 84.5 kJ/mol 2 C (graphite) + 2 H2 (g) —> C2H4 (g) ΔHf= 52.3 kJ/molCalculate the heat of hydrogenation of ethane, C2H4 given the following thermochemical equations: 2 C(graphite) + 3 H2(g) —> C2H6 (g) ΔHf= - 84.5 kJ/mol 2 C (graphite) + 2 H2(g) —> C2H4 (g) ΔHf= 52.3 kJ/molB2H6(g) + 3O2(g) --> B2O3(s) + 3H2O(g) ΔH = -2035 kJ Calculate the amount of heat released when each of the following amounts of diborane (B2H6) is burned. 1.00 g
- What is the enthalpy of combustion of butane in kJ mol−1? 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(l) A. 4x + 5y − z A. 4 x + 5 y − z , B. 4x + 5y + z B. 4 x + 5 y + z , C. 8x + 10y − 2z C. 8 x + 10 y − 2 z , D. 8x + 5y + 2zFind the heat of reaction and explain what happen to it. Calculate the ∆H of reaction for: C3H8 (g) + 5O2 (g) => 3CO2 (g) + 4H2O (l) The values of ∆H of reaction are as follows:C3H8 (g) = -103.95 kJ/molCO2 (g) = -393.5 kJ/molH2O (g) = -285.8 kJ/mol Topic: Enthalpy of ReactionThe heats of reaction for the following combustion reactions were determined experimentally: C2H4(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(ℓ) ∆H = -1411.1 kJ C2H5OH(ℓ) + 3 O2(g) → 2 CO2(g) + 3 H2O(ℓ) ∆H = -1367.5 kJ Considering the above reactions, what is the heat of reaction for the synthesis of ethanol from ethylene and water: C2H4 + H2O(ℓ) → C2H5OH(ℓ) ∆H = ? Report your answer in units of kJ, but do not include the units in your submitted answer. Include a "+" or "-" sign on your answer.
- The same student wanted to determine the heat of dissolution for potassium chlorate (KClO3, MW: 122.55 g/mol) in water. He measured 10 grams of KClO3 and dissolved it in a calorimeter containing 250 g of water. The temperature drop was 3.5 K. 1. What is qH2O in Joules? A. +146.4 B. -146.4 C. -3661 D. +3661 2. What is qdissolution in Joules? A. +146.4 B. -146.4 C. -3661 D. +3661 3. What is the ΔHdissolution in kilojoules per mole? A. +44.866 B. -44.866 C. +1.794 D. -1.794 4. Is the reaction endothermic or exothermic? A. Endothermic B. Exothermicb) Cyclohexene, C6H10 undergoes hydrogenation to produce cyclohexane, C6H12 according to the equation given below : C6H10 (l) + H2 (g) C6H12 (l) ∆???(C6H10) = -30 kJ/mol ∆???(C6H12) = -3930 kJ/mol i. Calculate the standard enthalpy of hydrogenation, ∆Ho of cyclohexene. ii. Sketch the enthalpy diagram of this reactionAt 1 atm how much heat is required to convert 91.0 g of H2O(s) at −18.0 ∘C to H2O(g) at 153.0 ∘C? Data: ?̂ H2O(s)=2.087 J/g⋅ ∘C Δℎ̂ fus=333.6 J/g ?̂ H2O(l)=4.184 J/g⋅ ∘C Δℎ̂ vap=2257 J/g ?̂ H2O(g)=2.000 J/g⋅ ∘C