How much energy is released per gram of hydrogen for the following reaction?
2H2(g) +O2 (g) → 2H2O(g)
a. -483.6 kJ b. -241.8kJ C. -120.9 kJ d. 60.5 kJ e. 241.8 kJ
6. 2H2(g) + O2(g) ---> 2H2O(g)
DH0rxn = (2*-241.82)-(2*0+1*0)
= -483.64 kj
2 mol H2 = 2*2 g water = -483.64 kj
energy released per gram hydrogen = -483.64/4 = -120.91 kj
answer: c. -120.91 kj
How much energy is released per gram of hydrogen for the following reaction?
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all 3. Calculate the heat released (kJ) in the reaction of 1.35L of acetylene (C2H2) and 0.235L of hydrogen gas at STP to form ethane gas as determined by the following equation: C2H2(g) + 2H2() → C2H6(g) Given: 2C2H2(g) +502(g) + 4CO2(g) + 2H20(g) 2C2H.(g) + 702(g) → 4CO2(g) + 6H20(g) 2H2(g) + O2(g) → 2H2O(g) AH = -2320 kJ/mol AH = -3040 kJ/mol AH = -572 kJ/mol
The following thermochemical equation is for the reaction of hydrogen(g) with oxygen(g) to form H2O(g). 2H2(g) + O2(g) 2H2O(g) AH=-484 kJ How many grams of H2(g) would have to react to produce 61.5 kJ of energy? grams
8. Find ∆H◦ of the reaction 2C2H6(g) + 7O2(g) = 4CO2(g) + 6H2O(g), as it is written, given the following: 2C(s) + 3H2(g) = C2H6(g), ∆H◦ = −84.68 kJ, 2H2(g) + O2(g) = 2H2O(g), ∆H◦ = −483.6 kJ, C(s) + O2(g) = CO2(g), ∆H◦ = −393.5 kJ. (A) −3194 kJ (B) −3109 kJ (C) −2940 kJ (D) −2855 kJ (E) −1428 kJ
The following thermochemical equation is for the reaction of hydrogen(g) with oxygen(g) to form water(g). 2H2(g) + O2(g)--2H2O(g) ΔΗ--484 kJ How many grams of H2(B) would have to react to produce 95.6 kJ of energy? grams Submit Answer Retry Entire Group 7 more group attempts remaining
Find ∆H◦ of the reaction 2C2H2(g) + 5O2(g) = 4CO2(g) + 2H2O(g), as it is written, given the following: 2C(s) + H2(g) = C2H2(g), ∆H◦ = +227.4 kJ, 2H2(g) + O2(g) = 2H2O(g), ∆H◦ = −483.6 kJ, C(s) + O2(g) = CO2(g), ∆H◦ = −393.5 kJ.
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