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13 Dec 2019

Given the following information regarding bond strength, estimate the heat evolved when the 1.0lb of propane undergoes combustion. INCLUDE UNITS and INCLUDE THE SIGN
C-H: 413 kJ/mole C=O: 745 kJ/mole O=O: 498 kJ/mole H-O: 467 kJ/mole C-C: 347 kJ/mol

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Reid Wolff
Reid WolffLv2
17 Dec 2019

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Related questions

Propane is often used as a home fuel in areas where natural gas is not available. When 3.00 grams of propane (C3H8 (g)) are burned in excess oxygen in a bomb calorimeter that has a total heat capacity of 32.7 kJ/K, the temperature of the calorimeter increases by 4.25 K.

a.) Calculate the heat of the calorimeter, qCal. (HINT: Units should be in kJ.)

b.) Calculate, by using the First Law of Thermodynamics, the heat of the reaction, qrxn.

c.) Assuming that ΔE ≈ ΔH, calculate the standard enthalpy of combustion in (i) kilojoules per gram of propane, and (ii) kilojoules per mole of propane.

Please explaine

Use the bond enthalpy data given to estimate the heat released when 6.50 g of oxygen gas reacts with excess hydrogen gas to form ammonia at 25 degree C. Draw Lewis structures of the molecules so that you may determine which bonds are being broken and which bonds are being formed in the reaction.

BE(O=H) = 498.7 kJ/mol

BE(H-H) = 436.4 kJ/mol

BE(O-H) = 460.0 kJ/mol

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