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The calculator estimates the cost and CO2 emissions for each fuel to deliver 100,000 BTU's of heat to your house. If 1 mol of acetylene produces -1301.1 kJ, then 4.8 mol of acetylene produces: \(\begin{array}{l}{\rm{ = 1301}}{\rm{.1 \times 4}}{\rm{.8 }}\\{\rm{ = 6245}}{\rm{.28 kJ }}\\{\rm{ = 6}}{\rm{.25 kJ}}\end{array}\). Explain why this is clearly an incorrect answer. the the bond enthalpies of the bonds broken. For example, C2H2(g) + 5 2O2(g) 2CO2(g) +H2O (l) You calculate H c from standard enthalpies of formation: H o c = H f (p) H f (r) The next step is to look Since the enthalpy change for a given reaction is proportional to the amounts of substances involved, it may be reported on that basis (i.e., as the H for specific amounts of reactants). \[\begin{align} 2C_2H_2(g) + 5O_2(g) \rightarrow 4CO_2(g) + 2H_2O(l) \; \; \; \; \; \; & \Delta H_{comb} =-2600kJ \nonumber \\ C(s) + O_2(g) \rightarrow CO_2(g) \; \; \; \; \; \; \; \; \; \; \; \; \; \; \; \; \; \; \; \; \; & \Delta H_{comb}= -393kJ \nonumber \\ 2H_2(g) + O_2 \rightarrow 2H_2O(l) \; \; \; \; \; \; \; \; \; \; \; \;\; \; \; \; \; \; & \Delta H_{comb} = -572kJ \end{align}\]. If the direction of a chemical equation is reversed, the arithmetic sign of its H is changed (a process that is endothermic in one direction is exothermic in the opposite direction). Method 1 Calculating Heat of Combustion Experimentally Download Article 1 Position the standing rod vertically. How graphite is more stable than a diamond rather than diamond liberate more amount of energy. (c) Calculate the heat of combustion of 1 mole of liquid methanol to H2O(g) and CO2(g). Thanks to all authors for creating a page that has been read 135,840 times. These values are especially useful for computing or predicting enthalpy changes for chemical reactions that are impractical or dangerous to carry out, or for processes for which it is difficult to make measurements. an endothermic reaction. For example, the enthalpy of combustion of ethanol, 1366.8 kJ/mol, is the amount of heat produced when one mole of ethanol undergoes complete combustion at 25 C and 1 atmosphere pressure, yielding products also at 25 C and 1 atm.
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