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Predict the output of energy as heat from the combustion of 1.0 dm3 of octane at 298 K and 1 bar. Its mass density is 0.703 g cm−3.
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- Predict the output of energy as heat from the combustion of 1.0 dm3 of octane at 298 K and 1 bar. Its mass density is 0.703 g cm−3 ?molar enthalpy of formation of H2O(l) from its elements in their standard states (25 oC and 100 kPa)?Express the standard enthalpy of the reaction in 4 sig figs and include the appropriate units.
- Calculate ΔrH⦵ and ΔrU⦵ at 298 K and ΔrH⦵ at 427 K for the hydrogenation of ethyne (acetylene) to ethene (ethylene) from the enthalpy of combustion and heat capacity data in Tables 2C.3 and 2C.4 of the Resource section. Assume the heat capacities to be constant over the temperature range involved.What is the standard enthalpy of formation of the decomposition of one mole of liquid sulfuric acid to steam, oxygen, and sulfur dioxide gas?Three cubic meters of a 1.5 molar aqueous sulfuric acid solution (SG=1.064) is stored at 25∘C. Determine the standard heat of formation of the solution in kJ/mol H2SO4 relative to the solute elements and water, as well as the total enthalpy of the solution relative to the same reference conditions.
- In the calibration step of a thermochemistry experiment, a current of 124 mA, from a 24.0 V source was allowed to flow through the electrical heater for 219 s and was found to result in an increase in the temperature of the calorimeter and its contents of +1.39 K. Given that the energy supplied by an electrical circuit is the voltage multiplied by the current, multiplied by the time, what is the heat capacity of the calorimeter and its contents? Answer: 469 J K-1Estimate the standard internal energy of formation of liquid methyl ethanoate, CH3COOCH3, at 298 K from its standard enthalpy of formation, which is -442 kJ mol-1.Describe how to find the relationshipbetween the state properties (P, V, T ) of agas and its molar mass or density.
- What is the standard enthalpy of isomerization (kJ/mol) of propanol to isopropanol in the liquid state?Benzoic acid of mass 1.40 g is reacted with oxygen in a constant volume calorimeter to form H2O(l) and CO2(g) at 298 K. The mass of the water in the inner bath is 1.40×103g. The temperature of the calorimeter and its contents rises 2.84 K as a result of this reaction. Part A Calculate the calorimeter constant. The standard enthalpy of combustion of benzoic acid at 298 K is −3227 kJ⋅mol−1. CP,m(H2O,l)=75.3J⋅mol−1⋅K−1.Derive an expression for the heat capacity at constant pressure Cp in terms of thermodynamic variables (N,V,P,T) by differentiating the enthalpy with respect to the temperature. How does Cp vary during free expansion of the ideal gas?