a) Calculate the heat evolve when the ethanol was combusted b) Calculate the enthalpy change of combustion per mole of ethanol

During an exothermic reaction… A) heat released and products are lower in potential energy than reactants  B) heat released and products are higher in potential energy than reactants C) heat absorbed and products are lower in potential energy than reactants D) heat absorbed and products are higher in potential energy than reactants E) no heat transform and products are the same in potential energy with reactants

Which statement about the reaction illustrated in the diagram is true? (B). (A] (C) (D) (E) O The energy required to break the bonds is more than the energy released upon forming new bonds. The energy required to break the bonds is less than the energy released upon forming new bonds. O No heat is required to start the reaction. The reaction is endothermic.

9:17 Question 14.f of 40 In welding, the temperature of the flame produced by the combustion of acetylene and oxygen varies based on the balance of the two gases in the reaction. The heat is used to melt metal so that pieces of metal can be joined together. ..lLTE An oxidizing flame (excess oxygen) is used to cut through metal. The temperature of an oxidizing flame is typically around 6692 °F. What is this temperature in K? Report your answer to four significant figures. K 1 4 7 +/- Tap here or pull up for additional resources 2 3 5 6 8 9 O Submit X x 100

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If 0.24 mols of substance B is able to produce 137J of heat. What is the change in reaction enthalpy in J associated with the following balanced reaction. (Hint: *pay attention the the coefficient for substances B *determine the sign for heat, is it + or -). Round and report your answer to an integer without decimal place including + or- - sign. Only enter numeric value, no unit. A+2B → AB2 + heat AHren =???

The reaction that produces the water gas mixture, described in Question 6.99, is C(s) + H₂O(g) → CO(g) + H₂(g) This reaction requires an input of 131 kJ of heat for every mole of carbon that reacts. (a) Is this reaction endothermic or exothermic? (b) What is the energy change for this reaction in units of kJ/mol of carbon?

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Try Again Your answer is incorrect. • (2): Your answer is incorrect. Combustion of hydrocarbons such as octane (CH₁8) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Earth's atmosphere can trap the Sun's heat, raising the average temperature of the Earth. For this reason there has been a great deal of international discussion about whether to regulate the production of carbon dioxide. 1. Write a balanced chemical equation, including physical state symbols, for the combustion of liquid octane into gaseous carbon dioxide and gaseous water. 2Cg H₁8 (1) + 250₂ (g) , 8 18 16CO₂ (g) + 18H₂O(g) 2 2. Suppose 0.310 kg of octane are burned in air at a pressure of exactly 1 atm and a temperature of 17.0 °C. Calculate the volume of carbon dioxide gas that is produced. Round your answer to 3 significant digits. L ロ→ロ X x10 S

Use the References to access important values if needed for this question Ethanol, C2H0, is most often blended with gasoline - usually as a 10 percent mix - to create a fuel called gasohol. Ethanol is a renewable resource and ethanol-blended fuels, like gasohol, appear to bum more efficiently in internal combustion engines. The combustion enthalpy of ethanol is 1366.9 kJ/mol The combustion enthalpy of 2-methylpentane, C6H14 is 4.157x103 kJ/mol. Calculate the energy released during the complete combustion of 382 g 2-methylpentane kJ Assuming the same efficiency, would 382 g ethanol provide more, less, or the same quantity of energy as 382 g 2-methylpentane? | Submit Answer Retry Entire Group 8 more group attempts remaining