ity College-CHM 101 (Section 90) - Spring20 - MARX > Activities and Due Dates > Ch 7 HW O Assignment Score: O Resources Ly Give Up? 50.1% O Hint Check Answer < Question 16 of 28 The combustion of ethane (C,H.) produces carbon dioxide and steam. 2 C,H,(s) +70,(g) → 4 CO,(g) + 6 H, O(g) How many moles of CO, are produced when 5.05 mol of ethane is burned in an excess of oxygen? moles of CO,: mol terms of use contactus help about us carecrs privacy policy MacBook A

Here's a formula for the combustion of ethane: 2 C,H, (g) + 7 O, (g) → 6 H,O (g) + 4 CO2 (g) AH = -5318 kJ/mol a.) How many grams of ethane do I need to burn to generate 50,000 kJ of heat?

Ignition wires heat sample Thermometer Stirrer A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.4059 g sample of 9,10-anthracenedione (C14H30,) is burned completely in a bomb calorimeter. The calorimeter is surounded by 1.116x10³ g of water. During the combustion the temperature increases from 22.76 to 25.09 °C. The heat capacity of water is 4.184 Jgl°c-!. Water The heat capacity of the calorimeter was determined in a previous experiment to be 965.5 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 9,10-anthracenedione based on these data. C14HgO2(s) - 1502(g) 4 H20(1) + 14 CO,(g) - Energy Molar Heat of Combustion = kJ/mol Sample dish Burning sample Steel Insulated outside chamber bomb Combustion (bomb) calorimeter.

The process of flambéing involves pouring liqueur on food for flavor. This addition to desserts adds tons of flavor, (C₂H5OH), which combusts in the presence of immense heat. You may have noticed this in restaurants, chemical equation for the combustion of ethanol as a reference in this assessment. C₂H₂OH (1) +30, (g) 2 CO₂ (g) + 3 H₂0 (g)  Use the graph above to explain if the combustion of ethanol is exothermic or endothermic

Write and balance the reaction for the complete combustion of heptane, C7H16. (Use the lowest possible whole number coefficients. Omit states-of-matter from your answer.)

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The combustion of methane is CH4 + 2O2 → CO2 + 2H2O ΔH = -802 kJ/molHow much heat is produced when 2 moles of methane is burned?Select one:A. -802 kJ B. -2250 kJ C. -1604 kJ D. -401 kJ

The following table is the data a student recorded after completing the Hess' Law Lab (VCL 3-12). 200.0 ml of water was added the measured amount of solid NaOH in a calorimeter. Parameter Reaction 1 Mass NaOH (g) 4.575 25.00 Initial temperature (°C) 30.05 Final temperature (°C) Using all the steps and procedues of this lab, calculate the energy released (kJ/mol) of NaOH in Reaction 1.

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Can you help me solve #4?