0.3 g of ethane undergoes combustion at 27°C in a bomb calorimeter. The temperature of calorimeter system (including the water) is found to rise by 0.5°C. The heat evolved during combustion of ethane at constant pressure is ________kJ mol–1.(Nearest integer)[Given : The heat capacity of the calorimeter system is 20 kJ K–1, R = 8.3 JK–1 mol–1.Assume ideal gas behaviour. Atomic mass of C and H are 12 and 1 g mol–1 respectively]

A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100.g of water (see sketch at right).First, a 8.000g tablet of benzoic acid C6H5CO2H is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of /26.454kJg.) The temperature of the water is observed to rise from 11.00°C to 56.81°C over a time of 14.2 minutes.Next, 5.690g of acetylene C2H2 are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 11.00°C to 67.44°C.Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction:A "bomb" calorimeter.→+2C2H2g  5O2g + 4CO2g  2H2OgBe sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits.Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values you calculate may not exactly match published values for this reaction.Is this reaction exothermic, endothermic, or neither? exothermicendothermicneitherIf you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. kJCalculate the reaction enthalpy ΔHrxn per mole of CO2. kJmol

For combustion of ethanol C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l), the amount of heat produced as measured in bomb calormeter, is 1364.47 kJ/mol at 25°C. Assuming all gases are behaving ideally, the enthalpy of combustion ΔCH, for ethanol will be : (R = 8.314 kJ/mol)

10.0 grams of octane are burned in a bomb calorimeter containing 2.00 × 102 g H2O. If the water temperature increases from 25.00°C to 37.00°C, how much energy was released by the system? [SHw = 1.00 cal/(g•°C)]

The molar heat of combustion of compound C is 1,250 kJ mol-1. If I were to burn 0.115moles of this compound in a bomb calorimeter with a reservoir that holds 2.50 dm3ofwater, what would the expected temperature increase be?

2 kg of a coal sample was burnt in a bomb calorimeter. The heat liberated was estimated and found to be 14114 kcal. Calculate the calorific value of the coal sample.a.14114 kcal /kgb.7057 kcal/kgc.7057 cal/gd.14114 cal /g