Calculate water equivalence, if the heat capacity of bomb calorimeter is 900

Determine the water equivalent of the bomb calorimeter apparatus which gave the following data in an experiment: GCV of benzoic acid = 6324 cal/g Wt. of benzoic acid taken = 1.364 g Wt. of calorimeter = 1025 g Wt. of calorimeter + water = 3025 g Initial temperature = 11.872 C Final temperature = 14.625 C Cooling correction = 0.015 C Heat from fuses = 22 cals Washing of the bomb on analysis indicate the presence of 3.5 ml of N/10 HNO3 and there is no H2SO4formed.

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

The work done in a Bomb – Calorimeter i

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]

1What is meant by the specific heat capacity of a material?The amount of energy required to raise the temperature of 1 kilogram of the material by 1 degree CelsiusThe amount of energy which is required to change 1 kilogram of the material from a liquid to a gasThe total amount of thermal energy which can be stored by 1 kilogram of the materialThe amount of energy which is required to change 1 kilogram of the material from a solid to a liquid2The specific heat capacity of water is 4200 J/kg °C.  Calculate the amount of energy required to raise the temperature of 500 g of water from 20 to 70 °C.147 kJ105 MJ (105,000,000 J)147 MJ (147,000,000 J)105 kJ3A heater is used to transfer 40 kJ of energy to the thermal store of a 2 kg copper cylinder.  By how much will this cause the temperature of the copper to increase?  The specific heat capacity of copper is 385 J/kg °C.0.05 °C51.9 °C207.8 °C0.21 °C