Calculate the amount of heat (in kilojoules) required to vaporize 2.24 kgkg of water at its boiling point. (ΔHvap=40.7 kJ/molΔHvap=40.7 kJ/mol at 100∘C.∘C.)Express your answer to three significant figures and include the appropriate units.

C₂H1002 A chemist carefully measures the amount of heat needed to raise the temperature of a 291.0 mg sample of CoH10O2 from 54.8 °C to 65.7 °C. The experiment shows that 5.41 J of heat are needed. What can the chemist report for the molar heat capacity of CoH10O2? Be sure your answer has the correct number of significant digits. -1 ₁ J-mol K x10

thermometer insulated container water A 57.9 g sample of quartz, which has a specific heat capacity of 0.730 J-g¹c¹, is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The temperature of the water starts off at 21.0 °C. When the temperature of the water stops changing it's 23.3 °C. The pressure remains constant at 1 atm. Calculate the initial temperature of the quartz sample. Be sure your answer is rounded to the correct number of significant digits. sample 0°C a calorimeter

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 0.7090 g sample of adipic acid (C6H1004) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.201×10° g of water. During the combustion the temperature increases from 22.33 to 24.58 °C. The heat capacity of water is 4.184 J gloc!. The heat capacity of the calorimeter was determined in a previous experiment to be 799.0 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of adipic acid based on these data. CGH1004(s) + (13/2) O2(g) → 5 H,O(1) + 6 CO2(g) + Energy Molar Heat of Combustion = kJ/mol

(Hess’s Law) Determine the heat of formation ΔH0f (in kJ/mol) of liquid hydrogenperoxide (H2O2) at 25°C from the following thermochemical equations.H2(g) + ½O2(g) → H2O(g) ΔH0 = -241.82 kJ/mol2H(g) + O(g) → H2O(g) ΔH0 = -926.92 kJ/mol2H(g) + 2O(g) → H2O2(g) ΔH0 = -1070.60 kJ/mol2O(g) → O2(g) ΔH0 = -498.34 kJ/molH2O2(l) → H2O2(g) ΔH0 = 51.46 kJ/mol

Diethyl ether, used as a solvent for extraction of organic compounds from aqueous solutions, has a high vapor pressure which makes it a potential fire hazard in laboratories in which it is used. How much energy is released when 315.0 g is cooled from 153.0°C to 0.0°C? boiling point: 34.5°C Heat of vaporization: 351 J/g Specific heat capacity, (CH3)2O(l): 3.74 J/(g·K) Specific heat capacity, (CH3)2O(g): 2.35 J/(g·K) 145 kJ 158 kJ 116 kJ 63.1 kJ 21.1 kJ

A 34.3 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter containing a certain mass of water.  If the temperature rose from 35.0 to 76.7°C, how much water, in kg, must the bomb calorimeter have contained?  The molar mass of ethanol is 46.07 g/mol.  Assume that the calorimeter doesn't absorb any heat.  The specific heat of water is 4.184 J/g °C.  C2H5OH(l) + 3 O2(g)  →  2 CO2(g) + 3 H2O(g)     ΔH°rxn = -1.24 x 103 kJ/mol

A 33.4 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter containing a certain mass of water.  If the temperature rose from 35.0 to 74.8°C, how much water, in kg, must the bomb calorimeter have contained?  The molar mass of ethanol is 46.07 g/mol.  Assume that the calorimeter doesn't absorb any heat.  The specific heat of water is 4.184 J/g °C.  C2H5OH(l) + 3 O2(g)  →  2 CO2(g) + 3 H2O(g)     ΔH°rxn = -1.24 x 103 kJ/mol

thermometer. A sample of aluminum, which has a specific heat capacity of 0.897 J·g *.°C*, is put into a calorimeter (see sketch at right) that insulated container contains 100.0 g of water. The aluminum sample starts off at 91.4 °C and the temperature of the water starts off at 19.0 °C. When the temperature of the water stops changing it's 26.9 °C. The pressure remains constant at 1 atm. water Calculate the mass of the aluminum sample. Be sure your answer is rounded to 2 significant digits. sample a calorimeter x10

A 36.7 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter containing a certain mass of water. If the temperature rose from 35.0 to 75.2°C, how much water, in kg, must the bomb calorimeter have contained? The molar mass of ethanol is 46.07 g/mol. Assume that the calorimeter doesn't absorb any heat. The specific heat of water is 4.184 J/g °C. C2H5OH() + 3 O2(g) → 2 CO2(s) +3 H20(g) AH°rxn 1.24 x 103 kJ/mol Please do not include units in your answer. Assume all numbers have at least 3 sig figs.