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Given,
moles of methanol = 4.50
Temperature = 464 K
Step by step
Solved in 4 steps
- A piece of metal weighing 8.00 g at a temperature of 46.0 oCo was placed in a calorimeter in 38.10 mL of water at 24.3 oC. The final equilibrium temperature was found to be 25.7 oC . What is the specific heat of the metal?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 0.6756 g sample of adipic acid (C6H10O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.097×103 g of water. During the combustion the temperature increases from 28.42 to 30.70 °C. The heat capacity of water is 4.184 J g-1°C-1.The heat capacity of the calorimeter was determined in a previous experiment to be 855.4 J/°C.Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of adipic acid based on these data.C6H10O4(s) + (13/2) O2(g) 5 H2O(l) + 6 CO2(g) + EnergyMolar Heat of Combustion = _______ kJ/molA 3.971 g sample of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and its contents increase from 24.87 ∘C to 28.06 ∘C. The heat capacity (calorimeter constant) of the calorimeter is 36.35 kJ/ ∘C, what is the heat of combustion per gram of the material?
- Part B 2.0000 g of the unknown compound is burned in a bomb calorimeter. During the combustion, the temperature of the calorimeter increases from 23.125°C to 28.997 °C. During calibration, the heat capacity of the calorimeter was found to be 9.9897kJ °C-1. In the previous experiment, the molar mass of the substance was found to be 148.16 gmol-1. What is AcombU for the unknown compound? να ΑΣφ ? kJ mol1 Submit Request AnswerIn this experiment you will place a sample of your salt in water in a constant pressure calorimeter. You will determine the enthalpy change for the dissociation of your salt, Delta Hdiss. A sample of 4.368 grams of the salt SrCl2 was placed in 35.5 g water, the initial temperature was 20.00℃ and the final temperature was 27.086365℃. What is the number of moles of SrCl2? 4.368 g SrCl2 x ( 1 mol SrCl2 / 123.073 g SrCl2 ) = 0.035491131 mol SrCl2 a. 0.035491 mol SrCl2 b. none of these c. 0.035 mol SrCl2 d. 0.03 mol SrCl2 e. 0.0355 mol SrCl2 f. 0.04 mol SrCl2 g. 0.035491131 mol SrCl2 h. 0.03549 mol SrCl2When 0.0901 mol of an unknown hydrocarbon is burned in a bomb calorimeter, the calorimeter increases in temperature by 2.19°C. If the heat capacity of the bomb calorimeter is 1.229 kJ/°C, what is the heat of combustion for the unknown hydrocarbon?
- Suppose 300 mL of 2.00 M HCl and 300 mL of 2.00 M NaOH, both initially at 23.0 celsius, are mixed in a thermos flask. When the reaction is complete, the temperature is 36.6 celsius. Assuming that the solutions have the same heat capacity as pure water, compute the heat released in kJChemistry 14) A 60.0 mL quantity of 0.80 M HCI is mixed with 60.0 mL of 0.80 M KOH in a constant pressure calorimeter with negligible heat capacity. If the initial temperatures of both solutions are equal to 20.24°C. Calculate the heat change of the neutralization reaction if the final temperature of the mixture is 30.0°C. Assume that the densities and specific heats of the solutions are the same as those of water (1.00 g/mL and 4.184 J/g °C, respectively). Note: this point is worth 10 points. A) + 4900.3 J B)-1171.2 J C)-2450.15 J D)-4900.3 J1. The change in internal energy of the combustion of solid naphthalene (C10H8) was determined to be equal to -5151 kJ/mol. Calculate its enthalpy of combustion. 2. What is the change in internal energy of a system if the system evolves 525 J of heat and has 1.25 kJ of work done on it
- A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy available from foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 0.508-g sample of benzil (C14H1002) in a bomb calorimeter containing 1060. g water. The temperature increases from 24.70 °C to 27.80 °C. The specific heat capacity of water is 4.184 J gl°C1. The combustion enthalpy is -6784 k]/mol benzil. C14H1002(s) + 31/2 02(g) →14 CO2(g) + 5 H20(I) A,H° = -6784 kJ/mol %3D Calculate the heat capacity of the calorimeter. heat capacity of calorimeter = J/CA generic solid, X, has a molar mass of 78.678.6 g/mol. In a constant‑pressure calorimeter, 30.730.7 g of X is dissolved in 327327 g of water at 23.00 °CX(s)⟶X(aq)X(s)⟶X(aq) The temperature of the resulting solution rises to 28.5028.50 °C. Assume the solution has the same specific heat as water, 4.184 J/(g·°C), and that there is negligible heat loss to the surroundings. How much heat was absorbed by the solution?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 1.1250 g sample of β-D-fructose (C6H12O6) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.200×103 g of water. During the combustion the temperature increases from 23.58 to 26.40 °C. The heat capacity of water is 4.184 J g-1°C-1.The heat capacity of the calorimeter was determined in a previous experiment to be 979.8 J/°C.Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of β-D-fructose based on these data.C6H12O6(s) + 6O2(g) 6 H2O(l) + 6 CO2(g) + Energy