In a bomb calorimeter (constant volume), 3.5 g of a gas (Molar Mass-28.0g/mol) react with anexcess of oxygen at 298.0 K. After combustion the temperature of the calorimeter increasesfrom 298.0 K to 298.45 K. If the heat capacity of the calorimeter is C=2.5 kJK^-1, calculate theAH of combustion in kimol-1. Assume the total number of moles of the gas doesn't changeduring combustion.

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Answered: In a bomb calorimeter (constant…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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49.85 grams of solid silver carbonate is dissolved in the calorimeter and the temperature goes from 23.15∘C to 10.01∘C g What is the ∆H for the solution process? The heat capacity of calorimeter and its contents is 311J∘C
A researcher studying the nutritional value of a new candy places a 4.60 g4.60 g sample of the candy inside a bomb calorimeter and combusts it in excess oxygen. The observed temperature increase is 2.27 ∘C.2.27 ∘C. If the heat capacity of the calorimeter is 43.90 kJ⋅K−1,43.90 kJ⋅K−1, how many nutritional Calories are there per gram of the candy?
A researcher studying the nutritional value of a new candy places a 5.10 g5.10 g sample of the candy inside a bomb calorimeter and combusts it in excess oxygen. The observed temperature increase is 2.18 ∘C.2.18 ∘C. If the heat capacity of the calorimeter is 42.00 kJ⋅K−1,42.00 kJ⋅K−1, how many nutritional Calories are there per gram of the candy?
When 1.553 g of liquid hexane (C6H14C6H14) undergoes combustion in a bomb calorimeter, the temperature rises from 26.22 ∘C to 38.01 ∘C. Find ΔErxn for the reaction in kJ/mol hexane. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 5.81 kJ/∘C Express your answer using three significant figures.
A bomb calorimetry experiment is performed with xylose, CsH10Os (s), as the combustible substance. The data obtained are: mass of xylose burned: 1.764g; heat capacity of calorimeter: 4.728 kJ/°C; initial calorimeter temperature: 23.29°C; final calorimeter temperature 27.19°C. What is the heat of combustion of xylose, in kilojoules per mole? Lütfen birini seçin: O a.-1.57x10 kJ/mol O b.-5.64x10 kJ/mol O c.-3.17x10 kJ/mol O d -3.34x10 kJ/mol O e. -2.38x10 kJ/mol
A generic solid, X, has a molar mass of 82.3 g/mol. In a constant-pressure calorimeter, 46.1 g of X is dissolved in 337 g of water at 23.00 °C. X(s) - X(aq) The temperature of the resulting solution rises to 29.50 °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? 9.156 kJ Incorrect What is the enthalpy of the reaction? AHrxn 16.35 kJ/mol %D Incorrect
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An electrical heater is used to add 20.00 kJ of heat to a constant-volume calorimeter. The temperature of the calorimeter increases by 4.92°C. When 1.50 g of ethanol (C2H5OH) is burned in the same calorimeter, the temperature increases by 10.96°C. Calculate the molar heat of combustion for ethanol (enter in kJ).
Palmitic acid (C16H32O2) is a major component of the oil from the fruit of oil palms (palm oil). The complete combustion of palmitic acid can be represented as: C16H32O2(s)+23O2(g)→16CO2(g)+16H2O(l) In a bomb calorimeter with a heat capacity of 10.66 kJ⋅∘C−1 0.7081 gg of palmitic acid (molar mass = 256.43 g⋅mol−1) was combusted. The temperature of the calorimeter was observed to rise by 2.580 ∘C. a. Determine the ΔrU for the combustion of palmitic acid. b. Determine the ΔrH (at 298 KK) for the combustion of palmitic acid.
Under constant- volume conditions, the heat of combustion of glucose, C6H12O6, is 15.57 kJ/g. A 3.50 gram sample of glucose is burned in a bomb calorimeter. The temperature of the calorimeter is increased From 20.94°C to 24.72°C.What is the total heat capacity of the calorimeter?
When 0.418 g of pentene, C5H12, is burned in a bomb calorimeter the temperature rises by 4.21 ∘C. The heat capacity of the calorimeter is 2.46 kJ/∘C. Calculate the combustion energy (ΔE) for pentene, C5H12 in kJ/g
If the specific heat capacity of benzene, C6H6, is 1.74 Jg∘CJg∘C, calculate its molar heat capacity. The atomic masses of carbon and hydrogen are: C = 12 g/mol H = 1 g/mol

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