The heat of combustion of octane is -5430 kJ/mol.
1.000 g sample of octane (C8H18) is burned in a bomb calorimeter at an initial temperature of 25.00ºC.
The heat capacity of the calorimeter (also known as the “calorimeter constant”) is 837 J/ºC.
Calculate E for the combustion of octane. (You will need a balanced chemical equation to find H)
What is the final temperature of the calorimeter?
The heat of combustion of octane is -5430 kJ/mol. 1.000 g sample of octane (C8H18) is...
When a 3.08 g sample of liquid octane (C8H18) is burned in a bomb calorimeter, the temperature of the calorimeter rises by 26.9 oC. The heat capacity of the calorimeter, measured in a separate experiment, is 6.22 kJ/∘C . The calorimeter also contains 3.00 kg of water, specific heat capacity of 4.18 J/g°C. Determine the heat of combustion of octane in units of kJ/mol octane.
When a 3.80-g sample of liquid octane (C8H18) is burned in a bomb calorimeter, the temperature of the calorimeter rises by 26.5 ∘C. The heat capacity of the calorimeter, measured in a separate experiment, is 6.21 kJ/∘C . You may want to reference (Page 265) Section 6.5 while completing this problem. Part A Determine ΔE for octane combustion in units of kJ/mol octane. Express your answer using three significant figures.
The combustion reaction for octane burning in oxygen is: 2 C8H18 (l) + 25 O2(g) → 16 CO2(g) +18 H2O(g) ∆H = -10869 kJ . Suppose an oxygen bomb calorimeter is loaded with oxygen gas and excess octane. The oxygen gas has a volume of 480.0 mL, pressure of 5.67 atm, and an initial temperature of 22.1 °C. The calorimeter has a heat capacity of 1.75 kJ/ °C . Assuming the oxygen reacts completely, what is the final temperature of...
The combustion reaction for octane burning in oxygen is: 2 C8H18 (1) + 25 O2(g) → 16 CO2(g) +18 H20() AH = -10869 kJ . Suppose an oxygen bomb calorimeter is loaded with oxygen gas and excess octane. The oxygen gas has a volume of 480.0 mL, pressure of 6.35 atm, and an initial temperature of 22.1 °C. The calorimeter has a heat capacity of 1.75 kJ/ °C. Assuming the oxygen reacts completely, what is the final temperature of the...
QUESTION 4 The combustion reaction for octane burning in oxygen is: 2 C8H18 ()25 O2(g)- 16 CO2(g) +18 H20(g) AH = -10869 kJ Suppose an oxygen bomb calorimeter is loaded with oxygen gas and excess octane. The oxygen gas has a volume of 480.0 mL, pressure of 8.28 atm, and an initial temperature of 22.1 °C The calorimeter has a heat capacity of 1.75 kJ/ °C Assuming the oxygen reacts completely, what is the final temperature of the calorimeter?
7A) Butane has a heat of combustion of -2882 kJ/mol. If a 10.09 g sample of butane is burned in a bomb calorimeter containing 2.610 kg of water initially at 20.13 degrees C, find the final water temperature. 7B) A sample of ethanol (CH3CH2OH) increases the temperature of the bomb calorimeter in Question 7A by 4.71 degrees C. If the heat of combustion of ethanol is -1407 kJ/mol, what was the mass of the ethanol sample? I only need the...
Butane (C4H10) has a heat of combustion of -2882 kJ/mol. If a 10.09 g sample of butane is burned in a bomb calorimeter containing 2.610 kg of water initially at 20.13 degrees C, find the final water temperature.
1a) Consider the reaction: C12H22O11(s)+12O2(g)→12CO2(g)+11H2O(l) in which 10.0 g of sucrose, C12H22O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/∘C. The temperature increase inside the calorimeter was found to be 22.0 ∘C. What is the heat of this reaction per mole of sucrose? 1b) One tablespoon of peanut butter has a mass of 17.0 g. It is combusted in a calorimeter whose heat capacity is 110 kJ/°C. The temperature of the calorimeter rises from 21.6...
Calculate the heat (in kJ) required to completely vaporize 11.42 g of n-octane, C8H18, if the sample is initially at –20 ºC. Pertinent data are: m.p. = -57 ºC, b.p. = 126 ºC, ΔHfus = 20.65 kJ/mol, ΔHvap = 38.6 kJ/mol, Cp(liq.) = 254 J/K-mol.
At constant volume, the heat of combustion of a particular compound is −3796.0 kJ/mol.−3796.0 kJ/mol. When 1.277 g1.277 g of this compound (molar mass=107.98 g/mol)(molar mass=107.98 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter, including its contents, rose by 4.263 ∘C.4.263 ∘C. What is the heat capacity (calorimeter constant) of the calorimeter?