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7. A 3.25 g sample of methanol, CH3OH, is combusted in a bomb calorimeter. The temperature...
I 7. A 3.25 g sample of methanol, CH3OH, is combusted in a bomb calorimeter. The temperature of the calorimeter increases by 10.6°C. If the heat capacity of the bomb is 846 JC and it contains 1.000 kg of water, what is the heat evolved per mole of ethanol combusted? (The specific heat capacity of water is 4.184 J/gK) (15 pts.)
A 3.250 g sample of methanol, CH_3OH, is combusted in a bomb calorimeter. The temperature of the calorimeter increases by 12.55 degree C. If the heat capacity of the bomb is 8500 J/degree C and it contains 1.200 kg of water, what is the heat evolved per mole of ethanol combusted? The specific heat capacity of water is 4.184 J/g middot K and the molar mass of methanol is 32.04 g/mol. -1321 kJ -726.4 kJ -621.2 kJ -105.2 kJ -63.01...
A 1.20-g sample of maleic acid (C4H4O4) is burned in a bomb calorimeter and the temperature increases from 24.70 °C to 27.41 °C. The calorimeter contains 1000 g of water and the bomb has a heat capacity of 839 J/°C. The heat capacity of water is 4.184 J g-1°C-1. Based on this experiment, calculate ΔE for the combustion reaction per mole of maleic acid burned.
A 2.50 g sample of ethanol, C2H5OH, was combusted in the presence of excess oxygen in a bomb calorimeter containing 2.00 kg of water. The temperature of the water increased from 22.500oC to 27.845oC. The heat capacity of the calorimeter is 2520 J/oC and the specific heat capacity of water is 4.184 J/goC. Calculate the molar enthalpy of the combustion reaction in kJ/mol
Benzoic acid, C7H6O2, occurs naturally in many berries. A 1.50-g sample of benzoic acid is combusted in a bomb calorimeter. The temperature of the calorimeter increases from 22.50 0C to 31.69 0C. The calorimeter contains 775 g water and has a heat capacity of 893 J/0C. Based on this information, how much energy (in kJ) is released when you metabolize 1.50 g of benzoic acid? The specific heat capacity of water is 4.184 J/(g⋅0C).
A quantity of 1.922 g of methanol (CH3OH) was burned in a constant-volume bomb calorimeter. Consequently, the temperature rose by 5.52°C. If the heat capacity of the bomb plus water was 8.75 kJ / °C, calculate the molar heat of combustion of methanol.
2. 1.487 g of methanol (CH3OH, a liquid at room temperature) is completely combusted at 25 °C in a bomb calorimeter with a heat capacity of 10.22 kJ/°C. The final temperature is found to be 28.291 °C. a. Calculate the standard heat of combustion of CH2OH(D) (ACH ) in kJ/mol at 25 °C. b. Calculate the standard heat of formation of CH3OH() (AFH ) in kJ/mol at 25 °C.
5. (10 points) A 2.20 g sample of fructose (CoH12Os) is burned in a bomb calorimeter containing 1350 g water at an initial temperature of 21.00 °c. After the reaction the temperature of the water is 23.52 °C. The heat capacity of the bomb is 450 J/°C. The specific heat capacity of water is 4.184 J/g. C. Calculate the quantity of heat released per mole of fructose in kJlmol.
A bomb calorimeter has a heat capacity of 675 J/°C and contains 925 g of water. If the combustion of 0.500 mole of a hydrocarbon increases the temperature of the calorimeter from 24.26°C to 53.88°C, determine the enthalpy change per mole of hydrocarbon. The specific heat of water = 4.184 J g-1 °C-1.Just the answerWhat is the enthalpy change when 175 g of C3H8 are burned in excess O2? C3H8(g) + 5 O2(g) ® 3 CO2(g) + 4 H2O(l) DH°...
1.14gm of Octane is combusted in bomb calorimeter, surrounded by 1000g of water. Initial temperature of water is 25C and final temperature is 33C. Heat Capacity of Calorimeter hardware (except for water) is 456 J/C . 2C8H18+25O2 --->16CO2+18H20 a)Calculate heat of solution and heat of calorimeter. b) Calculate net of reaction in KJ c)Determine molar enthalpy of combustion of octane in KJ/mol.