If 4.290 g of ethanol C2H5OH(l) is burned completely in a bomb calorimeter at 298.15 K,...
If 4.290 g of ethanol C2H5OH(l) is burned completely in a bomb calorimeter at 298.15 K, the heat produced is 124.34 kJ .
Part A
Calculate ΔH∘c for ethanol at 298.15 K.
Part B
Calculate ΔH∘f of ethanol at 298.15 K. The enthalpies of formation of CO2(g) and H2O(l) are −393.5 and −285.8 kJ⋅mol-1, respectively.
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If 4.290 g of ethanol C2H5OH(l) is burned
completely in a bomb calorimeter at 298.15 K,...
4.20 If 3.365 g of ethanol C_2H_5OH(l) is burned completely in a bomb calorimeter at 298.15...
4.20
If 3.365 g of ethanol C_2H_5OH(l) is burned completely in a bomb calorimeter at 298.15 K, the heat produced is 99.472 kJ. a. Calculate Delta H degree_ for ethanol at 298.15 K. b. Calculate Delta H degree_ of ethanol at 298.15 K. From the following data, calculate Delta H degree_ for the reaction CH_3COOH(g) rightarrow 2 H_2O(g) + 2 CO_2(g): Delta H degree _g (kJ mol^-1) CH_3COOH(l) + 2 O_2(g) rightarrow 2 H_2O(l) + 2 CO_2(g) -871.5 H_3O(l) rightarrow...
A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the...
A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature rose from 35.0 to 76.0°C and the heat capacity of the calorimeter is 23.3 kJ/°C, what is the value of DH°rxn? The molar mass of ethanol is 46.07 g/mol. C2H5OH(l) + O2(g) → CO2(g) + H2O(g) ΔH°rxn = ? (Points : 1) -1.24 × 103 kJ/mol +1.24 × 103 kJ/mol -8.09 × 103 kJ/mol -9.55 × 103 kJ/mol...
A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the...
A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature rose from 35.0 to 76.0°C and the heat capacity of the calorimeter is 23.3 kJ/°C, what is the value of DH°rxn? The molar mass of ethanol is 46.07 g/mol. C2H5OH(l) + O2(g) → CO2(g) + H2O(g) ΔH°rxn = ? (Points : 1) -1.24 × 103 kJ/mol +1.24 × 103 kJ/mol -8.09 × 103 kJ/mol -9.55 × 103 kJ/mol...
A 2.11 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity, C-5.65 kJ/"C. C2H5OH() + 3 O2...
A 2.11 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity, C-5.65 kJ/"C. C2H5OH() + 3 O2(g) + 2 CO2(g) + 3 H2O(g) AH'rxn=-1235 kJ If the initial temperature is 25.0°C, what is the final temperature (in "C) of the calorimeter? The molar mass of ethanol is 46.07 g/mol. Remember, in the heat equation, q=m's'AT, heat capacity is equivalent to Cum's, giving Heat capacity is extensive whereas specific heat is intensive. -CAT.
A sample of liquid methanol weighing 5.27 g was burned in a bomb calorimeter at 25°C,...
A sample of liquid methanol weighing 5.27 g was burned in a bomb calorimeter at 25°C, and 119.50kJ of heat was evolved. a. Calculate AHº for the combustion of 1 mole of methanol. b. Calculate A/Hºof liquid methanol. A Hºof CO2(g), H2O(g) and H20 (1) are -393.5 kJ/mol, 241.8 kJ/mol, -285.8 kJ/mol, respectively (10 pt)
With a good explanation please. An amount of 3.355 g ethanol C2H5OH(1) is burned completely in...
With a good explanation please.
An amount of 3.355 g ethanol C2H5OH(1) is burned completely in a calorimeter at 298.15 K. The heat produced is 99.472 kJ. It can be assumed that the measurement takes place under constant pressure of 1 bar. C2H5OH(1) + 302(g) + 2CO2(g) + 3H2O(1) 3a. (10 points) Calculate the standard enthalpy of reaction AHR based on the calorimeter mea- surement.
A 12.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity of 5.65 kJ/�C. Using the inform...
A 12.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity of 5.65 kJ/�C. Using the information below, determine the final temperature of the calorimeter if the initial temperature is 25.0�C. The molar mass of ethanol is 46.07 g/mol.
QUESTION 4 0.5 points Save Answer A 6.32 g sample of ethanol (C2H5OH) is burned in...
QUESTION 4 0.5 points Save Answer A 6.32 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity, C = 5.65 kJ/°C. C2H5OH() + 3 O2(g) 2 CO2(g) + 3 H2O(g) AH®rxn = -1235 kJ If the initial temperature is 25.0°C, what is the final temperature (in °C) of the calorimeter? The molar mass of ethanol is 46.07 g/mol. Remember, in the heat equation, q = m*s*AT, heat capacity is equivalent to C= m*s, giving...
Combustion of 2.5000 g of propane (C3H8) releases 115.75 kJ of heat when it is burned...
Combustion of 2.5000 g of propane (C3H8) releases 115.75 kJ of heat when it is burned to form CO2 (g) and H2O (l). The standard formation enthalpies of CO2 (g) and H2O (l) are -393.5 kJ/mol and -285.5 kJ/mol respectively. Calculate the Hrxn for the combustion of propane in kJ/mol Calculate ∆?? ? for propane
A 0.539-g sample of quinizarin (C14H8O4) is burned in a bomb calorimeter and the temperature increases...
A 0.539-g sample of quinizarin (C14H8O4) is burned in a bomb calorimeter and the temperature increases from 24.70 °C to 27.00 °C. The calorimeter contains 1.19×103 g of water and the bomb has a heat capacity of 912 J/°C. Based on this experiment, calculate ΔE for the combustion reaction per mole of quinizarin burned (kJ/mol). C14H8O4(s) + 14 O2(g) 14 CO2(g) + 4 H2O(l) E = kJ/mol
4.20
If 3.365 g of ethanol C_2H_5OH(l) is burned completely in a bomb calorimeter at 298.15 K, the heat produced is 99.472 kJ. a. Calculate Delta H degree_ for ethanol at 298.15 K. b. Calculate Delta H degree_ of ethanol at 298.15 K. From the following data, calculate Delta H degree_ for the reaction CH_3COOH(g) rightarrow 2 H_2O(g) + 2 CO_2(g): Delta H degree _g (kJ mol^-1) CH_3COOH(l) + 2 O_2(g) rightarrow 2 H_2O(l) + 2 CO_2(g) -871.5 H_3O(l) rightarrow...
A 2.11 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity, C-5.65 kJ/"C. C2H5OH() + 3 O2(g) + 2 CO2(g) + 3 H2O(g) AH'rxn=-1235 kJ If the initial temperature is 25.0°C, what is the final temperature (in "C) of the calorimeter? The molar mass of ethanol is 46.07 g/mol. Remember, in the heat equation, q=m's'AT, heat capacity is equivalent to Cum's, giving Heat capacity is extensive whereas specific heat is intensive. -CAT.
A sample of liquid methanol weighing 5.27 g was burned in a bomb calorimeter at 25°C, and 119.50kJ of heat was evolved. a. Calculate AHº for the combustion of 1 mole of methanol. b. Calculate A/Hºof liquid methanol. A Hºof CO2(g), H2O(g) and H20 (1) are -393.5 kJ/mol, 241.8 kJ/mol, -285.8 kJ/mol, respectively (10 pt)
With a good explanation please.
An amount of 3.355 g ethanol C2H5OH(1) is burned completely in a calorimeter at 298.15 K. The heat produced is 99.472 kJ. It can be assumed that the measurement takes place under constant pressure of 1 bar. C2H5OH(1) + 302(g) + 2CO2(g) + 3H2O(1) 3a. (10 points) Calculate the standard enthalpy of reaction AHR based on the calorimeter mea- surement.
QUESTION 4 0.5 points Save Answer A 6.32 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity, C = 5.65 kJ/°C. C2H5OH() + 3 O2(g) 2 CO2(g) + 3 H2O(g) AH®rxn = -1235 kJ If the initial temperature is 25.0°C, what is the final temperature (in °C) of the calorimeter? The molar mass of ethanol is 46.07 g/mol. Remember, in the heat equation, q = m*s*AT, heat capacity is equivalent to C= m*s, giving...
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