A sample of 2.22 moles of ethanol (C2H5OH) is initially at 25.0°C. If the sample absorbs...
A sample of 2.22 moles of ethanol (C2H5OH) is initially at 25.0°C. If the sample absorbs 5.94 kJ of heat, what is the final temperature of the ethanol? The specific heat capacity of ethanol is 2.46 J/g°C.
Select one:
a. 48.6°C
b. 1120°C
c. 26.1°C
d. 25.0°C
e. None of the above
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A sample of 2.22 moles of ethanol (C2H5OH) is initially at
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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.
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A solution is made by mixing 223.0 mL of ethanol initially at15.3 ∘C with 223.0 mL...
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A solution is made by mixing 285.0 mL of ethanol initially at 11.7 C with 285.0...
A solution is made by mixing 285.0 mL of ethanol initially at 11.7 C with 285.0 mL of water initially at 21.9 °C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL and the density of water is 1.00 g/mL. The specific heat of ethanol is 2.46 J/g.°C and the specific heat of water is 4.184 J/g °C. Ti = "C The specific heat capacities for several substances...
A solution is made by mixing 285.0 ml. of ethanol initially at 11.7°C with 285.0 ml....
A solution is made by mixing 285.0 ml. of ethanol initially at 11.7°C with 285.0 ml. of water initially at 21.9 °C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL. and the density of water is 1.00 g/ml. The specific heat of ethanol is 2.46 Jig:"C and the specific heat of water is 4.184 J/g:°C. Ti = 30.7 "C Incorrect
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.
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...
QUESTION 3 How much heat (in kJ) is required to raise the temperature of 122 g of ethanol (mw 46.07) from 11.29 °C to its boiling point of 78.37 °C and then vaporize it completely creating ethanol gas at the boiling temperature? (specific heat - 2.46 J/g°C, AHyap = 48.6 kJ/mol) QUESTION 4 What is the change in enthalpy (in kJ) when 40.1 g of ethanol (mw-46.07) is condensed at its boiling temperature? (specific heat 2.46 J/g°C, AHvap 48.6 kJ/mol)...
A solution is made by mixing 285.0 mL of ethanol initially at 11.7 C with 285.0 mL of water initially at 21.9 °C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL and the density of water is 1.00 g/mL. The specific heat of ethanol is 2.46 J/g.°C and the specific heat of water is 4.184 J/g °C. Ti = "C The specific heat capacities for several substances...
A solution is made by mixing 285.0 ml. of ethanol initially at 11.7°C with 285.0 ml. of water initially at 21.9 °C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL. and the density of water is 1.00 g/ml. The specific heat of ethanol is 2.46 Jig:"C and the specific heat of water is 4.184 J/g:°C. Ti = 30.7 "C Incorrect
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