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4 Question 10 How much heat in kJ is produced by the combustion of 155 g...
2. How much heat is produced by the combustion of 10.0 L of ethanol (CHsOH, 46.07 g/mole). Density of ethanol = 0.789 g/mL The combustion reaction is: C2HsOH () 30(8) 2CO(8) 3HOu)AH1366.8 kJ 298 Your answer:k
How much heat is produced by the combustion of 125 g of acetylene (CH)? CH2(g) + O2(b) — 2002(g) +H30() AH* = -1301.1 kJ/mol Select the correct answer below: O 1,62 x 10" k! O -4.81 x 10 O 3.2 x 10° O -6.25 X 10'
The experimentally determined heat of combustion of ethanol is 1233 kJ/mol. Calculate the heat of combustion of ethanol in kJ/g. Molar mass of ethanol C2H5OH = 46 g/mol C2H5OH(g) + 3 O2(g) → 2 CO2 (g) + 3 H2O(l) LaTeX: \DeltaΔH = -1233 kJ/mol
The heat of combustion of substance X (molar mass 260 g/mol) is -3196 kJ/mol. How much heat is released in the combustion of 8 g of X? Include the correct sign for heat of combustion with your answer and enter to 2 decimal places.
The experimentally determined heat of combustion of methane is 50.1 kJ/g. Calculate the heat of combustion of methane in kJ/mol. Molar mass of methane CH4 = 16 g/mol CH4(g) + 2 O2(g) → CO2 (g) + 2 H2O(l)
Resources Hint Check Answer Question 8 of 10 > How much heat energy is required to convert 70.9 g of solid ethanol at-114.5 °C to gasesous ethanol at 175.0°C? The molar heat of fusion of ethanol is 4.60 kJ/mol, and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of -114.5°C and a normal boiling point of 78.4°C. The specific heat capacity of liquid ethanol is 2.453/g • °C, and that of gaseous ethanol is...
How much heat energy is required to convert 15.0 g of solid ethanol at -114.5 °C to gasesous ethanol at 143.1 °C? The molar heat of fusion of ethanol is 4.60 kJ/mol and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of -114.5 °C and a normal boiling point of 78.4 °C. The specific heat capacity of liquid ethanol is 2.45 J/g·°C and that of gaseous ethanol is 1.43 J/g·°C. How much heat energy...
Question1: Question2: Determine the amount of heat energy (in kJ) needed to warm a 58.5 g sample of ethanol (C2H5OH) from -150°C to 55°C. CH,OH 46.07 g/mol A Hape 38.56 kJ/mol AHIUS 4.90 kJ/mol Boiling 78.5°C Freezing Point -117.3°C Specific Heat Capacity (c) of solid 0.249 J/g.°C Specific Heat Capacity (c) of liquid 2.44 J/g.°C Specific Heat Capacity (c) of gas 1.70 J/g.°C Determine the mass (in grams) of N, that will dissolve in 155 Lof water that is in...
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)...
Answer it plz 4. Determine the theoretical AH°rxn: The theoretical heat of combustion of ethanol (AH®rxn) can be calculated using the standard molar heat of formations from the thermochemical equation. CH3CH2OH (C) + 3 O2(g) → 2 CO2 (g) + 3 H2O(g) AHørxn = ? rxn ΔΗ, - ZnAH"prod) Z(MAH react) AHP (H20 (g)) = -241.83 kJ/mol: AH (CO2(g)) = -393.51 kJ/mol; AH(CH3CH2OH (e)) = -277.0 kJ/mol; and recall that AHF of element = 0