The thermochemical equation for the combustion of
ethanol is:
C2H5OH (l) + 3 O2 (g) -> 2 CO2 (g) + 3 H2O (g) ΔHrxn = -1360 kJ
What is the enthalpy change when 3.50 kg of ethanol react with excess oxygen?
The thermochemical equation for the combustion of ethanol is: C2H5OH (l) + 3 O2 (g) ->...
The thermochemical equation for the combustion of ethanol is: 5. C2H&OH (I)+3 O2 (g) 2 CO2 (g)+3 H2O (g) AH-1360 kJ What is the enthalpy change when 3.50 kg of ethanol react with excess oxygen?
The thermochemical equation for the combustion of propane is: C3H8 (g) + 5 O2 (g) 3 CO2 (g) + 4 H2O (l) H = -2220 kJ What is the enthalpy change when 35.0 g of propane react?
The thermochemical equation of combustion of methane is: CH4(g) + 2O2(g) → CO2(g) + 2 H2O(l) ΔΗ =-890.3 kJ 1. Calculate the AH when 5.00 g CH4 react with excess of oxygen. 2. Calculate AH when 2L CH4 at 49 °C and 782 mmHg react with an excess of oxygen 3. Calculate AH when 2L CH4 react with L O2 in a reaction vessel kept at 49 °C and 782 mmHg.
Measuring Heat of Reaction Problems 5. A sample of ethanol (C2H5OH), weighing 6.83 g underwent combustion in a bomb calorimeter by the following reaction: 02 (g) 2 CO2 (g)3 H2O () C2H5OH ()3 If the heat capacity of the calorimeter and contents was 18.1 kJ/°C and the temperature of the calorimeter rose from 25.50 to 36.73, (1) what is the AH of the reaction? Using the definitions at the beginning of the module describe (2) the calorimeter + contents, (3)...
Using the balanced equation for the combustion of ethanol, answer the following question. C2H6O(l) + 3 O2(g) → 2 CO2(g) + 3 H2O (g) How many grams of O2 are needed to react with 0.28 mol of ethanol?
Question 3 Propane (C3H8) undergoes combustion according to the following thermochemical equation: C3H8(g) + 5 O2(g) -- 3 CO2(g) + 4H2O(g) Arxn = -2043.0 kJ Substance Heat of Formation (kJ/mol) CO2(g) -393.5 H2O(g) -241.8 O2(g) 0 C3H8(g) ? Calculate the standard enthalpy of formation of propane C3H8 a. -104.7 kJ/mol ob. +1407.7 kJ/mol C. -1407.7 kJ/mol O d. +104.7 kJ/mol o e. -4190.7 kJ/mol
Calculate DG0rxn for the combustion of ethanol C2H5OH(g), at 750°C using the following data: C2H5OH(g) + O2(g) → CO2(g) + H2O(g) ∆G0f (C2H5OH(g)) = -167.9 kJ/mol, ∆G0f (02(g)) = 0 kJ/mol, ∆G0f (CO2(g)) = -394.4 kJ/mol, ∆G0f (H2O(g)) = -228
The thermochemical equation for the burning of ethyl alcohol is C2H5OH(l) + 3O2(g) --> 2CO2(g) + 3H2O(l) ΔH = -1,367 kJ What is the enthalpy change (in kJ) for burning 10.01 g of ethyl alcohol?
Using the balanced equation for the combustion of ethanol, answer the following question. C2H6O(l) + 3 O2(g) → 2 CO2(g) + 3 H2O (g) ethanol How many grams of O2 are needed to react with 0.19 mol of ethanol?
A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction is C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l) The bomb had a heat capacity of 500 J/K, and the calorimeter contained 610 g of water. Burning 4.50 g of ethanol, C2H5OH(L) resulted in a rise in temperature from 16.5 °C to 20.9 °C. Calculate the enthalpy of combustion of ethanol, in kJ/mol. (The specific heat capacity of liquid water is 4.184...