Propane, a component in natural gas, can be used as a fuel in combustion reactions. What is the maximum amount of work (in kJ) that could be supplied by the following reaction under the given conditions at 319 K?
C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (g)
where ΔHorxn = -2045 kJ, ΔSorxn = 103 J/K, and [C3H8] = 1.13 M, [O2] = 11.15 M, [CO2] = 7.35 M, and [H2O] = 1.49 M.
Propane, a component in natural gas, can be used as a fuel in combustion reactions. What...
12. Methane, a major component in natural gas, can be used as a fuel in combustion reactions (proposed by oil tycoon T. Boone Pickens in an add campaign this past year). What is the maximum amount of work (in kJ) that could be supplied by following reaction under the given conditions at 298 K? CH4 (g) + 2 O2(g) Æ CO2 (g) + 2 H2O (g) where ΔHo rxn = -803 kJ and ΔSo rxn = -4.00 J/K and PCH4...
The combustion of propane gas (C3H8) is used to fuel barbeque grills. In order to produce 5.65 moles of water how many moles of oxygen gas are needed? C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l
12. Propane (C3H8) is used as a fuel in many gas grills. The balanced equation for the combustion of C3Hg is shown in Equation 10. C3H8(g) +502(g) + 3 CO2(g) + 4H2O(g) + energy (Eq. 10) (a) How many grams of CO2 could possibly be produced if 10.0 g of CzHg reacts with an ample supply of Oz? (b) How many grams of CO2 could possibly be produced with an ample supply of C3Hg, but only 10.0 g of O2?...
Using the following equation for the combustion of propane, calculate the amount of propane consumed if the reaction gave off 333 kJ heat. C3H8(g) + 5 O2(g) --> 3 CO2(g) + 4 H2O(g) ΔH = -2044 kJ
Calculate the standard enthalpy of reaction for the combustion of propane. NOTE: This equation is not balanced. Round to the nearest whole number. C3H8(g) + O2 --> CO2(g) + H2O(l) kJ/mol Compound Hf (kJ/mole) C3H8(g) -105 CO2(g) -394 H2O(l) -284
Problem: Bapco needs to burn natural-gas fuel that contains 75 mol% methane, 15 mol% ethane, and 10 mol% nitrogen. The following two reactions takes place: CH4(g) 20209) CO2(0) 2H2o) C2H6 (g) + 3.502(g) 2C02(g)3H20 (g) a) What is the standard heat of combustion (kJ/mol) of the fuel at 25 oC with water(g) as a product b) The fuel is supplied to a furnace with 60% excess air, both entering at 250C. The products leave at 600°C. If the combustion is...
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?
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
The combustion of propane is given by the following reaction. C3H8 + 5 O2 → 3 CO2 + 4 H2O The enthalpy of reaction is −2202.0 kJ/mol. How much energy (in kilojoules) will be released if 23.55 grams of propane is burned. (Molar mass of propane = 44.11 g/mol). kJ
The propane fuel (C3H8) used in gas barbeques burns according to this thermochemical equation. If a pork roast must absorb 1.5×103 kJ to fully cook, and if only 15 % of the heat produced by the barbeque is actually absorbed by the roast, what mass of CO2 is emitted into the atmosphere during the grilling of the pork roast?