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Ethane, a minority component of natural gas, burns to form carbon dioxide and water according to...
Ethane, a minority component of natural gas, burns to form carbon dioxide and water according to this reaction: 2H3C−CH3(g)+7O2(g)→4CO2(g)+6H2O(g) 2 H 3 C − C H 3 ( g ) + 7 O 2 ( g ) → 4 C O 2 ( g ) + 6 H 2 O ( g ) Note that the average bond energy for the breaking of a bond in CO2 C O 2 is 799 kJ/mol k J / m o l ....
ethane burns in air to form carbon dioxide and water vapor 2H3C-CH3(g)+7O2(g)-->4CO2(g)+6H2O(g) Use average bond energies to calculate delta H rxn for the reaction
The combustion of ethane (C2H6) produces carbon dioxide and steam. 2C2h6(g) + 702(g) → 4CO2(g) + 6H2O(g) How many moles of CO2 are produced when 5.65 mol of ethane is burned in an excess of oxygen? The combustion of ethane (C,H,) produces carbon dioxide and steam. 2C,H, (g) + 702(g) + 4CO2(g) + 6H2O(g) How many moles of Co, are produced when 5.65 mol of ethane is burned in an excess of oxygen? moles of CO,
Ethane is burned in air (oxygen) to form carbon dioxide and water by the following reaction. Determine the maximum grams of carbon dioxide that can be formed if 57.9 g of ethane are reacted with 57.9 g of oxygen. 2 C2H6 + 7 O2 = 4 CO2 + 6H2O.
The combustion of ethane (C2H6) produces carbon dioxide and steam. 2C2H6(g)+7O2(g)⟶4CO2(g)+6H2O(g) How many moles of CO2 are produced when 5.45 mol of ethane is burned in an excess of oxygen? moles of CO2: mol
The combustion of ethane (C2H6) produces carbon dioxide and steam. 2C2H6(g)+7O2(g)⟶4CO2(g)+6H2O(g) How many moles of CO2 are produced when 5.05 mol of ethane is burned in an excess of oxygen?
Review Coristas Petole Table Natural gas burns in air to form carbon dioxide and water releasinghe CH,(s) +0,6) - CO.(a)+H06) AH-812.3. Part A What minimum mass of CH is required to heat 800 g of water by 26.0°C? (Assume 10015 heating efficiency) (For water. = 4.18 J/C) 1745 4,00 x 10' 0.1748 Suomi Rest
0.189 moles of ethane gas are mixed with 2.1 moles of oxygen in a sealed container and the mixture is then ignited (initiating a combustion reaction) to form carbon dioxide and water. 2 C2H6(g) + 702(g) 4CO2(g) + 6H2O(g) What is the volume of CO2 formed when the partial pressure of CO2 is 200 kPa and a temperature of 200 °C? (Assume that all gases behave ideally). (A) (B) (C) (D) (E) 7.4 x 10-3 m3 3.7* 10-3 m3 4.1...
Pentane (C5H12) burns in oxygen to produce carbon dioxide and water via the following reaction: C5H12(g)+8O2(g)) Δ⟶ 5CO2(g)+6H2O(g) Calculate the mass of CO2 that can be produced if the reaction of 36.5 g of pentane and sufficient oxygen has a 65.0 % yield.
When methane (CH4) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction is CH4(g)+O2(g)→CO2(g)+H2O(g) This type of reaction is referred to as a complete combustion reaction. What mass of carbon dioxide is produced from the complete combustion of 4.50×10−3 g of methane? Express your answer with the appropriate units.