Complete combustion of methane
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.
Part C
What mass of water is produced from the complete combustion of 8.90x10-3 g of methane?
Express your answer with the appropriate units.
What mass of water is produced from the complete combustion of 8.90x10-3 g of methane?
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.
When methane (CH4CH4) 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)CH4(g)+O2(g)→CO2(g)+H2O(g) This type of reaction is referred to as a complete combustion reaction. Part A What mass of carbon dioxide is produced from the complete combustion of 1.80×10−3 gg of methane? Part B What mass of water is produced from the complete combustion of 1.80×10−3 gg of methane? Part C What mass of oxygen is needed for the...
CH4(g)+O2(g)→CO2(g)+H2O(g) Part A. What coefficients are needed to balance the equation for the complete combustion of methane? Enter the coefficients in the order CH4, O2, CO2, and H2O, respectively. Part B. What mass of carbon dioxide is produced from the complete combustion of 8.30×10−3 g of methane? Part C. What mass of water is produced from the complete combustion of 8.30×10−3 g of methane? Part D. What mass of oxygen is needed for the complete combustion of 8.30×10−3 g of...
Methane (CH4) burns in air to form carbon dioxide and water as shown below. CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) If a sample of methane occupies 426. mL at 2.31 atm, what volume (in mL) of oxygen gas at the same temperature and pressure is required to complete the reaction?
Gaseous methane (CH4) reacts with gaseous oxygen gas (O2) to produce gaseous carbon dioxide (CO2) and gaseous water (H2O). If 0.198 g of water is produced from the reaction of 0.16 g of methane and 0.45 g of oxygen gas, calculate the percent yield of water. Round answer to 2 significant figures.
Balanced equation: CH4(g)+2O2(g)→CO2(g)+2H2O(g) Part B: What mass of carbon dioxide is produced from the complete combustion of 2.70×10−3 g of methane? Part C: What mass of water is produced from the complete combustion of 2.70×10−3 g of methane? PartD: What mass of oxygen is needed for the complete combustion of 2.70×10−3 g of methane?
Gaseous methane (CH4) reacts with gaseous oxygen gas (O2) to produce gaseous carbon dioxide (CO2) and gaseous water (H2O). If 1.08 g of water is produced from the reaction of 0.64 g of methane and 4.7 g of oxygen gas, calculate the percent yield of water. Round your answer to 2 significant figures. 0 % x 6 ?
Part B What mass of carbon dioxide is produced from the complete combustion of 7.10×10−3 g of methane? Express your answer with the appropriate units. Part C What mass of water is produced from the complete combustion of 7.10×10−3 g of methane? Express your answer with the appropriate units. Part D What mass of oxygen is needed for the complete combustion of 7.10×10−3 g of methane? Express your answer with the appropriate units.
Gaseous methane CH4 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O . Is 1.88g of water is produced from the reaction of 0.96g of methane and 7.2g of oxygen gas, calculate the percent yield of water. Round your answer to 2 significant figures.
Gaseous methane CH4 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. If 0.578g of water is produced from the reaction of 0.64g of methane and 1.9g of oxygen gas, calculate the percent yield of water. Be sure your answer has the correct number of significant digits in it.