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What mass of carbon dioxide will be produced when 15g of octane is burned with 15g of oxygen gas?
To determine the mass of carbon dioxide produced from burning octane (C₈H₁₈) with oxygen (O₂), we first need to look at the balanced combustion reaction: 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O. The molar mass of octane is approximately 114 g/mol, and for oxygen, it's about 32 g/mol. With 15 g of octane, we can calculate the moles of octane, which is about 0.131 moles. This stoichiometry shows that 2 moles of octane produce 16 moles of CO₂, leading to approximately 2.1 grams of CO₂ produced from 15 grams of octane, assuming oxygen is in excess.
How many moles of water will be produced from 1 mole of octane?
9
How many moles of H2O are produced when 0.468 mol of octane is burned?
First write down the BALANCED reaction eq'n. Octane + oxygen = Water + Carbon Dioxide. 2CH3(CH2)6CH3 + 25O2 = 18H2O + 16CO2 The molar ratios are 2:25 :: 18:16 So '2' moles of octane produces 18 moles of water. So by equivlance 0.468 : x :: 2 : 18 Algebraically rearrgange x = (0.468/2) X 18 => x = 0.234 x 18 = > x = 4.212 moles water produces.
What mass of octane must be burned in order to liberate 5340 kilojouls of heat?
To calculate the mass of octane burned, we can use the heat of combustion of octane which is 5470 kJ/mol. First, convert the given energy to kilojoules per mole. Then, use the molar mass of octane to convert moles to grams. This will give you the mass of octane that must be burned.
How many moles of carbon dioxide are produced when 84.4 moles of hexane is burned?
To determine the number of moles of carbon dioxide produced when hexane is burned, we need to consider the balanced chemical equation for the combustion of hexane, which is C6H14 + 19/2 O2 -> 6 CO2 + 7 H2O. From the balanced equation, we can see that for every mole of hexane burned, 6 moles of carbon dioxide are produced. Therefore, if 84.4 moles of hexane is burned, 6 * 84.4 = 506.4 moles of carbon dioxide would be produced.
What mass of carbon dioxide will be produced when 15g of octane is burned with 15g of oxygen gas?
To determine the mass of carbon dioxide produced from burning octane (C₈H₁₈) with oxygen (O₂), we first need to look at the balanced combustion reaction: 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O. The molar mass of octane is approximately 114 g/mol, and for oxygen, it's about 32 g/mol. With 15 g of octane, we can calculate the moles of octane, which is about 0.131 moles. This stoichiometry shows that 2 moles of octane produce 16 moles of CO₂, leading to approximately 2.1 grams of CO₂ produced from 15 grams of octane, assuming oxygen is in excess.
How many moles of water will be produced from 1 mole of octane?
9
How many moles of H2O are produced when 0.468 mol of octane is burned?
First write down the BALANCED reaction eq'n. Octane + oxygen = Water + Carbon Dioxide. 2CH3(CH2)6CH3 + 25O2 = 18H2O + 16CO2 The molar ratios are 2:25 :: 18:16 So '2' moles of octane produces 18 moles of water. So by equivlance 0.468 : x :: 2 : 18 Algebraically rearrgange x = (0.468/2) X 18 => x = 0.234 x 18 = > x = 4.212 moles water produces.
What mass of octane must be burned in order to liberate 5340 kilojouls of heat?
To calculate the mass of octane burned, we can use the heat of combustion of octane which is 5470 kJ/mol. First, convert the given energy to kilojoules per mole. Then, use the molar mass of octane to convert moles to grams. This will give you the mass of octane that must be burned.
How many moles of carbon dioxide are produced when 84.4 moles of hexane is burned?
To determine the number of moles of carbon dioxide produced when hexane is burned, we need to consider the balanced chemical equation for the combustion of hexane, which is C6H14 + 19/2 O2 -> 6 CO2 + 7 H2O. From the balanced equation, we can see that for every mole of hexane burned, 6 moles of carbon dioxide are produced. Therefore, if 84.4 moles of hexane is burned, 6 * 84.4 = 506.4 moles of carbon dioxide would be produced.
How many moles of carbon dioxide are produced when 10.0 moles of propane are burned in excess oxygen on gas grill?
30 moles
What mass of carbon dioxide will be produced in this engine when 15.0 g of octane is burned with 15.0 g of oxygen gas?
The balanced chemical equation for the combustion of octane is: 2 C8H18 + 25 O2 -> 16 CO2 + 18 H2O From the equation, 1 mole of octane produces 16 moles of CO2. Therefore, 15.0 g of octane will produce 15.0 g x (16/114.20) = 2.10 g of CO2 when burned with 15.0 g of oxygen gas.
How many moles are in 95.0 gram of octane?
how many moles are in 95.0 gram of octane?
7. How many moles of water can be produced by burning 325 g of octane (C8H18) in excess oxygen.?
To determine the moles of water produced from burning 325 g of octane (C8H18), we first need the balanced combustion reaction: [ \text{C}8\text{H}{18} + 12.5 \text{O}_2 \rightarrow 8 \text{CO}_2 + 9 \text{H}_2\text{O} ] Next, we calculate the molar mass of octane, which is approximately 114.22 g/mol. Thus, the number of moles of octane in 325 g is: [ \text{moles of C8H18} = \frac{325 \text{ g}}{114.22 \text{ g/mol}} \approx 2.85 \text{ moles} ] From the balanced equation, 1 mole of octane produces 9 moles of water. Therefore, the moles of water produced are: [ 2.85 \text{ moles C8H18} \times 9 \text{ moles H2O/mole C8H18} \approx 25.65 \text{ moles H2O} ] Thus, approximately 25.65 moles of water can be produced.
How many moles of water can be produced by burning 325g of octane in excess oxygen?
Balanced equation: 2C8H18 + 25O2 ==> 16CO2 + 18H2Omoles of octane used: 325 g x 1 mole/114g = 2.85 moles octanemoles H2O produced: 18 moles H2O/2 moles C8H18 x 2.85 moles C8H18 = 25.65 moles H2O
How many moles of carbon and hydrogen are there in 5 moles of octane?
In 5 moles of octane, C8H18, there are 40 moles of carbon atoms (5 moles octane x 8 carbon atoms) and 90 moles of hydrogen atoms (5 moles octane x 18 hydrogen atoms).
How many moles of CO2 are produced when 5.60 mol of ethane are burned in an excess of oxygen?
The balanced equation for the combustion of ethane (C2H6) is: 2C2H6 + 7O2 -> 4CO2 + 6H2O From the equation, for every 2 moles of ethane burned, 4 moles of CO2 are produced. Therefore, if 5.60 mol of ethane are burned, then (5.60 mol / 2 mol ethane) * 4 mol CO2 = 11.2 mol of CO2 are produced.
