2 C8H18 (l) + 25 O2 (g) ----> 16 CO2 (g) + 18 H2O (g)
(OR 2 C8H18 (l) + 25 O2 (g) right arrow 16 CO2 (g) + 18 H2O (g))
Use the following conversions: 1 mol = MW in g (2 d.p.) = 22.414 L
All gases are at STP. How many liters of CO2 would be produced from the reaction of 5.0 L of C8H18 with 55 L of O2?
Theoretical yield of CO2 from 5.0 L C8H18 = _____________
Theoretical yield of CO2 from 55 L O2 = _____________
Limiting reagent = ____________(C8H18 or O2 or CO2)
2 C8H18 (l) + 25 O2 (g) ----> 16 CO2 (g) + 18 H2O (g)
2 moles of C8H18 react with 25 moles of O2
2*22.414L of C8H18 react with 25 *22.414L of O2
5L of C8H18 react with = 25*22.414*5/(2*22.414) = 62.5L of O2 is required
O2 is limiting reagent
25 moles of O2 react with excess of C8H18 to gives 16 moles of CO2
25*22.414L of O2 react with excess of C8H18 to gives 16*22.414L of CO2
55L of O2 react with excess of C8H18 to gives = 16*22.414*55/(25*22.414) = 35.2L of CO2
Theoretical yield of CO2 from 55 L O2 = 35.2L of CO2 >>>>answer
How many liters of CO2 would be produced from the reaction of 5.0 L of C8H18 with 55 L of O2?
Given the following: 2 C8H18 + 25 O2 ====è 16 CO2 + 18 H2O Find the limiting reagent for making CO2 from 35.4 Moles C8H18 and 145 moles O2. Then find the grams excess reagent left at the end of the reaction
The combustion of octane (C8H18) in oxygen proceeds as follows 2 C8H18(g) + 25 O2(g) ---> 16 CO2 (g) + 18 H2O(l) How many moles of CO2are produced when 5.0 moles of octane, C8H18, is burned in 5.0 moles of oxygen?
The combustion of octane, C8H18, proceeds according to the reaction 2 C8H18(l) + 25 O2(g) --> 16 CO2(g) + 18 H2O(l) If 442 mol of octane combusts, what volume of carbon dioxide is produced at 20.0 ?C and 0.995 atm?
Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with 8.000 moles of O2.2 C8H18 + 25 O2 ? 16 CO2 + 18 H2Oa)12.50%b)25.00%c)20.00%d)50.00%
Use this balanced equation to answer the following stoichiometry problem. 2C3H18(1) + 25 O2(g) →16 CO2(g) + 18 H2O(g) The molar masses in grams are: C8H18 = 114; O2 = 32; CO, = 44; H20 = 18. If you burn 72.9 g of octane, how many liters at STP of CO2 are produced? O 179 L 129 L 83.5L 115L
Combustion of Octane: C8H18 + O2 → CO2 + H2O Question 1: What are the coefficients for the balanced reaction of the combustion of octane? Problem 2: If 20 g of octane combust with 20 g of oxygen, which is the limiting reagent?
How much heat is produced if 22.2 g of octane (C8H18) is combusted according to the following reaction? 2 C8H18 (g) + 25 O2 (g) --> 16 CO2 (g) + 18 H2O (l) ΔH = -5471 kJ/mol
Burning octane is: 2 (C8H18) + 25 (O2) ......... 16 (CO2) + 18 (H2O) How many moles of oxygen would you need to burn 2.37 moles of octane?
Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with 4.000 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O 20.00% 50.00% 25.00% 12.50%
According to the following combustion reaction of gasoline (Octane), how many moles of C8H18 needs to be reacted to produce 16 moles of CO2? C8H18 (l) + 25/2 O2 (g) → 8CO2 (g) + 9 H2O