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How many liters of water can be made from 5 L of oxygen gas and an excess of hydrogen?
55 grams O2 × (1 mol O2 ÷ 32 g O2) × (2 mol H2O ÷ 1 mol O2) × (22.4 L ÷ 1 mol H2O) = 77 L H2O(g)In the liquid form, it works out to just under 62 milliliters.
Calculate the number of atoms of O contained in 16.0 pounds of O?
16.0 lbs = 7,257 g of O2 Oxygen exists in the gas form as 02 7,257g O2 * 1 mol O2/ 32 g * 2 mol O / 1 mol O2 * 6.022x10^23 atoms/mol = 2.73E26 atoms of O
The number of moles of h2o formed when 1 mole of o2 reacts with c5h12 in the reaction c5h12 plus 8o2 equals 5co2 plus 6h2o is?
C5H12 + 8 O2 --> 5 CO2 + 6 H2O (1 mol O2)(6 mol H2O/8 mol O2) = 0.75 mol H2O
How many grams of H2O will be produced from 32.0 grams of O2?
Start with the balanced equation of the formation of water:2 H2 + O2 --> 2 H2OIt takes one mole of oxygen to produce 2 moles of water.32.0 g O2 * (1 mol O2/32.00 g O2) * (2 mol H2O/1 mol O2) * (18.02 g H2O/1 mol H2O) = 36.04 gTherefore, about 36.04 grams of water will be produced from 32.0 grams of oxygen gas, assuming that it can react with unlimited amounts of hydrogen gas.
How many moles O2 must react with excess H2 to form 7.89 mol H2O?
Oxygen limits the reaction, so......Balanced equation. 2H2 + O2 -> 2H2O 7.89 mole H2O (1 mole O2/2 mole H2O) = 3.95 mole oxygen gas needed ------------------------------------------
How much mass does 1 mol of o2 gas have?
15.99 x 2 g
How many liters of water can be made from 5 L of oxygen gas and an excess of hydrogen?
55 grams O2 × (1 mol O2 ÷ 32 g O2) × (2 mol H2O ÷ 1 mol O2) × (22.4 L ÷ 1 mol H2O) = 77 L H2O(g)In the liquid form, it works out to just under 62 milliliters.
Calculate the number of atoms of O contained in 16.0 pounds of O?
16.0 lbs = 7,257 g of O2 Oxygen exists in the gas form as 02 7,257g O2 * 1 mol O2/ 32 g * 2 mol O / 1 mol O2 * 6.022x10^23 atoms/mol = 2.73E26 atoms of O
What is the volume of oxygen that will be used by 12g of Mg to be completely converted into MgO?
The reaction : Mg + O2-----------> MgO The balanced reaction : 2 Mg + O2-----------> 2 MgO that is 2 moles of Mg reacts with one mole of oxygen gas. moles of Mg reacted = 12 g / 24 g mol-1=0.5 mol. Thus the no. of mol of O2 reacted = 0.5 mol /2 =0.25 mol If the gas is at standard temperature and pressure, then Volume of 1 mol of O2 gas = 22.4 dm3 Volume of 0.25 mol of O2 gas = 22.4 x 0.25 dm3= 5.6 dm3 the volume of oxygen that will be used to react completely with 12 g Mg =5.6 dm3 (provided that the gas is at the standard conditions.)
How many moles of ozone O3 could be formed from 96.0g of oxygen gas O2?
A) 0.500 mol B) 1.000 mol C) 2.00 mol D) 3.00 mol E) 1/16 mol
How many liters of oxygen gas are present in 11.3 grams of oxygen gas?
Because oxygen gas (O2) has a molar mass of 32g/mol, 11.3 g * 1/32 mol/g gives about .35 moles. An ideal gas has a volume of 22.4 L/mol at STP, so 11.3 g O2 would have a volume of 7.91 L at STP.
The number of moles of h2o formed when 1 mole of o2 reacts with c5h12 in the reaction c5h12 plus 8o2 equals 5co2 plus 6h2o is?
C5H12 + 8 O2 --> 5 CO2 + 6 H2O (1 mol O2)(6 mol H2O/8 mol O2) = 0.75 mol H2O
How many grams of water are produced by reacting 15.8 g H2 with excess oxygen?
24g H2 x 1 mol H2 x 2 mol H2O x 18g H2O/ 2g H2 x 2 mol H20= 216 g H2O 160g O2 x 1 mol O2 x 2 mol H2O x 18g H2O/ 32g O2 x 1 mol O2 x 1 mol H2O= 180 g H2O
How many oxygens atoms does 1 mol of O2 gas have?
Type your answer here... 2 × (6.02 × 1023)
How many moles and how many molecules are in 64 g of oxygen gas?
1 mole O2 weighs 32 gso 64 g O2 is 2 mol O2 gaswhich has 2 X 6.022 X 1023 = 1.2066 X 1024 molecules of O2
How many liters of pure oxygen at STP is consumed by a human being in 24 hours if the human body requires daily energy that comes from metabolizing 816 grams of sucrose c12 h22 o11?
816 g C12H22O11 x (1 mol C12H22O11 / 342.0 g C12H22O11) x (12 mol O2 / 1 mol C12H22011) x (22.4 L O2 / 1 mol O2) = 641 L O2
How many moles of oxygen gas O2 needed to react with 4.00 mol of Mg?
Do you mean this reaction? 2Mg + O2 -> 2MgO 4.11 moles Mg (1 mole O2/2 mole Mg) = 2.06 moles oxygen gas consumed --------------------------------------------------
