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How many moles of H2 are required to react with 5.0 moles O 2?
You use the Mole-to-Mole ratio. If the equation is 2CH4 + 2H2O = 6H2 + 2CO, then you would start with your given, 8.0 mol CO and multiply that with your mol-to-mol ratio which is (2mol CO/ 2 mol CH4). Your answer will be 8.0 mol.
How many grams of water form when 1.24L of H2 gas at STP reacts with O2?
When 1.24 L of H2 gas reacts with O2 at STP, the mole ratio between H2 and H2O is 2:2. This means that for every 1 mole of H2 gas reacting, 1 mole of water is formed. Using the ideal gas law, you can calculate the number of moles of H2 gas reacting, and then use the mole ratio to determine the number of moles of water formed. Finally, you can convert moles of water to grams using the molar mass of water.
What is the mole ratio of salt to water in Co(NO3)2.6H2O?
2:1
How many moles K are needed to react with 15 moles of Cl2?
H2 +Cl2---------------->2HCl Since H2 and Cl2 react in 1:1 mole ratio the number of moles of H2 reacting is equal to the number of moles of Cl2 which is equal to 0.213
What is the mole ratio of water vapor to H2?
The mole ratio of water vapor (H₂O) to hydrogen gas (H₂) can be determined from the balanced chemical equation for the combustion of hydrogen: 2 H₂ + O₂ → 2 H₂O. From this equation, we see that 2 moles of H₂ produce 2 moles of H₂O, resulting in a mole ratio of 1:1. Thus, for every mole of hydrogen gas, one mole of water vapor is produced.
What is the mole ratio of C5H12 to H2 in the following reaction?
The mole ratio of C5H12 to H2 in the reaction is 1:8. This means that for every 1 mole of C5H12, 8 moles of H2 are consumed or produced in the reaction.
How many moles of H2 are required to react with 5.0 moles O 2?
You use the Mole-to-Mole ratio. If the equation is 2CH4 + 2H2O = 6H2 + 2CO, then you would start with your given, 8.0 mol CO and multiply that with your mol-to-mol ratio which is (2mol CO/ 2 mol CH4). Your answer will be 8.0 mol.
How many grams of water form when 1.24L of H2 gas at STP reacts with O2?
When 1.24 L of H2 gas reacts with O2 at STP, the mole ratio between H2 and H2O is 2:2. This means that for every 1 mole of H2 gas reacting, 1 mole of water is formed. Using the ideal gas law, you can calculate the number of moles of H2 gas reacting, and then use the mole ratio to determine the number of moles of water formed. Finally, you can convert moles of water to grams using the molar mass of water.
Give the mole ratio for the following equation Zn 2HCl -- ZnCl2 H2?
The mole ratio for the given equation is 1:2:1. This means that for every 1 mole of zinc (Zn) used, 2 moles of hydrochloric acid (HCl) are required to produce 1 mole of zinc chloride (ZnCl2) and 1 mole of hydrogen gas (H2).
What is the mole ratio of salt to water in Co(NO3)2.6H2O?
2:1
How many molecules (not moles) of NH3 are produced from 5.69104 g of H2?
The reaction would be H2 + 3N2 ==>2NH3moles H2 used = 5.69104 g x 1 mole/2.00 = 2.84552 moles H2moles NH3 produced (assuming N2 is NOT limiting) = 2 moles NH3/mole H2 x 2.84552 moles H2 = 5.69104 moles NH3 producedMolecules of NH3 produced = 5.69104 moles x 6.02x10^23 molecules/mole = 3.4x10^24 molecules
What is the mole to mole ratio of nitrogen gas and hydrogen gas?
1:3 because...in the equation N2+3H2---> 2NH3the product is 2NH3... there are 2 Nitrogens and 6 Hydrogens (2*3) making the ratio 2:6; but the correct simplified answer is 1:3
How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 19.1 moles of water vapor?
CO2 + H2 <-> CO + H2O all one to one ( I assume that 99.1 is grams. Always units!!!! ) 99.1 grams H2O (1 mole H2O/18.016 grams)(1 mole H2/1 mole H2O) = 5.50 moles of hydrogen gas needed If that was 99.1 moles water vapor then it would take 99.1 moles hydrogen gas at a one to one ratio.
How many moles K are needed to react with 15 moles of Cl2?
H2 +Cl2---------------->2HCl Since H2 and Cl2 react in 1:1 mole ratio the number of moles of H2 reacting is equal to the number of moles of Cl2 which is equal to 0.213
Calculate the number of mole of hydrogen in 37.66gm?
37.66 (g H2) / 2.016 (g/mol H2)= 18.68 mole H2Molar mass of hydrogen: 2.016 (g/mol H2)
How many liters of Hydrogen gas are formed from the complete reaction of 1.07 moles of carbon. C h20--- CO H2?
You stated the amount of carbon you had, but how much water (separated into its constituents by electrolysis, otherwise if you dump water on carbon you wind up with nothing more than wet carbon) is available? Let's assume you've got an excess of it and go from there.In a real-life situation you won't get any hydrogen gas. In order of reactivity are hydrogen, oxygen and carbon. One of three things will happen here.The most likely reaction is that the hydrogen and oxygen will recombine into water and, once again, you've got wet carbon...that is, unless the heat from the very exothermic 2H2 + O2 -> 2H2O reaction sets the carbon on fire, in which case it'll scavenge atmospheric O2 and you'll receive some CO2, some CO and a little free carbon, aka "soot."Under different circumstances, you might get some CH4 and some O2. And because you have 1.07 moles C, you'll wind up with 1.07 moles methane - giving you 23.968 liters of methane at STP.If you have a really nice lab that can emulate photosynthesis, you could convert the three elements into glucose. That's not too likely; you will probably wind up with the same block of carbon and glass of water that you started out with.The chemical reaction should be written as shown below : C + H2O -----> CO + H2 The balanced chemical reaction equation indicates that 1.0 mole of H2 gas is produced for each mole of carbon that reacts. Therefore you have : n H2 = (1.07 mole C ) ( 1.0 mole H2 / 1.0 mole C ) = 1.07 moles H2 At STP, there are 22.7 L per mole of ideal gas. Therefore the H2 liters at STP is given by : V H2 at STP = ( 22.7 L at STP / mole ideal gas ) ( 1.07 moles H2 ) V H2 at STP = 24.3 L of H2 at STP
How many grams of H2 are needed to produce 14.84 g of NH3?
To find the grams of H2 needed, we first calculate the moles of NH3 using its molar mass. Then, we use the balanced chemical equation to determine the mole ratio of H2 to NH3. Finally, we convert moles of H2 to grams using its molar mass.
