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CO2 + H2 -> CO + H2O one to one here 30.6 moles H2O (1 mole H2/1 mole H2O) = 30.6 moles Hydrogen gas needed
decomposition
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.
Balanced equation first.2H2 + O2 --> 2H2OGet moles products.4 grams H2 (1 mole H2/2.016 grams) = 1.984 moles H264 grams O2 (1 mole O2/32 grams) = 2.000 moles O2I suspect hydrogen gas of limiting and driving the reaction.1.984 moles H2 (1 mole O2/2 moles H2) = 0.992 moles O2 ( you have more than this in equation )2.000 moles O2 (2 mole H2/1 mole O2) = 4.000 moles H2 ( you do not have this much and H2 will drive this reaction )1.984 moles H2 (2 moles H2O/2 moles H2)(18.016 grams/1 mole H2O)= 36 grams water produced====================
20 moles of Al will react with water to form 60 moles of H2 and 30 moles of O2, because of the stoichiometry 2:1 in getting H2 en O2 from water, and Al needing an oxidationstate of 3+, so 1 mole is oxidized by 3 moles of H2O.
c5h12toh2
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.
CO2 + H2 -> CO + H2O one to one here 30.6 moles H2O (1 mole H2/1 mole H2O) = 30.6 moles Hydrogen gas needed
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.
decomposition
Balanced equation first.2H2 + O2 --> 2H2OGet moles products.4 grams H2 (1 mole H2/2.016 grams) = 1.984 moles H264 grams O2 (1 mole O2/32 grams) = 2.000 moles O2I suspect hydrogen gas of limiting and driving the reaction.1.984 moles H2 (1 mole O2/2 moles H2) = 0.992 moles O2 ( you have more than this in equation )2.000 moles O2 (2 mole H2/1 mole O2) = 4.000 moles H2 ( you do not have this much and H2 will drive this reaction )1.984 moles H2 (2 moles H2O/2 moles H2)(18.016 grams/1 mole H2O)= 36 grams water produced====================
20 moles of Al will react with water to form 60 moles of H2 and 30 moles of O2, because of the stoichiometry 2:1 in getting H2 en O2 from water, and Al needing an oxidationstate of 3+, so 1 mole is oxidized by 3 moles of H2O.
Mg + 2HCl => MgCl2 + H2 2 moles HCl : 1 mole H2. 2.02 x .5 moles = 1.01 1.01g H2
H2O > H2 > He
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
Balanced equation. 2H2 + O2 --> 2H2O 5 moles H2 (2 moles H2O/2 mole H2)(18.016 grams/1 mole H2O) = 90 grams of water ===============
Balanced equation. 2H2 + O2 >> 2H2O ( now find limiting reactant ) 7 grams H2 (1 mole H2/2.016 grams) = 3.472 moles H2 60 grams O2 (1 mole O2/32 grams) = 1.875 moles O2 1.875 moles O2 (2 mole H2/1 mole O2) = 3.75 mole H2 ( checked O2, but I know H2 limits because you do not have 3.75 moles H2, so H2 drives reaction) 3.472 moles H2 (2 mole H2O/2 mole H2)(18.016 grams/1 mole H2O) = 62.552 grams H2O produced, so; 58 grams/62.552 times 100 = 92.7% yield of H2O, call it 93%