The nunber of moles of oxygen is 2,5.
1 mole
N2 + 3H2 -> 2NH3 3 moles hydrogen gas. You should know that because of the formula of ammonia.
Since hydrogen is a gas, we would need more information to answer it. As chance wrote, you will need twice as much hydrogen as oxygen. However, in order to know what the volume of that hydrogen is, we also need to know the temperature and pressure so that we can use the universal gas law to get the answer.
No, this would make 5 moles. This is because water is H2O. This means that for each oxygen molecule used, there will be 2 hydrogen molecules used. In the given equation Only 5 moles of oxygen could be used to pair with all 10 moles of hydrogen, therefore giving you an excess of 5 oxygen molecules.
Carbon dioxide form a milky suspension of calcium carbonate in calcium hydroxide; hydrogen doesn't react. But hydrogen react with oxygen when a flame exist.
Here is the BALANCED reaction eq'n. 2H2(g) + O2(g) = 2H2O(l) The prefix number are the Molar Ratios 2:1::2 So oxygen is ONE(1) mole Hence hydrogen is TWO(2) moles It produces TWO(2) moles of water.
1 mole
Absolutely none, as there is no oxygen in hydrogen cyanide. Its formula is HCN--one atom each of hydrogen, carbon and nitrogen.
2H2 + O2 --> 2H2OAs you can see by the balanced reaction, for every 1 mole of oxygen used, 2 moles of water are formed. Also notice that for every 1 mole of oxygen used, you need 2 moles of hydrogen to produce the 2 moles of water. So in your case 110 moles of oxygen would produce 220 moles of water & would also require 220 moles of hydrogen (which you have in excess since you have 230 moles of hydrogen). So 220 moles of water are the most that can be formed.
N2 + 3H2 -> 2NH3 3 moles hydrogen gas. You should know that because of the formula of ammonia.
For each mole of hydrogen gas (H2) reacting with chlorine gas (Cl2), you will get 2 moles of HCl. H2 + Cl2 = 2 HCl
Since hydrogen is a gas, we would need more information to answer it. As chance wrote, you will need twice as much hydrogen as oxygen. However, in order to know what the volume of that hydrogen is, we also need to know the temperature and pressure so that we can use the universal gas law to get the answer.
No, this would make 5 moles. This is because water is H2O. This means that for each oxygen molecule used, there will be 2 hydrogen molecules used. In the given equation Only 5 moles of oxygen could be used to pair with all 10 moles of hydrogen, therefore giving you an excess of 5 oxygen molecules.
This reaction?? 2H2O -> 2H2 + O2 this would be one to one and you would get; 174.82 moles of water vapor Without an equation I do not really know what you mean.
Carbon dioxide form a milky suspension of calcium carbonate in calcium hydroxide; hydrogen doesn't react. But hydrogen react with oxygen when a flame exist.
What compound? Please copy your homework questions completely. How else can we help you cheat?To find the number of moles of oxygen (or any other element), multiply the number of atoms present on the molecule (in subscript) by the number of molecules present in the reaction (in standard script to the left of the molecule)In this case:2 H2 + O2 --> 2 H2OOn the reactant side (to the left of the arrow), there are 4 moles of hydrogen present because we have inserted 2 moles of diatomic hydrogen (multiply the subscript 2 by the standard script 2 to the left of the molecule). We can calculate that there are 2 moles of oxygen present because we have inserted one mole of diatomic oxygen. On the products side (the right side of the arrow) we produced 2 moles of water (indicated by the standard script 2 to the left of the molecule) Each molecule of water contains 2 molecules (2 moles) of hydrogen and one molecule (one mole) of oxygen. Thus, we have a balanced equation because this gives us 4 moles of hydrogen and 2 moles of oxygen, just like we had on the reactant side.The multipliers in standard script to the left of the molecule gives us the molar ratio. 2 moles of diatomic hydrogen react with 1 mole of diatomic oxygen to produce 2 moles of water. Thus, if we were to burn .5 moles of diatomic hydrogen in excess oxygen, we would produce .5 moles of water. This is because, by looking at our chemical equation, we see that the molar ratio of diatomic hydrogen to water is 2:2 (or 1:1). We would have .25 moles of oxygen because the ratio of hydrogen to oxygen is 4:2 (or 2:1).Were this the question on your homework, the answer would be ".25 moles"
CO2 + H2 -> CO + H2O one to one here 30.6 moles H2O (1 mole H2/1 mole H2O) = 30.6 moles Hydrogen gas needed