This is based on calculations too. It contains 18 hydrogen moles.
3H2 + N2 --> 2NH3 is the balanced equation. 13.14g of ammonia is 0.773mol, and that means 1.16mol hydrogen (according to the 2:3 ratio.) 1.16mol of hydrogen = 2.32g of hydrogen.
how many grams of hydrogen peroxide are needed to produce 5.0 moles of water? how many grams of hydrogen peroxide are needed to produce 5.0 moles of water?
This value is 0,2 g hydrogen.
N2 + 3H2 -> 2NH3 The stoichiometric equation (or balanced equation) for the formation of ammonia from this we can read off the mole ratio between hydrogen and ammonia; 3M H2 needed to produce 2M NH3 times each by 9 (so the ratio remains the same and 18M NH3 is formed) 27M H2 needed to produce 18M NH3
40 l h2
According balanced equation ,3 mols are needed. So 3mol shoul be mixed
52,4 moles of hydrogen
2,18 g hydrogen are needed.
1,364 g hydrogen are needed.
2,21 g hydrogen are needed.
162g is the theoretical yield of beryllium that is needed to produce 36.0 g of hydrogen.
3,13 g hydrogen are needed.
84,2 moles hydrogen are needed.
Equation. CO2 + H2 - CO + H2O all one to one, so you need 53.6 moles of hydrogen gas
Yes, it is required during photosynthesis to produce glucose
The answer is 1,97 h hydrogen.
The ratio of atomic weights for hydrogen and oxygen is 1/16 so the ratio in a water molecule which has 2 hydrogens for each oxygen would be 2/16. Another way to look at it is that the ratio of the mass of hydrogen in a water molecule to the total mass of the molecule would be 2/18. For 1.8 g of water this is equivalent to 0.2/1.8, i.e. you need 0.2 g of hydrogen to produce 1.8 grams of water.
The balanced equation for the formation of NH3 is N2 + 3 H2 --> 2 NH3. 13.64 grams of ammonia is equal to .801 moles. Then 1.2015 moles of hydrogen are needed, or 2.42 grams.
The "gas" needed for the electron transport chain is Hydrogen. In the electron transport chain its not Hydrogen gas H2 but a Hydrogen Ion H negative that flows across the membrane to produce engery.
The answer is 2.23 g hydrogen.
the theoretical yield is 162 grams
5g of oxygen are required to completely react with 10g of hydrogen resulting in water with no net losses. Or exactly 2:1 = H20 (2 hydrogen < > 1 oxygen)