0
What number of grams of NH3 produced by the reaction of 3.5g of hydrogen gas with sufficient nitrogen gas?
Wiki User
∙ 13y ago
Assuming you mean the decomposition of ammonia: 2NH3 --> N2 + 3H2, 100g NH3 = 5.88mol (100/17), and the ratio of ammonia to nitrogen is 2:1. 5.88mol/2=2.94mol, so that's the amount of nitrogen produced. 2.94x28 (molar mass of N2) gets you 82.3g nitrogen produced.
Marielle Hane
Wiki User
∙ 9y agoFirst lets convert the 100g N2 into moles (100/28=3.57 moles). Now lets look at the balanced reaction equation:
N2 + 3H2 -> 2NH3
This means that if I have 3.57 moles of N2, I will make 7.14 moles of NH3. Now, assuming that everything can be modelled as an ideal gas:
V=(nRT)/P
V=(7.14*.0821*273)/1= 160.03 L
Wiki User
∙ 13y agoBalanced equation first. ( hydrogen limits, which saves that work! )
N2 + 3H2 >> 2NH3
3.5 grams hydrogen gas (1 mole H2/2.016 g)(2 mole NH3/3 mole H2)(17.034 grams/1 mole NH3)
= 19.7, or 20 grams of NH3 produced
Wiki User
∙ 11y agoWell, since ammonia has the chemical formula NH3. Therefore the relative Atomic Mass is 17 (14+(1)3). So 100 divided by 17, times 3 = 17.64705882352941g. I did this in order to figure out firstly, how much the weight of 1 of the 17 nuclear particles, which make up ammonia, would have to be present (in grams) for everything to be in proportion to which would make 100g. Then by timesing it by 3 shows how much the 3 hydrogen atoms contributed in weight towards the 100 grams. To prove that 17.64... is correct you can add (100/(17) X (17-3).
Wiki User
∙ 8y agoAssuming you mean the decomposition of ammonia: 2NH3 --> N2 + 3H2, 100g NH3 = 5.88mol (100/17), and the ratio of ammonia to nitrogen is 2:1. 5.88mol/2=2.94mol, so that's the amount of nitrogen produced. 2.94x28 (molar mass of N2) gets you 82.3g nitrogen produced.
Wiki User
∙ 8y agoAt STP 22.4 L is 1 mole, so 100 L/22.4. = 4.46 moles of NH3 which means 4.46 moles of N (nitrogen). Since each mole of N2 gas supplies 2 moles of N, you need 2.23 moles of N2 gas. The grams of N2 gas would be 2.23 moles x 28g/mole = 62.44 grams.
Wiki User
∙ 12y ago40.0 liters
Work: 25g | 1 mol N2 | 2 mol NH3 | 22.4 L NH3
| 28g N2 | 1 mol N2 | 1 mol NH3
Wiki User
∙ 6y agoThe volume of ammonia is 738,2 L at STP.
Wiki User
∙ 8y ago100g NH3 contain 82,24 g nitrogen.
Wiki User
∙ 8y agoThe answer is 63.24 g nitrogen.
Add your answer:
Earn +20 pts
How many moles of ammonia gas are produced by the reaction of 3 mole of nitrogen gas with excess hydrogen gas N2 H2 ---- NH3?
N2 + 3H2 --> 2NH3 You have been told, indirectly, that nitrogen limits and will drive the reaction. 3 moles N2 (2 moles NH3/1 mole N2) = 6 moles ammonia gas produced ========================
What is the chemical reaction between ammonia and cupric oxide?
copper , nitrogen & water produced
Does the removal of hydrogen gas as it is produced shift the reaction to the left or the right?
Right
What temperature does nitrogen gas burn?
Nitrogen burns to form Nitrogen Dioxide at about 2200F. It is an exothermic reaction, meaning it will produce heat sufficient to sustain itself if the heat is confined, for example in an internal combustion engine.
If an excess of nitrogen is reacted with 3.41 grams of hydrogen how many grams of ammonia can be produced?
Balanced equation first. N2 + 3H2 >> 2NH3 (hydrogen is limiting and drives the reaction ) 3.41 grams H2 (1mol/2.016g )(2mol NH3/3mol H2 )(17.034g NH3/1mol NH3 ) = 19.2 grams of ammonia produced ( this is called the Born-Haber process )
From what elements is ammonia produced?
a reaction with nitrogen and hydrogen
Which reaction adds hydrogen ions to the blood?
nitrogen
Nitrogen gas react with hydrogen gas to form ammonia what are the reactants in this chemical reaction?
nitrogen gas and hydrogen gas
What is the chemical formula when nitrogen gas reacts with hydrogen gas?
Nitrogen and hydrogen react to form ammonia. This is the reaction in the Haber process, in which the gases are mixed at high pressure and moderately high temperature and passed over an iron catalyst.
What mass of ammonia NH3 could be produced from the reaction of 44.5 g of nitrogen N2 and 2.58 g of hydrogen H2?
The equation for the reaction is N2 + 3 H2 -> 2 NH3. The gram atomic mass of nitrogen is 14.0067, and the gram atomic mass of hydrogen is 1.00794. Therefore, the mass fraction of nitrogen in ammonia is 14.0067/[14.0067 + (3*)(1.00794)] or about 0.8225, and, since nitrogen and hydrogen are the only two elements present, the mass fraction of hydrogen is 1*- 0.8225 or about 0.1775. The mass fraction of nitrogen in the amounts of nitrogen and hydrogen specified is 44.5/(44.5 + 2.58) or about 0.945. Therefore, hydrogen is the limiting reactant in this mixture, and the mass of ammonia produced is 2.58/0.1775 or 14.5 grams, to the justified number of significant digits. ________________ *An exact integer.
How many moles of hydrogen cyanide would be produced from the complete reaction of 10 moles of oxygen gas?
Absolutely none, as there is no oxygen in hydrogen cyanide. Its formula is HCN--one atom each of hydrogen, carbon and nitrogen.
What is produced when hydrogen reacts with water?
There is no reaction.
What is the reaction state of N in NH4?
Nitrogen has four bonds with hydrogen.
When nitrogen combines with hydrogen is there a chamical reaction or a phsical reaction?
Studies on the subject have continually proven that there is no such thing as a phsical reaction.
What is the reaction called when nitrogen plus hydrogen yield ammonia?
Haber's process
What gas is formed when hydrogen reacts with nitrogen?
After this reaction ammonia (NH3) is obtained.
How many moles of ammonia gas are produced by the reaction of 3 mole of nitrogen gas with excess hydrogen gas N2 H2 ---- NH3?
N2 + 3H2 --> 2NH3 You have been told, indirectly, that nitrogen limits and will drive the reaction. 3 moles N2 (2 moles NH3/1 mole N2) = 6 moles ammonia gas produced ========================
