0
What else can I help you with?
Why does the yield of ammonia at equllibrium increase as the temperature is decreased?
When the temperature is decreased, the reverse reaction (in this case, the decomposition of ammonia into nitrogen and hydrogen) is favored because it is an exothermic reaction. In response to the increased reverse reaction, the forward reaction (formation of ammonia from nitrogen and hydrogen) increases to re-establish equilibrium, ultimately leading to a higher yield of ammonia.
Nitrogen and hyrogen form ammonia by the reaction N2 plus 3H2 to 2NH3. If 56 grams of nitrogen and 85 grams of hydrogen react to form 62 grams of ammonia. What is the percent yield?
To find the percent yield, first calculate the theoretical yield of ammonia based on the given amounts of nitrogen and hydrogen. Then compare the actual yield (62g) with the theoretical yield to calculate the percent yield using the formula: (actual yield/theoretical yield) x 100%. The percent yield would be the actual mass of ammonia produced (62g) divided by the theoretical yield of ammonia.
Why is pressure used in the production of ammonia?
The formation of Ammonia by Haber's process is a reversible process, one volume of nitrogen reacts with three volumes of hydrogen and form two volumes of Ammonia, N2 + 3H2 = 3NH3 , According to Le-Chatlier's principle the increase in pressure brings the molecules of nitrogen and hydrogen closer to each other and shifts the reaction towards formation of ammonia, so higher pressure is responsible for higher yield of ammonia.
What are the conditions used to make ammonia?
Ammonia is produced through the Haber-Bosch process, which involves reacting nitrogen and hydrogen gases at high temperature (400-500°C) and pressure (150-200 atm) in the presence of an iron catalyst. This process typically takes place in a reactor to facilitate the formation of ammonia.
What are the ideal conditions to get high yield of ammonia?
To achieve a high yield of ammonia, the ideal conditions include a high pressure (around 200 atmospheres), a low temperature (around 450 degrees Celsius), and the presence of a catalyst (usually iron mixed with other metals). Additionally, maintaining an optimized stoichiometric ratio of hydrogen to nitrogen is crucial for maximizing the production of ammonia.
What is the reaction called when nitrogen plus hydrogen yield ammonia?
Haber's process
Why does the yield of ammonia at equllibrium increase as the temperature is decreased?
When the temperature is decreased, the reverse reaction (in this case, the decomposition of ammonia into nitrogen and hydrogen) is favored because it is an exothermic reaction. In response to the increased reverse reaction, the forward reaction (formation of ammonia from nitrogen and hydrogen) increases to re-establish equilibrium, ultimately leading to a higher yield of ammonia.
Nitrogen and hyrogen form ammonia by the reaction N2 plus 3H2 to 2NH3. If 56 grams of nitrogen and 85 grams of hydrogen react to form 62 grams of ammonia. What is the percent yield?
To find the percent yield, first calculate the theoretical yield of ammonia based on the given amounts of nitrogen and hydrogen. Then compare the actual yield (62g) with the theoretical yield to calculate the percent yield using the formula: (actual yield/theoretical yield) x 100%. The percent yield would be the actual mass of ammonia produced (62g) divided by the theoretical yield of ammonia.
Which process is iron used as catalyst?
Iron is used as a catalyst in the Haber process, which is the industrial method for producing ammonia from nitrogen and hydrogen gases. The presence of iron catalyst helps to increase the rate of the reaction and improve the yield of ammonia.
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 )
Why is pressure used in the production of ammonia?
The formation of Ammonia by Haber's process is a reversible process, one volume of nitrogen reacts with three volumes of hydrogen and form two volumes of Ammonia, N2 + 3H2 = 3NH3 , According to Le-Chatlier's principle the increase in pressure brings the molecules of nitrogen and hydrogen closer to each other and shifts the reaction towards formation of ammonia, so higher pressure is responsible for higher yield of ammonia.
What is the balanced equation describing the reaction between hydrogen gas and nitrogen gas to produce ammonia NH3?
3H2 + N2 --> 2NH3 Since Hydrogen (H) and Nitrogen (N) both appear in nature diatomically they only appear as H2 and N2. We must add 3 molecules of Hydrogen and 1 molecule of Nitrogen to get 2 molecules of ammonia. We cannot, in nature, have half of a diatomic Hydrogen or Nitrogen atom, for that reason the equation must yield 2 molecules of Ammonia.
What are the conditions used to make ammonia?
Ammonia is produced through the Haber-Bosch process, which involves reacting nitrogen and hydrogen gases at high temperature (400-500°C) and pressure (150-200 atm) in the presence of an iron catalyst. This process typically takes place in a reactor to facilitate the formation of ammonia.
What are the ideal conditions to get high yield of ammonia?
To achieve a high yield of ammonia, the ideal conditions include a high pressure (around 200 atmospheres), a low temperature (around 450 degrees Celsius), and the presence of a catalyst (usually iron mixed with other metals). Additionally, maintaining an optimized stoichiometric ratio of hydrogen to nitrogen is crucial for maximizing the production of ammonia.
What effect does increasing pressure have on the yield of ammonia in the Haber process?
It increases the yield. 3 moles of hydrogen react with one mole of nitrogen to produce two moles of ammonia. As there is a REDUCTION in molecules, there will be a reduction in pressure. This is alsos an equilibrium reaction. So by Le Chetalier's principle, if we increase pressure, the system will react to reduce the pressure again. This can be done by producing more ammonia - in other words, an increase in product yield.
How can the yield of ammonia be increased?
To increase the yield of ammonia in the Haber process, you can: Increase the pressure: Higher pressure shifts the equilibrium towards the product side, increasing the amount of ammonia produced. Optimize the temperature: Lower temperatures are favorable for ammonia production, but it’s a balance to prevent the reaction from being too slow. Use a suitable catalyst: Iron catalysts are commonly used to speed up the reaction without being consumed. Optimize the ratio of reactants: Ensuring the ideal ratio of nitrogen and hydrogen in the reaction mixture can also improve the yield of ammonia.
Balance ammonia plus oxygen to yield nitrogen trioxide plus water?
2 NH3 + 3 O2 = N2O3 + 3H2O
