Nitrogen and hydrogen gases react to form ammonia gas. N_2(g) + 3 H_2(g) ? 2 NH_3(g) At a...
Question:
Nitrogen and hydrogen gases react to form ammonia gas.
N_2(g) + 3 H_2(g) ? 2 NH_3(g)
At a certain temperature and pressure 0.70 L of N_2 reacts with 2.1 L of H_2. If all the N_2 and H_2 are consumed, what volume of NH_3, at the same temperature and pressure, will be produced? _ L
Gas Stoichiometry:
For reactions at constant temperature and pressure, the stoichiometric coefficients of the balanced chemical equation can be taken as the volumes of gases reacting. The ratio of coefficients can then be used as conversion factors to relate the quantities of gases to one another.
Answer and Explanation:
Become a Study.com member to unlock this answer! Create your account
View this answerSee full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
Molarity & Stoichiometry | Definition, Formula & Calculation
from
Chapter 9 / Lesson 4
12K
Learn how to find the molarity of a solution or the moles of gas in a given volume using stoichiometry. See examples of calculating moles from molarity.
Related to this Question
- Nitrogen and hydrogen gases react to form ammonia gas via the following reaction: N 2 ( g ) + 3 H 2 ( g ) 2 N H 3 ( g ) . At a certain temperature and pressure, 1.5 L of N 2 reacts with 4.5 L of H 2 . If all of the nitrogen and hydrogen gas is cons
- Nitrogen and hydrogen gases react to form ammonia gas. N_2(g) + 3 H_2(g)\to 2 NH_3(g)
- Nitrogen and hydrogen gases react to form ammonia gas via the following reaction: N2(g) + 3H2(g) arrow 2NH3(g) At a certain temperature and pressure, 1.5 L of N2 reacts with 4.5 L of H2. If all the N
- If 4.67 L of nitrogen gas and 36.56 L of hydrogen gas were allowed to react, how many liters of ammonia gas could form? Assume all gases are at the same temperature and pressure.
- If 7.35 L of nitrogen gas and 26.04 L of hydrogen gas were allowed to react, how many liters of ammonia gas could form? Assume all gases are at the same temperature and pressure.
- If 2.76 L of nitrogen gas and 29.21 L of hydrogen gas were allowed to react, how many liters of ammonia gas could form? Assume all gases are at the same temperature and pressure.
- Nitrogen and hydrogen react in the Haber's process to form ammonia. All substances are in the gas phase. If 0.385 atm of nitrogen and 0.792 atm of hydrogen react, what is the partial pressure of ammonia (in mmHg) when this reaction goes 69% complete. The
- Nitrogen dioxide and dinitrogen monoxide gases react to form nitrogen monoxide gas(es). NO2(g) + N2O(g) 3 NO(g) At a certain temperature and pressure 48.1 L of NO2 reacts with 48.1 L of N2O. If all
- Nitrogen and oxygen gases react to form dinitrogen trioxide gas. 2 N_2(g) + 3 O_2(g) ---> 2 N_2O_3(g) At a certain temperature and pressure 5.6 L of N_2 reacts with 8.4 L of O_2. If all the N_2 and O_2 are ...
- Nitrogen gas (N2) reacts with hydrogen gas (H2) to form ammonia (NH3). At 200 degrees C in a closed container, 1.1 atm of nitrogen gas is mixed with 2.1 atm of hydrogen gas in an otherwise empty conta
- Ammonia gas can be formed through the reaction between nitrogen gas and hydrogen gas. This reaction was conducted in a sealed container at a constant volume of 1 L and a constant temperature of 25 degrees Celsius. If the pressure on the container initiall
- Nitrogen gas reacts with hydrogen gas to form ammonia. The nitrogen gas is in a closed 500.0 mL flask at 751 mm Hg connected to a 1.25 L flask containing the hydrogen gas at 1.21 atm pressure. Both fl
- Ammonia is often formed by reacting nitrogen and hydrogen gases. How many liters of ammonia gas can be formed from 23.7 L of hydrogen gas at 93.0 degrees C and a pressure of 38.9 kPa?
- Nitrogen gas (N2) reacts with hydrogen gas (H2) to form ammonia gas (NH3). Nitrogen and hydrogen gases are in a 15.0-L container fitted with a movable piston (the piston allows the container volume to change so as to keep the pressure constant inside
- Hydrogen gas, H_2, reacts with nitrogen gas, N_2, to form ammonia gas, NH_3, according to the equation 3H_2(g)+N_2(g) \rightarrow 2NH_3(g) NOTE: Throughout this tutorial use molar masses expressed to
- Ammonia is formed by reacting nitrogen and hydrogen gases. How many liters of ammonia gas is formed from 13.7 L of hydrogen gas at 93 degree C and pressure of 40 kPa?
- Ammonia is often produced by reacting nitrogen gas with hydrogen gas. How many liters of ammonia gas can be formed from 12.9 L of hydrogen gas at 93.0 degrees C and a pressure of 43.5 kPa? (Assume an
- Ammonia is formed by reacting nitrogen and hydrogen gases. How many liters of ammonia gas is formed from 13.7 L of hydrogen gas at 93 degrees C and pressure of 40 kPa?
- Nitrogen and hydrogen gas react to form ammonia gas. At a certain temperature and pressure, 1.2 L of N_2 reacts with 3.6 L of H_2. If all of both gases are consumed what is the final volume of NH_3 produced?
- Ammonia is created in the Haber process in a rigid container (nitrogen gas plus hydrogen gas react to form ammonia gas). 10 moles of hydrogen gas are mixed with 5 moles of nitrogen gas. The initial pressure exerted on the container is 10 atm. Assuming the
- Ammonia (NH_3) is formed industrially by reacting nitrogen and hydrogen gases. How many liters of ammonia gas can be formed from 13.7 L of hydrogen gas at 93.0^o C and a pressure of 2.25 atm?
- Ammonia is often formed by reacting nitrogen and hydrogen gases. How many liters of ammonia gas can be formed from 17.2 L of hydrogen gas at 93.0^oC and a pressure of 45.8 kPa?
- If 3.00 L of nitrogen and 7.00 L of hydrogen were allowed to react, how many liters of NH_3 (g) could form? Assume all gases are at the same temperature and pressure, and that the limiting reactant is used up. N_2(g) + 3H_2(g) \to 2NH_3(g)
- If 5.0 L of nitrogen at 12 degrees C and 1.30 atm pressure reacts with the same volume of hydrogen at the same temperature and pressure, what volume of ammonia is obtained at that temperature and pressure?
- Ammonia decomposes completely to hydrogen and nitrogen gas. If the total pressure of the reaction vessel at the end of the reaction is 250 mmHg, what is the partial pressure of nitrogen gas?
- Ammonia reacts with oxygen at 120 degrees Celsius to form nitrogen monoxide and water in a sealed 40 L container. When 34 g of ammonia reacts with 96 g of oxygen, what is the partial pressure of the nitrogen monoxide? What is the total pressure? Write the
- Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 200 mL flask with 0.96 atm of ammonia gas at 43.0 ^oC.
- Nitrogen gas (N_2) reacts with hydrogen gas (H_2) to form ammonia (NH_3). At 200 degrees C in a closed container, 1.04 atm of nitrogen gas is mixed with 2.03 atm of hydrogen gas. At equilibrium, the total pressure is 2.03 atm. Calculate the Kp value for
- When 6 liter of nitrogen gas reacts with 18 liters of hydrogen gas at constant temperature and pressure, how many liters of ammonia gas will be produced?
- Nitrogen and hydrogen react to form ammonia. Consider the mixture of N2 and H2 in a closed container. In this container, there are 6 diatomic molecules of hydrogen and 6 diatomic molecules of nitrogen
- When 18 liters of nitrogen gas react with 54 liters of hydrogen gas at constant temperature and pressure, how many liters of ammonia gas will be produced?
- A 24.0-L gas reaction chamber is charged with 65.0 atm of nitrogen gas and 154 atm of hydrogen gas at 200 degrees Celsius. a. Suppose that a reaction occurs to form ammonia according to the following equation until the limiting reactant is completely reac
- Nitrogen and oxygen react to form nitric oxide (NO). All substances are in the gas phase. If 0.352 atm of nitrogen and 0.511 atm of oxygen react, what is the partial pressure of nitric oxide (in mm of
- Nitrogen gas and hydrogen gas react to produce ammonia according to the following equation: N 2 ( g ) + 3 H 2 ( g ) 2 N H 3 ( g ) How many liters of hydrogen gas measured at 101.3 kPa and 273 K, are needed to react with 11.2 L of nitrogen gas, measure
- Nitrogen can react with oxygen to form nitrogen monoxide. N2(g) + O2(g) arrow 2NO(g); Kp = 1.0 x 10-30 at 25 degrees Celsius When equilibrium is established, the partial pressures of nitrogen and oxygen are 1.2 atm and 3.1 atm, respectively. What is the e
- Ammonia reacts with oxygen gas to form nitrogen monoxide and water. At constant temperature and pressure, how many of nitrogen monoxide can be made by the reaction of 800.0 ml of oxygen gas?
- Ammonia gas is produced by reacting hydrogen gas with nitrogen gas. To produce 50.0 g of ammonia gas using air as your source of nitrogen gas, what volume of air is required if the air is introduced at 29 C and 745 mmHg? (the mole fraction of nitrogen gas
- If 15.0 L of nitrogen is reacted with excess hydrogen, how many liters of ammonia could be produced? Assume all gas is ideal and measured at the same temperature and pressure.
- Hydrogen gas and nitrogen gas react to produce ammonia. How many liters of ammonia can be produced from 2 liters of hydrogen gas and 2 liters of nitrogen gas at STP?
- Ammonia and hydrogen chloride gases react to form solid ammonium chloride. A 10.0 L reaction flask contains ammonia at 0.452 atm and 22 degrees C, and 155 mL of hydrogen chloride gas at 7.50 atm and 2
- Ammonia reacts with oxygen gas to form nitrogen monoxide and water. At constant temperature and pressure, how much nitrogen monoxide can be made by the reaction of 800 mL of oxygen gas?
- VI). A sample of NH_3 gas is completely decomposed to nitrogen and hydrogen gases. a). Write a balanced chemical equation of this reaction. b). If the total pressure of the gas at the end of the rea
- Ammonia, NH_3, for fertilixer is made by causing hydrogen and nitrogen to react at high temperature and pressure. How many moles of ammonia can be made from 0.15 moles of nitrogen gas?
- At constant temperature and pressure, how many liters of ammonia will be formed when 6.00 L of nitrogen reacts with 30.0 L of hydrogen?
- When 4 litres of nitrogen gas react with 6 litres of hydrogen gas at constant temperature and pressure, how many litres of ammonia gas will be produced?
- A sample of ammonia gas (NH_3) is completely decomposed into nitrogen gas and hydrogen gas. If the total pressure at the end of the reaction is 866 mm Hg, what was the initial pressure of the ammonia?
- To produce 1.0 L of NH3(g) from hydrogen gas and nitrogen gas all at the same temperature and pressure would require ________ liters of hydrogen. N2(g) + 3 H2(g) --> 2 NH3(g)
- Ammonia gas is produced by reacting hydrogen gas with nitrogen gas. To produce 450 g of ammonia gas using air as your source of nitrogen gas, what volume of air is required if the air is introduced at 25 degrees C and 740 mmHg? A. 290 L B. 425 L C. 338
- In the Haber-Bosch process, nitrogen and hydrogen gas are reacted under high temperature of 500 degrees C and pressure 200 atm to form ammonia gas (NH3) according to the following equation: N2 + 3H2
- Ammonia was formed at 450 degrees C by passing a mixture of nitrogen gas and hydrogen gas at a 1 : 3 mole ratio over a catalyst. When the total pressure was held constant at 10.13 bar it was found that the product gas contained 2.04% by volume of ammonia.
- Ammonia is formed when nitrogen and hydrogen are mixed: N2(g) + 3 H2(g) = 2 NH3(g) A 2.00 L steel vessel contains 1.33 atm of nitrogen and 6.23 atm of hydrogen at 325 C. a) What will be the partial pressure of each gas if the reaction goes to completion?
- Nitrogen dioxide decomposes according to the reaction given below where K_P = 4.48 x 10^{-13} at a certain temperature. 2 NO_2(g) <---> 2NO(g) + O_2(g) A pressure of 0.89 atm of NO_2 is introduced into a container and allowed to ...
- Ammonia (NH_3) can be formed from nitrogen and hydrogen from the following balanced equation: N_2(g) + 3 H_2(g) \rightarrow 2 NH_3(g) Assuming that all gases are at the same temperature and pressure, calculate how many milliliters of hydrogen gas are ne
- Ammonia, NH3, is synthesized commercially from nitrogen gas and hydrogen gas at high temperature and pressure. What is the limiting reactant when 6 N2 molecules and 15 H2 molecules are mixed? H2 Bot
- I need to see the problem solved! The answer is 0.61 but I can't seem to get that answer. Show all work! Nitrogen gas reacts with hydrogen gas to form ammonia gas. N_2(g) + 3 H_2 =>2NH_3 (g) The re
- Ammonia will decompose into nitrogen and hydrogen at high temperatures. An industrial chemist studying this reaction fills a 75.0 L tank with 29 mole of ammonia gas at 35.0^\circ C. He then raises the temperature, and when the mixture has come to equilibr
- Nitrogen dioxide decomposes according to the reaction given below where K_p = 4.48 times 10^{-13} at a certain temperature. 2 NO_2(g) rightleftharpoons 2 NO(g) + O_2(g). A pressure of 0.51 atm of NO_2 is introduced into a container and allowed to come to
- How many liters of ammonia gas can be formed from the complete reaction of 150 l of hydrogen gas with excess nitrogen gas at 25 degree C and 1 atm? N_2 (g) + 3H_2 (g) \rightarrow 2NH_3 (g)
- Ammonia gas is produced by reacting hydrogen gas with nitrogen gas. To produce 856 g of ammonia gas using air as your source of nitrogen gas, what volume of air is required if the air is introduced at 27 degrees C and 760 mmHg? (The mole fraction of nitro
- As NH3 (g) is decomposed into nitrogen gas and hydrogen gas at constant pressure and temperature, the volume of the product gases collected is twice the volume of NH3 reacted. Explain. As NH3(g) is decomposed into nitrogen gas and hydrogen gas at constant
- Consider the following chemical equation: N2(g) + 3H2(g) yields 2NH3(g). What volumes of nitrogen gas and hydrogen gas, each measured at 11 degC and 0.998 atm, are needed to produce 5.00 g of ammonia?
- If 2.01 moles of nitrogen react with 4.96 moles of hydrogen, what is the maximum volume of ammonia (in L) that can be produced at a pressure of 1.03 atm and 347 K? N2(g) + 3 H2(g) to 2 NH3(g).
- Nitrogen gas with oxygen gas to form Dinitrogen Tetraoxide. N_2(g) + 2O_2(g) to N_2O_4(g) A 17.7 L reacting vessel, initially at 298 K, contains nitrogen at a partial pressure of 337 mm Hg and oxygen gas at a partial pressure of 491 mm Hg. What is the pre
- What volume of ammonia at 7.0 atm and 235 degrees C would you get from 333 g of nitrogen reaction with enough mass of hydrogen?
- What volume of nitrogen at 215 degress celcius and 715 mmHg would be required to react with .100 moles of hydrogen to produce ammonia? N_2+3H_2 \rightarrow 2NH_3
- N_2(g) + 3 H_2(g) -->2 NH_3(g) What volume of ammonia gas at 27 C and at a pressure of 683 tort will be produced from excess nitrogen and 1.5 liters of hydrogen gas measured at the same temperature
- If 2.00 L of nitrogen and 5.00 L of hydrogen were allowed to react, how many litres of NH_3 (g) could form? The condition of the gas collected were 745 mmHg and 22 degree C.
- What volume of nitrogen gas is produced when 53.7 liters of nitrogen monoxide react according to the following reaction? (All gases are at the same temperature and pressure.) nitrogen monoxide(g) + hydrogen(g) nitrogen(g) + water(l). liters nitrogen gas.
- Chlorine and oxygen gases react to form chlorine dioxide gas. Cl2(g) + 2 O2(g) 2 ClO2(g) At a certain temperature and pressure, 0.70 L of Cl2 reacts with 1.4 L of O2. If all the Cl2 and O2 are consu
- If 2.97 moles of nitrogen reacts with 4.96 moles of hydrogen, what is the maximum volume of ammonia (in L) that can be produced at a pressure of 1.01 atm and 327 K? N2(g) + 3H2(g) 2NH3(g).
- Chlorine and oxygen gases react to form chlorine dioxide gas. Cl2(g) + 2 O2(g) 2 ClO2(g) At a certain temperature and pressure, 1.4 L of Cl2 reacts with 2.8 L of O2. If all the Cl2 and O2 are consumed, what volume of ClO2, at the same temperature and pres
- Nitrogen dioxide decomposes according to the following equation, for which K_p = 0.0000196 at a given temperature. 2 NO2(g) Longleftrightarrow 2 NO(g) + O2(g) (a) A pressure of 6 atm of NO_2 is pl
- Some nitrogen gas and hydrogen gas are placed in a 5.00 L container at 500 degrees Celsius. When equilibrium is reestablished, 3.01 moles of N2, 2.10 moles of H2, and 0.565 moles of NH3 are present. Calculate Kc for this reaction at 500 degrees Celsius.
- What volume of ammonia gas will be produced when 1.26 L of nitrogen react completely in the following equation? N_2 + 3H_2 to 2NH_3.
- What is the initial pressure of H_2S(g) in the flask? Express your answer numerically in atmospheres. Ammonium bisulfide, NH_4HS, forms ammonia, NH_3, and hydrogen sulfide, H_2S, through the reaction N...
- Calculate the volume of ammonia gas is produced at STP when 140 g of nitrogen gas reacts with 30 g of hydrogen gas.
- Nitrogen gas and oxygen gas react according to the following equation. Energy + N2(g) + O2(g) arrow 2NO(g) Nitrogen gas and oxygen gas are placed in a sealed container and are allowed to reach equilibrium. What effect will cooling the system have? A. It w
- Title: Nitrogen gas reacts with hydrogen gas to form ammonia. At 200 C in a closed container, 1.00 atm of nitrogen gas is mixed with 2.00 atm of hydrogen gas. At equilibrium, the total pressure is 2.00 atm. Calculate the partial pressure of hydrogen gas a
- N2 (g) + 3 H2 (g) → 2 NH3 (g) Calculate the volume of ammonia produced at 67 ^oC and 3.49 atm from the complete reaction of 3.48 g of nitrogen with excess hydrogen. - 3.21 L NH3 - 3.97 L NH3 - 11.2 L NH3 - 1.99 L NH3
- Ammonia may be oxidized to nitrogen monoxide in the presence of catalysts according to the equation 4NH_3 + 5O_2 gives 4NO and 6H_2O. If 27 litres of reactants are consumed, what volume of nitrogen monoxide is produced at the same temperature and pressure
- How many liters of ammonia gas can be formed from 11.3 L of hydrogen gas at 93.0 degrees C and a pressure of 42.4 kPa?
- Ammonia gas and carbon dioxide gas react to form aqueous urea (NH2CoNH2) and water. What volume of ammonia at 25 degrees Celcius and 1.5 atm pressure is needed to produce 500 g of urea?
- For the formation of nitrogen dioxide, N O ( g ) + S O 3 ( g ) N O 2 ( g ) + S O 2 ( g ) K f = 1.18 x 10 2 a t 460 o C In a certain experiment, the original partial pressures of NO and S O 3 are 0.025 atm. What is the partial pressure of N O
- What will be the volume of ammonia formed from 2 L of nitrogen and 2 L of hydrogen at constant temperature and pressure?
- Assuming all gases are at the same temperature and pressure, how many milliliters of hydrogen gas must react to give 49.0 mL of NH_3? Consider the reaction: 3H_2(g) + N_2(g) to 2NH_3(g).
- Assuming all gases are at the same temperature and pressure, how many milliliters of hydrogen gas must react to give 41.0 mL of NH_3? The reaction is: 3H_2(g) + N_2(g) to 2NH_3(g).
- What volume of nitrogen gas can be produced from he decomposition of 37.6 L of ammonia with both gases measured at 725 degree C and 5.05 atm pressure? What total volume of gas at 667 degree C and 11.
- N_2 + 3H_2 to 2 NH_3 What volume of ammonia at STP is produced if 25.0 g of nitrogen gas is reacted with an excess of hydrogen gas?
- The synthesis of ammonia gas (NH_3) from nitrogen gas (N_2) and hydrogen gas (H_2) is a major commercial reaction carried out at high temperature and pressure, which of these gases should behave the least like an ideal gas in this reaction? Van der Waals
- A steel cylinder nitrogen, hydrogen, and ammonia gases is at 500 degrees C and 5.00 atm. If the partial pressure of nitrogen is 1850 mm Hg and hydrogen is 1150 mm Hg, what is the partial pressure of ammonia in mmHg?
- A sample of ammonia, NH_3, is completely decomposed to nitrogen and hydrogen gas. Calculate the partial pressure of hydrogen if the total pressure after the reaction is 741 Torr.
- If 97.0mL of nitrogen gas reacts with 42.0 mL of oxygen gas, what is the volume of NO_2 produced? Assume all gases are at the same temperature and pressure. N_2(g) + O_2(g) \rightarrow NO_2(g)
- N 2 + 3 H 2 2 N H 3 What volume of ammonia at STP is produced if 25.0 g of nitrogen gas is reacted with an excess of hydrogen gas?
- Nitrogen dioxide decomposes on heating according to the following equation 2NO_2 (g) to 2NO (g) + O_2 (g). When 4 mole of nitrogen dioxide were put into a 1 dm^3 container and heated to a constant tem
- 10 moles of NH3 was placed in a previously evacuated 20 L container. After a sudden temperature rise to 961.4 K, 80% of ammonia dissociated into hydrogen and nitrogen according to the following reaction. 2/3NH3 arrow 1/3N2 + H2 What is the total pressure
- Under certain conditions, ammonia can break down into its component gases. 2NH3(g) arrow N2(g) + 3H2(g) A container starts out with 4.27 moles of ammonia. The ammonia breaks down completely and the resultant gas mixture of nitrogen and hydrogen has a tota
- If 3.02 liters of ammonia react with an excess of oxygen at 500 ^oC and 3 atm pressure, 4NH_3(g) + 5O_2(g) => 4NO(g) + 6H_2O(g) what volume of steam will be produced at the same temperature and pressure?
- N_{2}(g) + 3 H_{2}(g) \leftrightharpoons 2 NH_{3}(g) + Energy For the reaction of nitrogen gas and hydrogen gas to make methane, what stresses (adding or removing NH_{3}, increasing or decreasing pressure, increasing or decreasing temperature, adding or r
- A container contains 5.0 L of nitrogen gas at a temperature of 23 degrees C. It is known that there was 4.0 moles of nitrogen gas put into the container. What pressure will be exerted by N_2 gas. gas laws
- A 24.0-L gas reaction chamber is charged with 65.0 atm of nitrogen gas and 154 atm of hydrogen gas at 200 degrees Celsius. (a) Calculate the initial moles of N2 and H2 gases, respectively, in the reaction chamber before a reaction occurs. (b) Which gas is
Explore our homework questions and answers library
Browse
by subject