Assuming ideal gas behavior, calculate the mass NH3 (in g) present in the reaction mixture at equilibrium. what is the percent yield of the reaction under theee conditions? Ammonia can be synthesized according to the reaction: N2 (g) + 3H2 (g)= 2NH3 (g) K, = 5.3 x 10-5 at 725 K A 200.0 L reaction container initially contains 1.95 kg of N2 and 0.470 kg of H2 at 725 K.

Assuming ideal gas behavior, calculate the mass NH3 (in g) present in the reaction mixture at equilibrium. what is the percent yield of the reaction under theee conditions? Ammonia can be synthesized according to the reaction: N2 (g) + 3H2 (g)= 2NH3 (g) K, = 5.3 x 10-5 at 725 K A 200.0 L reaction container initially contains 1.95 kg of N2 and 0.470 kg of H2 at 725 K.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: "Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas…

A: Initial moles of CO = 5.8 mol

Q: Methanol and oxygen react to form carbon dioxide and water, like this: 2 CH;OH(1)+3…

A: We have given the Masses of reactant and product as follow Mass of CH3OH = 4.49g Mass of O2 = 2.90 g…

Q: A sample of nickel carbonyl, Ni(CO)4, is placed in a vessel and allowed to reach equilibrium.…

A: Given, Ni(CO)4(g) <---> Ni(s) + 4 CO(g) Reactant gaseous product…

Q: Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S,(g)+C(s) =…

Q: Carbon disulfide and chlorine react according to the following equation: CS2(g) + 3C12(g) =S2C12(g)…

A: Calculate amount of Cl2 at equilibrium?

Q: N,(g)+3H,(g)- 12NH,(g) Complete the table below, so that it lists the initial molarity of each…

A: Molarity is defined as number of solute present in 1000 ml of solution . Mole=…

Q: 2X₂Y3 = 2X₂ + 3Y₂ Keq = 4 x 10° The initial concentration of the reactant is 2 M. Calculate its…

A: The given equilibrium reaction is 2X2Y3 ⇌ 2X2 + 3Y2(g); Keq = 4 × 108 The…

Q: Br₂(g) + Cl₂(g) = 2 BrCl(g) Kp = 1.1 x 10 at 150 K A 203.0 L flask initially contains 1.055 kg of…

A: Given:Volume= 191 mL Mass of Br2 = 1.055 kg Mass of Cl2 = 1.124 kg To calculate:Mass of BrCl…

Q: the equilibrium constant for the gas phase reaction N2(g) + 3H2(g) 2NH3(g) is Kc = 4.34 x 10 ^ -3…

A: Equilibriun constant only depends upon the temperature. But the change in pressure and volume only…

Q: Keq from Equilibrium Composition, Variously Expressed. At some temperature, an equilibrium mixture,…

A: Given, PCl5(g) ⇌PCl3(g) + Cl2(g) Number of molecules of PCl5 = 5.74 × 1020 molecule Moles of PCl3 =…

Q: consider the following reaction (see image) a reaction mixture initally contains 0.50 M CH4 , and…

Q: Carbon dioxide and water react to form methanol and oxygen, like this: 2 CO,(9)+4 H,0(9)→2CH,OH(1)+3…

Q: Suppose a 500. mL flask is filled with 1.3 mol of O, and 0.10 mol of SO3. This reaction becomes…

A: GIVEN: Volume of the Flask = 500 mL= 0.5 L Moles of O2=1.3 mol Moles of SO3 =0.10 mol Given…

Q: Initially, 0.1500 mol of SO3(g) were placed in a 1.00 L reaction vessel, heated to a high…

A: Answer: Decomposition reaction of SO3 is given to us and by forming ICE table we have to find out…

Q: Consider the following reaction: 2 H20(g) + 2 SO2(g) = 2 H2S(g) + 3 O2(g) A reaction mixture…

A: In this question, we want to determine the value of Kc ( Equilibrium constant ) for a given…

Q: 18. À mixture of Û.i0Û moi of H2 and 0.132 moi of CO is piaced in a reaction container and allowed…

A: Given equilibrium is 2H2(g) + CO(g) ⇌ CH3OH(g) Initial moles of H2 = 0.100 mol Initial moles of…

Q: Consider the following reaction: CO (g) + 2 H2 (g) = CH3OH (g) A reaction mixture in a 5.15 L flask…

A: Given: CO (g) + 2 H2 (g) <=> CH3OH (g) Mass of CO = 27.1 g Mass of H2 = 2.32 g Mass of CH3OH…

Q: Consider the reaction: 3 H₂ (g) +N2 (8) 2 NH; (g) AH 91.8 kJ/mol If this reaction is at equilibrium…

A: According to Le Chatelier principle if a system is in equilibrium is subjected to change of…

Q: At a certain temperature, 0.4411 mol of N2 and 1.681 mol of H2 are placed in a 2.5L container.…

A: The equilibrium constant of a chemical reaction gives insight into the relationship between the…

Q: Suppose a 250. mL flask is filled with 0.90 mol of N, and 1.2 mol of NH,. This reaction becomes…

Q: N2(g) + 3H2(g) 2NH3(g) {and the volume is reduced}

A: 1) As we know, by increasing volume equilibrium shifts in the direction where number of gaseous…

Q: "Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas…

A: Answer:Given reaction:In the reaction, 2 moles of gases (1 mole CO and 1 mole H2O) are forming 2…

Q: Methanol and oxygen react to form carbon dioxide and water, like this: 2CH,OH(1)+30,(g)-2…

Q: Iron(III) oxide and hydrogen react to form iron and water, like this: Fe₂O3(s) + 3 H₂(g) 2 Fe(s)+ 3…

A: The reaction given isSince the concentration of solid components are not considered in equilibrium…

Q: "Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas…

A: Equilibrium constant is calculated by taking the ratio of equilibrium concentration of product to…

Q: Suppose a 500. mL flask is filled with 0.20 mol of NO, and 1.3 mol of NO. This reaction becomes…

A: Dear student this question is related to equilibrium concentration.

Q: 1.00 g each of CO, H2O, and H2ar4e sealed in a 1.41 L vessel and brought to equilibrium. How many…

A: Equilibrium is the most stable state for a equilibrium reaction.

Q: A mixture of 0.10 mole NO, 0.050 mole H₂, and 0.10 mole H₂O is placed in a 2.0 L vessel. The…

A: Given -> Initial mole of NO = 0.10 mole Initial mole of H2 = 0.050 mole Initial mole of H2O =…

Q: At 30 degrees Celsius the Kc for 2CO(g) + O2(g) = 2CO2(g) is 2.24 x 1022. Predict in which direction…

Q: Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO2(g)+…

Q: Consider the following equilibrium: N₂O4(8) 2NO2(g) A 1.00 L container is initially filled with…

A: Volume of container = 1.0LInitially filled amount of N2O4(g) = 0.200 molAmount of NO2(g) at…

Q: At a certain temperature, 0.760 mol SO, is placed in a 1.50 L container. 2 SO, (g) =2 SO,2(g) +…

A: 2SO3 (g) = 2SO2 (g) + O2 (g) Kc = [SO2]2[O2]/[SO3]2

Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

Assuming ideal gas behavior, calculate the mass
NH3 (in g) present in the reaction mixture at
equilibrium. what is the percent yield of the reaction
under theee conditions?
Ammonia can be synthesized according to the
reaction:
N2 (g) + 3H2 (g)= 2NH3 (g)
K, = 5.3 x 10-5 at 725 K
%3D
A 200.0 L reaction container initially contains 1.95
kg of N2 and 0.470 kg of H2 at 725 K.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Suppose a 500. mL flask is filled with 0.30 mol of SO, and 1.2 mol of SO3. This reaction becomes possible: 2SO, (g) +O,(g) 2SO3 Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of O,. You can leave out the M symbol for molarity. so, SO2 O2 initial change equilibrium
Keq from Equilibrium Composition, Variously Expressed. At some temperature, an equilibrium mixture, in a 1.00-L container, involving the chemical system PCI5(g) = PCI3(g) + Cl2(g) is found to contain 5.74x1020 molecules of PCI5, 0.00921 mol of PCI3, and 0.228 g of Cl2. Calculate the equilibrium constant (Keg expressed in terms of the molar concentrations) at this temperature. (No units required.)
Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO₂(9)+H₂O(1)→2 HNO3(aq) + NO(g) At a certain temperature, a chemist finds that a 4.4 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound amount NO₂ 10.6 g H₂O 138.4 g HNO3 21.8 g NO 19.6 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. с K = [] x10 ×
Consider the following equilibrium. N2(s) + O2(g) 2 NO(g) At 2300 K, the equilibrium constant K - 1.7 x 10. Suppose that 0.015 mol NO(g), 0.16 mol N, (9), and 0.16 mol O, (9) are placed into a 10.0 L flask and heated to 2300 K. (a) Is the system at equilibrium? If the system is not at equilibrium, in which direction must the reaction proceed to reach equilibrium? The system is at equilibrium. OThe system is not at equilibrium. The reaction must proceed to the left. The system is not at equilibrium. The reaction must proceed to the right (b) Calculate the equilibrium concentrations of all three substances. (Enter unrounded answers.) [02 - [NO M
Consider the following reaction. 2 NO₂(g) = N₂O4(g) 4 When the system is at equilibrium, it contains NO₂ at a pressure of 0.860 atm, and N₂O at a pressure of 0.0740 atm. The volume of the container is then reduced to half its original volume. What is the pressure of each gas after equilibrium is reestablished? atm PNO₂ = atm PN₂0₁ =
Suppose a 500. mL flask is filled with 1.4 mol of N, and 1.3 mol of NO. This reaction becomes possible: N,(2) +0,(2)- -2NO(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of N,. You can leave out the M symbol for molarity. N2 O2 NO initial change equilibrium olo
For the following reaction 2 SO2(g) + O2(g) <-> 2 SO3(g) + heat If the equilibrium situation is stressed by increasing the volume of the container, the reaction will shift toward a No change b Right or products c Left or reactants
After equilibrium is reached in the reaction of 6.30 g H2 with 150. g I2, analysis shows that the 1.00 L flask contains 64.0 g of HI. How many moles of H2, I2, and HI are present in this equilibrium mixture? What is the Keq for this reaction?
O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant Suppose a 250. mL flask is filled with 1.8 mol of NO3 and 1.1 mol of NO2. The following reaction becomes possible: NO₂(g) + NO(g) + 2NO₂(g) The equilibrium constant K for this reaction is 0.707 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places. M × S 1/5
Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide. A chemical engineer studying this reaction fills a 100L tank with 27. mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 9.0 mol of nitrogen dioxide gas. The engineer then adds another 6.8 mol of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the moles of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits. mol