Ammonia and oxygen react to form nitrogen and water, like this: 4 NH,(g)+30,(g) - 2 N2(9)+6H,O(g) Imagine 96. mmol of N, and 288. mmol of H,0 are added to an empty flask, and then answer the following questions. O Zero. What is the rate of the reverse reaction before any N2 or H20 has been added to the flask? O Greater than zero, but less than the rate of the forward reaction. O Greater than zero, and equal to the rate of the forward reaction. O Greater than zero, and greater than the rate of the forward reaction. O Zero. What is the rate of the reverse reaction just after the N2 and H20 has been added to the flask? O Greater than zero, but less than the rate of the forward reaction. O Greater than zero, and equal to the rate of the forward reaction. O Greater than zero, and greater than the rate of the forward reaction. Zero. O Greater than zero, but less than the rate of the forward reaction. What is the rate of the reverse reaction at equilibrium? O Greater than zero, and equal to the rate of the forward reaction. O Greater than zero, and greater than the rate of the forward reaction. O None. O Some, but less than 96. mmol. How much N2 is in the flask at equilibrium? O 96. mmol. O More than 96. mmol.

Ammonia and oxygen react to form nitrogen and water, like this: 4 NH,(g)+30,(g) - 2 N2(9)+6H,O(g) Imagine 96. mmol of N, and 288. mmol of H,0 are added to an empty flask, and then answer the following questions. O Zero. What is the rate of the reverse reaction before any N2 or H20 has been added to the flask? O Greater than zero, but less than the rate of the forward reaction. O Greater than zero, and equal to the rate of the forward reaction. O Greater than zero, and greater than the rate of the forward reaction. O Zero. What is the rate of the reverse reaction just after the N2 and H20 has been added to the flask? O Greater than zero, but less than the rate of the forward reaction. O Greater than zero, and equal to the rate of the forward reaction. O Greater than zero, and greater than the rate of the forward reaction. Zero. O Greater than zero, but less than the rate of the forward reaction. What is the rate of the reverse reaction at equilibrium? O Greater than zero, and equal to the rate of the forward reaction. O Greater than zero, and greater than the rate of the forward reaction. O None. O Some, but less than 96. mmol. How much N2 is in the flask at equilibrium? O 96. mmol. O More than 96. mmol.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 4QAP: Consider the following hypothetical reaction: 2AB2(g)A2(g)+2B2(g)A 500.0-mL flask is filled with...

See similar textbooks

Similar questions

Candle wax is a mixture of hydrocarbons. In the reaction of oxygen with candle w ax in Figure 11.2, the rate of consumption of oxygen decreased with time after the flask was covered, and eventually' the flame went out. From the perspective of the kinetic-molecular theory, describe what is happening in the flask. FIGURE 11.2 When a candle burns in a closed container, the flame will diminish and eventually go out. As the amount of oxygen present decreases, the rate of combustion will also decrease. Eventually, the rate of combustion is no longer sufficient to sustain the flame even though there is still some oxygen present in the vessel.
The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?
11.41 For a drug to be effective in treating an illness, its levels in the bloodstream must be maintained for a period of time. One way to measure the level of a drug in the body is to measure its rate of appearance in the urine. The rate of excretion of penicillin is first order, with a half-life of about 30 min. If a person receives an injection of 25 mg of penicillin at t = 0, how much penicillin remains in the body after 3 hours?
Consider the following hypothetical reaction: 2AB2(g)A2(g)+2B2(g)A 500.0-mL flask is filled with 0.384 mol of AB2. The appearance of A2 is monitored at timed intervals. Assume that temperature and volume are kept constant. The data obtained are shown in the table below. (a) Make a similar table for the disappearance of AB2. (b) What is the average rate of disappearance of AB2 over the second and third 10-minute intervals? (c) What is the average rate of appearance of A2 between t=30 and t=50?
For the reaction 4NO2(g)+O2(g)2N2O5(g) (a) express the rate of formation of N2O5 in terms of the rate of disappearance of O2. (b) suppose the rate of disappearance of O2 is 0.0037 mol L1 s1. Calculate the rate of disappearance of NO2.
The reform reaction between steam and gaseous methane ( CH4 ) produces "synthesis gas," a mixture of carbon monoxide gas and dihydrogen gas. Synthesis gas is one of the most widely used industrial chemicals, and is the major industrial source of hydrogen. Suppose a chemical engineer studying a new catalyst for the reform reaction finds that 526. liters per second of methane are consumed when the reaction is run at 186.°C and 0.36atm . Calculate the rate at which dihydrogen is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits.
If the rate at which O2 appears, ∆3O24>∆t, is 6.0 * 10-5 M>s at a particular instant, at what rate is O3 disappearing at this same time, -∆3O34>∆t?
Consider the following balanced chemical equation. 3O2+C2H5OH⟶3H2O+2CO2 How is the rate of appearance of CO2, Δ[CO2]Δ?, related to the rate of disappearance of O2? −23(Δ[O2]Δ?) −13(Δ[O2]Δ?) −32(Δ[O2]Δ?) 23(Δ[O2]Δ?) 13(Δ[O2]Δ?) 32(Δ[O2]Δ?)
A bimolecular chemical reaction is one in which two chemicals react to form another substance. Suppose that one molecule of each of the two chemicals reacts to form two molecules of a new substance. If x represents the number of molecules of the new substance at time t, then the rate of change of x is proportional to the square of the numbers of molecules of the original chemicals available to be converted. That is, if each of the chemicals initially contained A molecules, then dx dt = k(A − x)2 where k is a constant. If 40% of the initial amount A is converted after 1 hour, how long will it be before 50% is converted? (Give an exact answer. Do not round.)
In the Haber reaction, patented by German chemist Fritz Haber in 1908, dinitrogen gas combines with dihydrogen gas to produce gaseous ammonia. This reaction is now the first step taken to make most of the world's fertilizer. Suppose a chemical engineer studying a new catalyst for the Haber reaction finds that 322. liters per second of dinitrogen are consumed when the reaction is run at 286.°C and 0.16atm. Calculate the rate at which ammonia is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits.
Use the kinetic theory to justify the following observations: (a) the rate of a reaction in the gas phase depends on the energy with which two molecules collide, which in turn depends on their speeds; (b) in the Earth’s atmosphere, light gases, such as H2 and He, are rare but heavier gases, such as O2, CO2, and N2, are abundant.
Nitric oxide, NO, reacts with hydrogen to give nitrous oxide, N2O, and water.2NO(g) + H2(g) ---------> N2O(g) + H2O(g)In a series of experiments, the following initial rates of disappearance of NO wereobtained