Consider the formation of benzene (C6H6) from hexane (C6H14) at 25°C. C6H14(g) C6H6(g) + 4H2(g) The rate of the reaction is 2.5 x 10-4 M/s. Which of the following statements is FALSE? O The rate of formation of benzene is equal to the rate of the reaction. The rate of formation of H2 is equal to the rate of the reaction. O The rate of formation of benzene is equal to the rate of disappearance of hexane. The rate of disappearance of hexane is the same as the rate of the reaction

Consider the formation of benzene (C6H6) from hexane (C6H14) at 25°C. C6H14(g) C6H6(g) + 4H2(g) The rate of the reaction is 2.5 x 10-4 M/s. Which of the following statements is FALSE? O The rate of formation of benzene is equal to the rate of the reaction. The rate of formation of H2 is equal to the rate of the reaction. O The rate of formation of benzene is equal to the rate of disappearance of hexane. The rate of disappearance of hexane is the same as the rate of the reaction

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.96PAE: The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) -* 2 HI(g)...

See similar textbooks

Related questions

Q: Consider the following reaction: 2O3(g)-->3O2(g) The rate law for this reaction is as follows:…

A: Chemical kinetics is the branch of chemistry that mainly deals with the rate of reaction and change…

Q: Consider the hypothetical reaction. X(g) + 2Y(g) → XY2(g) A [Y] -5.0 x 10-2 mol L-1 s-1 At What is…

Q: Consider the following reaction in aqueous solution: 5Br−(??) + BrO3−(??) + 6H+(??) ⟶…

Q: at rate

Q: For the reaction 2Al(s) + 3CuCl2(aq) → 2AlCl3(aq) + Cu(s): If the concentration of aluminum chloride…

Q: Consider the gas phase reaction between H2 and CO: H20(g) + CO(g) --> CO2{g) + H2(g) What is the…

Q: It takes a minute and a half for the concentration of oxygen to decrease from 4.2 x10 2 M to 2.4 x10…

Q: N2(g) + 3H2(g) → 2NH3(g) Suppose that a particular moment during the reaction, molecular…

A: For the given reaction,N2 + 3H2 → 2NH3The expression for the rate of the disappearance of reactants…

Q: (a) Consider the combustion of hydrogen, 2 H21g2 + O21g2 ¡ 2 H2O1g2. If hydrogen is burning at the…

A: When a hydrocarbon reacts with oxygen then, it will form carbon dioxide and water and liberate huge…

Q: Write the rate of reaction in terms of the rate of disappearance of reactant and the rate of…

Q: The oxidation of ammonia produces nitrogen and water via the following reaction: 4NH3(g) + 302(g) →…

A: The correct option is:

Q: Consider the combustion of ether: 1 C4H10O(g) + 6 O2(g) 4 CO2(g) + 5 H2O(g). If CO2 is produced at…

Q: Consider the reaction: N₂ (g) + - 3H₂(g) 2NH₂ (g) Suppose that a particular moment during the…

A: We know that rate of a reaction can be expressed as nA ------> mB (-1/n)d[A]/dt = 1/m d[B]/dt…

Q: Given the following reaction: 2D(g) + 2E(g) + 4F(g) → 4G(g) + 8H(g) What is the rate of the reaction…

A: The rate of a reaction is equal to the change in the concentration of reactants or products per unit…

Q: Consider this reaction: 2N,05 (g) → 2N,0, (g) +O2 (g) At a certain temperature it obeys this rate…

Q: The rate law for the reaction 2NO(g) + 2H₂(g) - N₂(g) + 2H₂O(g) is rate = k[NO]²[H₂] If the rate of…

Q: Time (s) [NO2] (mol/L) 0 0.440 1.55×103 0.418 3.88×103 0.389 5.81×103 0.368 1.16×104 0.317 2.32×104…

Q: A chemical engineer is studying the rate of this reaction. 2N,0, (2) → 2N,0, (g) +0, (g) He fills a…

A: We have to predict the half life, rate constant, concentration after 2 second.

Q: Consider the following reaction: 5Br (ag) + BrO, (aq) + 6H*(aq) → 3Br (aq) + 3H;O() If the rate of…

Q: The reaction between N2O5 and water $$N2O5(g)+H2O(g)2HNO3(g) is a source of nitric acid in the…

Q: The oxidation of ammonia produces nitrogen and water via the following reaction: 4NH3(g) + 302(g) →…

A: The rate of the formation of the product or the rate of consumption of the reactants is known as the…

Q: Consider the balanced reaction below. 2 N2H4(g) + N2O4(g) → 3 N2(g) + 4 H2O(g) a) Write the…

Q: Consider the reaction 5Br−(aq)+BrO−3(aq)+6H+(aq)→3Br2(aq)+3H2O(l) The average rate of…

A: Rate of reaction may be defined as :-The change in any one of the reactants or products per unit…

Q: Consider the reaction 5Br−(aq)+BrO−3(aq)+6H+(aq)→3Br2(aq)+3H2O(l) The average rate of consumption…

Question

Consider the formation of benzene (C6H6) from hexane (C6H14) at 25°C.
C6H14(g) → C6H6(g) + 4H2(g)
The rate of the reaction is 2.5 x 10-4 M/s. Which of the following statements is
FALSE?
The rate of formation of benzene is equal to the rate of the reaction.
O The rate of formation of H2 is equal to the rate of the reaction.
The rate of formation of benzene is equal to the rate of disappearance of hexane.
The rate of disappearance of hexane is the same as the rate of the reaction

2. For the reaction BrOs + 5Br+ 6H* → 3Br. + 3H:O the rate of disappearance of
BrOs is 1.5 x 10-2 M/s at 25°C at a particular instant. What is the rate of
appearance of Br2 at the same instant? *
O 1.5 x 10-2 M/s
4.5 x 10-2 M/s
O 3.0 x 10-3 M/s
O 5.0 x 10-3 M/s

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 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

Ozone, O3, in the Earths upper atmosphere decomposes according to the equation 2 O3(g) 3 O2(g) The mechanism of the reaction is thought to proceed through an initial fast, reversible step followed by a slow, second step. Step 1: Fast, reversible O3(g) O2(g) + O(g) Step 2: Slow O3(g) + O(g) 2 O2(g) (a) Which of the steps is rate-determining? (b) Write the rate equation for the rate-determining step
A study of the rate of dimerization of C4H6 gave the data shown in the table: 2C4H6C8H12 (a) Determine the average rate of dimerization between 0 s and 1600 s, and between 1600 s and 3200 s. (b) Estimate the instantaneous rate of dimerization at 3200 s from a graph of time versus [C4H6]. What are the units of this rate? (c) Determine the average rate of formation of C8H12 at 1600 s and the instantaneous rate of formation at 3200 s from the rates found in parts (a) and (b).
Explain what is meant by the average rate of a reaction.
The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.
How do the rate of a reaction and its rate constant differ?
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 rate of the decomposition of hydrogen peroxide, H2O2, depends on the concentration of iodide ion present. The rate of decomposition was measured at constant temperature and pressure for various concentrations of H2O2and of KI. The data appear below. Determine the order of reaction for each substance, write the rate law, and evaluate the rate constant. Rate [H2OJ [Kll (mL min-’) (mol L ’) (mol L ’) 0.090 0.15 0.033 0.178 0.30 0.033 0.184 0.15 0.066
When every collision between reactants leads to a reaction, what determines the rate at which the reaction occurs?
Consider a hypothetical reaction between A and B: A + B products Use the following initial rate data to calculate the rate constant for this reaction. [A] (mol/L) [B] (mol/L) Initial Rate (mol/L s) 0.20 1.0 3.0 0.50 1.0 11.8 2.0 2.0 189.5
Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following initial rates of reaction have been observed for certain reactant concentrations: [NO] (moI/L1) [CI2] (mol/L) Rate (moI/L/h) 0.50 0.50 1.14 1.00 0.50 4.56 1.00 1.00 9.12 What is the rate equation that describes the rate’s dependence on the concentrations of NO and CI2? What is the rate constant? What are the orders with respect to each reactant?
Isomerization of CH3NC occurs slowly when CH3NC is heated. CH3NC(g) CH3CN(g) To study the rate of this reaction at 488 K, data on [CH3NC] were collected at various times. Analysis led to the following graph. (a) What is the rate law for this reaction? (b) What is the equation for the straight line in this graph? (c) Calculate the rate constant for this reaction. (d) How long does it take for half of the sample to isomerize? (e) What is the concentration of CH3NC after 1.0 104 s?
A friend of yours states, A balanced equation tells us how chemicals interact. Therefore, we can determine the rate law directly from the balanced equations. What do you tell your friend?