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Chapter 16: Q16.59P (page 731)

For the reaction , how many unique collisions between A and B are possible if 1.01 mol of A(g) and 2.12 mol of B(g) are present in the vessel?

Short Answer

Expert verified

There are 7.46×1047possible collisions between particles A and B.

Step by step solution

01

The number of A and B particles

A material has 6.022×1023particles per mole. Then, as follows, calculate the number of particles in 1.01 moles ThenumberofAparticles=1.01molA×6.022×1023AmolA=6.08222×1023A

Determine the number of particles in 2.12 moles B in the same way:

ThenumberofBparticles=2.12molB×6.022×1023BmolB=12.76664×1023B

02

The number of unique collision between A and B

To find the number of distinct collisions between A and B, multiply the number of particles of each:

Thenumberofuniquecollision=6.08222×1023×12.76664×1023=7.46×1047

As a result, there are 7.46×1047possible collisions between particles A and B.

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Most popular questions from this chapter

Even when a mechanism is consistent with the rate law, later work may show it to be incorrect. For example, the reaction between hydrogen and iodine has this rate law: rate=k[H2][I2] . The long-accepted mechanism had a single bimolecular step; that is, the overall reaction was thought to be elementary:

H2(g)+I2(g)→2HI(g)

In the 1960s, however, spectroscopic evidence showed the presence of free I atoms during the reaction. Kineticists have since proposed a three-step mechanism:

(1)I2(g)⇌2I(g)[fast](2)H2(g)+I(g)⇌H2I(g)[fast](3)H2I(g)+I(g)⇌2HI(g)[slow]

Show that this mechanism is consistent with the rate law.

The rate law for the general reaction

aA+bB+...→cC+dD+...

is rate =k[A]m[B]n...

(a) Explain the meaning of k.

(b) Explain the meanings of m and n. Does m a and n b? Explain.

(c) If the reaction is first order in A and second order in B, and time is measured in minutes (min), what are the units for k?

What is the central idea of collision theory? How does this idea explain the effect of concentration on reaction rate?

Nitrification is a biological process for removing NH3from wastewater as NH4+:

NH4++2O2→NO3-+2H++H2O

The first-order rate constant is given as

K1=0.47e0.095(T°C-15°C)

WhereK1 is inday-1 and T is in°C

  1. If the initial concentrationNH3is 3.0mol/m3, how long will it take to reduce the concentration to 0.35mol/m3in the spring (T =20°C)?
  2. In the winter (T = 10°C)?
  3. Using your answer to part (a), what is the rate ofO2 consumption?

Explain why the coefficients of an elementary step equal the reaction orders of its rate law but those of an overall reaction do not.
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