/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Q62 E Complete the changes in concentr... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 13: Q62 E (page 758)

Complete the changes in concentrations (or pressure, if requested) for each of the following reactions.


Short Answer

Expert verified

a)

2H2(g) + O2 (g) 鈬� 2H2O (g)

Change in concentration

-2X

-X

+2X

Change in concentration

-1.50M

1.50M/2 =0.75M

1.50M

b)

CS2 (g) +4H2(g)鈬� CH4 (g) 2H2S(g)

Change in concentration

\[{\rm{+x}}\]

\[+4{\rm{x}}\]

\[-{\rm{x}}\]

\[-2{\rm{x}}\]

Change in concentration

\[0.020{\rm{M}}\]

\[0.020M\cdot4=0.080{\rm{M}}\]

\[-0.020{\rm{M}}\]

\[-0.020M \cdot 2=-0.040{\rm{M}}\]

c)

H2 (g) + cl2 (g)鈬� 2HCl (g)

Change in concentration

+x

+x

-2x

Change in concentration

1.50M

1.50M

-1.50M.2=-3.00M

d)

2NH3(g) + 2O2(g)鈬� N2O (g) 3H2 O(g)

Change in concentration

\[-\frac{{2x}}{3}\]

\[-\frac{{2x}}{3}\]

\[+\frac{x}{3}\]

\[+x\]

Change in concentration

\[-\frac{{60.6{\rm{\;torr\;}}2}}{3}=-40.4{\rm{\;torr\;}}\]

\[-\frac{{60.6{\rm{\;torr\;}}\cdot 2}}{3}=-40.4{\rm{\;torr\;}}\]

\[+\frac{{60.6{\rm{\;torr\;}}}}{3}=+20.2{\rm{\;torr\;}}\]

\[60.6{\rm{\;torr\;}}\]

e)

NH4HS(s)鈬� NH3 (g) + H2S (g)

Change in concentration

\[+{\rm{x}}\]

\[+x\]

Change in concentration

\[9.8\cdot{10^{-6}}{\rm{M}}\]

\[9.8\cdot{10^{-6}}{\rm{M}}\]

f)

Fe(S) + 5CO(g)鈬� Fe(CO)4(g)

Change in concentration

\[{\rm{ - 5x}}\]

\[ + x\]

Change in concentration

\[ - 0.012{\rm{atm}} \cdot 5 = - 0.06{\rm{atm}}\]

\[0.012{\rm{atm}}\]

Step by step solution

01

Definition of change in concentration

The rate of a chemical reaction is defined as the rate of change in concentration of a reactant or product divided by its coefficient from the balanced equation.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Pure iron metal can be produced by the reduction of iron(III) oxide with hydrogen gas.

(a) Write the expression for the equilibrium constant \(\left( {{K_c}} \right.)\)for the reversible reaction

\(F{e_2}{O_3}(s) + 3{H_2}(g) \rightleftharpoons 2Fe(s) + 3{H_2}O(g)\) \(\Delta H = 98.7kJ\)

(b) What will happen to the concentration of each reactant and product at equilibrium if more \(Fe\)is added?

(c) What will happen to the concentration of each reactant and product at equilibrium if \({H_2}O\) is removed?

(d) What will happen to the concentration of each reactant and product at equilibrium if \({H_2}\) is added?

(e) What will happen to the concentration of each reactant and product at equilibrium if the pressure on the system is increased by reducing the volume of the reaction vessel?

(f) What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system is increased?

Write the mathematical expression for the reaction quotient, \({Q_c}\), for each of the following reactions:

(a) \({N_2}(g) + 3{H_2}(g) \rightleftharpoons 2N{H_3}(g)\)

(b) \(4N{H_3}(g) + 5{O_2}(g) \rightleftharpoons 4NO(g) + 6{H_2}O(g)\)

(c) \({N_2}{O_4}(g) \rightleftharpoons 2N{O_2}(g)\)

(d) \(C{O_2}(g) + {H_2}(g) \rightleftharpoons CO(g) + {H_2}O(g)\)

(e) \(N{H_4}Cl(s) \rightleftharpoons N{H_3}(g) + HCl(g)\)

(f) \(2\;Pb{\left( {N{O_3}} \right)_2}(s) \rightleftharpoons 2PbO(s) + 4N{O_2}(g) + {O_2}(g)\)

(g) \(2{H_2}(g) + {O_2}(g) \rightleftharpoons 2{H_2}O(l)\)

(h) \({S_8}(g) \rightleftharpoons 8\;S(g)\)

Question: A reaction is represented by this equation: \({K_c} = 1 \times 1{0^3}\)

(a) Write the mathematical expression for the equilibrium constant.

Calculate the number of moles of \(HI\) that are at equilibrium with \(1.25mol\)of \({H_2}\)and \(1.25\,mol\)of \({I_2}\) in a \(5.00\,L\)flask at \(44{8^0}C\).\({H_2} + {I_2} \rightleftharpoons 2HI\)

\({K_c} = 50.2\,at\,44{8^o}C\)

What is the pressure of \(C{O_2}\)in a mixture at equilibrium that contains \(0.50atm\)\({H_2}\), \(2.0atm\)of \({H_2}O\), and \(1.0atm\)of \(CO\) at \(99{0^0}C\)?

\({H_2}(g) + C{O_2}(g) \rightleftharpoons {H_2}O(g) + CO(g)\)

\({K_P} = 1.6\,at\, 99{0^o}C\)
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Physical Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Chemistry Branches

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.