please help within five minutes

timer Asked: Jan 29th, 2015

Question description

Consider the reaction:

H2O(g) + CO(g) H2(g) + CO2(g)

Which of the following statements are true and which are false.

1.   At equilibrium, individual molecules cannot undergo any chemical reactions.

2.     1 mol of H2O(g) and 1 mol of CO(g) are placed in a vessel and 1 mol of H2(g) and 1 mol of CO2(g) are placed in another of equal volume. At equilibrium, at 350°C, the amounts of H2O(g) in the two vessels are not equivalent.

3.    Amounts of all reactants and products corresponding to an exact equilibrium composition for this reaction are sealed in a vessel. The CO placed in the vessel is labelled with 14C. After an indefinite period of time 14C may be found in both CO and CO2 molecules.

4.    Reactions with large equilibrium constants are always fast.

 5.  At equilibrium, the overall composition of the reaction mixture is changing slowly.

6.   Q = K when the system is at equilibrium.

Identify the relationship between Kp and Kc for each of the following balanced chemical reactions.

NH4Cl(s) NH3(g) + HCl(g)
CaCO3(s) CaO(s) + CO2(g)
C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(g)
SiO2(s) + 4HF(g) SiF4(g) + 2H2O(g)
2NO(g) N2(g) + O2(g)

Tutor Answer

(Top Tutor) Studypool Tutor
School: University of Virginia
Studypool has helped 1,244,100 students
flag Report DMCA
Similar Questions
Hot Questions
Related Tags

Brown University

1271 Tutors

California Institute of Technology

2131 Tutors

Carnegie Mellon University

982 Tutors

Columbia University

1256 Tutors

Dartmouth University

2113 Tutors

Emory University

2279 Tutors

Harvard University

599 Tutors

Massachusetts Institute of Technology

2319 Tutors

New York University

1645 Tutors

Notre Dam University

1911 Tutors

Oklahoma University

2122 Tutors

Pennsylvania State University

932 Tutors

Princeton University

1211 Tutors

Stanford University

983 Tutors

University of California

1282 Tutors

Oxford University

123 Tutors

Yale University

2325 Tutors