0. Calculate the stan 2FES:(s) + 50:(g) → 2FEO(s) +4SO:(g)AH°rn =-1370 kJ 4H for FeO(s)=-268 kJ/mol %D 4H for SO:(g)= -297 kJ/mol; %3D %3D (a) -177 kJ (b) -1550 kJ (c) -774 kJ (d) -686 kJ (e) +808 kJ 7. Calculate the change in the internal energy (4U) for the reaction of Ni with CO, if 158 kJ heat was evolved and 8.68 kJ work was done on the system. (a) -158 kJ Ni(s) +4 CO (g) Ni(CO)«(g) (c) 167 kJ (b) 149 kJ (d) -167 kJ (e) -149 kJ 8. State which of the following sets of quantum numbers would be impossible: (a) n =1,1=0, m = 0, m,= +1/2 (d) n=2, 1=1, m =0, m, = -1/2 (b) n =2, 1= 2, mị =+2, m,= +1/2 (e) n=2, 1=1, m =-1, m, = -1/2 (c) n=3, 1=2, m =+2, m, = -1/2 %3D 9. Which element has the highest first ionization energy? (a) Be (b) B (c) C (d) N (e) O 10 The atom having the valance chell.configuration 4s? 4n would be in:
0. Calculate the stan 2FES:(s) + 50:(g) → 2FEO(s) +4SO:(g)AH°rn =-1370 kJ 4H for FeO(s)=-268 kJ/mol %D 4H for SO:(g)= -297 kJ/mol; %3D %3D (a) -177 kJ (b) -1550 kJ (c) -774 kJ (d) -686 kJ (e) +808 kJ 7. Calculate the change in the internal energy (4U) for the reaction of Ni with CO, if 158 kJ heat was evolved and 8.68 kJ work was done on the system. (a) -158 kJ Ni(s) +4 CO (g) Ni(CO)«(g) (c) 167 kJ (b) 149 kJ (d) -167 kJ (e) -149 kJ 8. State which of the following sets of quantum numbers would be impossible: (a) n =1,1=0, m = 0, m,= +1/2 (d) n=2, 1=1, m =0, m, = -1/2 (b) n =2, 1= 2, mị =+2, m,= +1/2 (e) n=2, 1=1, m =-1, m, = -1/2 (c) n=3, 1=2, m =+2, m, = -1/2 %3D 9. Which element has the highest first ionization energy? (a) Be (b) B (c) C (d) N (e) O 10 The atom having the valance chell.configuration 4s? 4n would be in:
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
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Chapter2: Atoms, Molecules, And Ions
Section: Chapter Questions
Problem 90QAP: Calculate the average density of a single Al-27 atom by assuming that it is a sphere with a radius...
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general chemistry , please solve question 7 And 8
![1. A car is moving with a velocity of 65 km/hr. How many miles would it travel in 35 sec. (1 mile = 1.61 km)
(c) 2.5
(a) 0.39
(b) 1.1
(d) 0.18
(e) 0.56
2. Naturally occurring rubidium consists of two isotopes; 84.912 amu and 86.901 amu. What is the average atomic
weight (amu) of rubidium if the fractional abundance of the heavier isotope is 0.2800?
(a) 85.907
(b) 85.469
(c) 86.021
(d) 85.005
(e) 86.153
3. If a sample of N;Os decomposes to produce 1.381 g O2, how many grams of NO2 are formed? (Molar mass of NO2 =
2N;Oso > 4NO:(g) + O2(g)
(c) 5.520
46.01 g/mol, Oz= 32.00 g/mol).
(b) 3.967
(a)
4.625
(d) 7.942
(e) 1.438
4. What is the net ionic equation for the reaction that occurs when nitric acid is added to copper(II) hydroxide?
2HNO,(aq) +Cu(OH):(s) → Cu(NO3):(aq) + 2H;0()
(a) H"(aq) + OH (aq) HO()
(b) 2H (aq)+ Cu(OH):(s) Cu (aq) + 2H:0()
(c) 2HNO:(aq) +Cu(OH)2(s) Cu(NO:)(aq) + 2H;0()
(d) 2H"(aq) +2N0, (aq) + Cu"(aq)+20H(aq)Cu(NO,)2(aq)+ 2H;0(1)
(e) 2H (aq) + 2NO, (aq)+ Cu (aq) + 20H(aq) Cu"(aq) + 2NO, (aq) + 2H;0(1)
5. If 0.0870 g of a gas occupies 33.6 ml at STP, calculate the molecular mass of the gas
(R= 0.0821 L.atm/K.mol, PV = nRT).
(a) 29.0
(b) 41.2
(c) 58.0
(d) 66.4
(e) 87.0
6. Calculate the standard heat of formation, 4H, for FeS2(s), given the following information:
2FES2(s) + 50:(g)2FEO(s) +4SO2(g)AH°n = -1370 kJ
AH for FeO(s) = -268 kJ/mol
AH for SO(g) = -297 kJ/mol;
(a) -177 kJ
(b) -1550 kJ
(c) -774 kJ
(d) -686 kJ
(e) +808 kJ
7. Calculate the change in the internal energy (4U) for the reaction of Ni with CO, if 158 kJ heat was evolved and 8.68
kJ work was done on the system.
(a) -158 kJ
Ni(s) + 4 CO (g) Ni(CO)«(g)
(c) 167 kJ
(b) 149 kJ
(d) -167 kJ
(e) -149 kJ
8. State which of the following sets of quantum numbers would be impossible:
(a) n =1, 1=0, m = 0, m,= +1/2
(d) n=2, 1=1, m = 0, m, = -1/2
(c) n=3,1=2, m = +2, m, = -1/2
(b) n =2, 1= 2, m = +2, m=+1/2
(e) n=2, 1=1, m =-1, m, = -1/2
9. Which element has the highest first ionization energy?
(a) Be
(b) В
(c) C
(d) N
(e) O
10. The atom having the valence-shell configuration 4s 4p' would be in:
(a) Group 6A and Period 5
(d) Group 7A and Period 4
(b) Group 4B and Period 4
(e) Group 7B and Period 4
(c) Group 6B and Period 7
11. Which of the following electron configurations is wrong:
(a) Mg (Z= 12): Is'2s 2p 3s?
(c) Cu (Z 29): 1s²2s 2p 3s²3p 3d104s'
(e) S (Z = 16): 1s'2s²2p°3s?3p*
(b) Br (Z= 35): [Ar] 3d04s24p
(d) V (Z= 23): [Ar] 3d
1](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F920cf533-1733-4c18-b13a-a1fb71feb791%2F2469d5d6-4dd8-4797-aff7-84d6250327f3%2Fa0ww4dj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1. A car is moving with a velocity of 65 km/hr. How many miles would it travel in 35 sec. (1 mile = 1.61 km)
(c) 2.5
(a) 0.39
(b) 1.1
(d) 0.18
(e) 0.56
2. Naturally occurring rubidium consists of two isotopes; 84.912 amu and 86.901 amu. What is the average atomic
weight (amu) of rubidium if the fractional abundance of the heavier isotope is 0.2800?
(a) 85.907
(b) 85.469
(c) 86.021
(d) 85.005
(e) 86.153
3. If a sample of N;Os decomposes to produce 1.381 g O2, how many grams of NO2 are formed? (Molar mass of NO2 =
2N;Oso > 4NO:(g) + O2(g)
(c) 5.520
46.01 g/mol, Oz= 32.00 g/mol).
(b) 3.967
(a)
4.625
(d) 7.942
(e) 1.438
4. What is the net ionic equation for the reaction that occurs when nitric acid is added to copper(II) hydroxide?
2HNO,(aq) +Cu(OH):(s) → Cu(NO3):(aq) + 2H;0()
(a) H"(aq) + OH (aq) HO()
(b) 2H (aq)+ Cu(OH):(s) Cu (aq) + 2H:0()
(c) 2HNO:(aq) +Cu(OH)2(s) Cu(NO:)(aq) + 2H;0()
(d) 2H"(aq) +2N0, (aq) + Cu"(aq)+20H(aq)Cu(NO,)2(aq)+ 2H;0(1)
(e) 2H (aq) + 2NO, (aq)+ Cu (aq) + 20H(aq) Cu"(aq) + 2NO, (aq) + 2H;0(1)
5. If 0.0870 g of a gas occupies 33.6 ml at STP, calculate the molecular mass of the gas
(R= 0.0821 L.atm/K.mol, PV = nRT).
(a) 29.0
(b) 41.2
(c) 58.0
(d) 66.4
(e) 87.0
6. Calculate the standard heat of formation, 4H, for FeS2(s), given the following information:
2FES2(s) + 50:(g)2FEO(s) +4SO2(g)AH°n = -1370 kJ
AH for FeO(s) = -268 kJ/mol
AH for SO(g) = -297 kJ/mol;
(a) -177 kJ
(b) -1550 kJ
(c) -774 kJ
(d) -686 kJ
(e) +808 kJ
7. Calculate the change in the internal energy (4U) for the reaction of Ni with CO, if 158 kJ heat was evolved and 8.68
kJ work was done on the system.
(a) -158 kJ
Ni(s) + 4 CO (g) Ni(CO)«(g)
(c) 167 kJ
(b) 149 kJ
(d) -167 kJ
(e) -149 kJ
8. State which of the following sets of quantum numbers would be impossible:
(a) n =1, 1=0, m = 0, m,= +1/2
(d) n=2, 1=1, m = 0, m, = -1/2
(c) n=3,1=2, m = +2, m, = -1/2
(b) n =2, 1= 2, m = +2, m=+1/2
(e) n=2, 1=1, m =-1, m, = -1/2
9. Which element has the highest first ionization energy?
(a) Be
(b) В
(c) C
(d) N
(e) O
10. The atom having the valence-shell configuration 4s 4p' would be in:
(a) Group 6A and Period 5
(d) Group 7A and Period 4
(b) Group 4B and Period 4
(e) Group 7B and Period 4
(c) Group 6B and Period 7
11. Which of the following electron configurations is wrong:
(a) Mg (Z= 12): Is'2s 2p 3s?
(c) Cu (Z 29): 1s²2s 2p 3s²3p 3d104s'
(e) S (Z = 16): 1s'2s²2p°3s?3p*
(b) Br (Z= 35): [Ar] 3d04s24p
(d) V (Z= 23): [Ar] 3d
1
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