C) [N₂0₂]-kt D) 1/[N₂Os] - 1/[N2Os]o + kt 16) Given: N2(g) + 3 H₂(g) <->2 NH3(g) At equilibrium at a certain temperature, the concentration of NH3(g), H₂(g) and N₂(g) are 0.49 M, 1.61 M and 0.14 M, respectively. Calculate the value of Ke for this reaction. A) 1.26 B) 0.612 C) 0.411 D) 1.96 17) Consider the following reaction: LBCLO N₂O5 Joe
C) [N₂0₂]-kt D) 1/[N₂Os] - 1/[N2Os]o + kt 16) Given: N2(g) + 3 H₂(g) <->2 NH3(g) At equilibrium at a certain temperature, the concentration of NH3(g), H₂(g) and N₂(g) are 0.49 M, 1.61 M and 0.14 M, respectively. Calculate the value of Ke for this reaction. A) 1.26 B) 0.612 C) 0.411 D) 1.96 17) Consider the following reaction: LBCLO N₂O5 Joe
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Q 16 please
![11) Calculate the osmotic pressure associated with 90.0 g of an enzyme of molecular weight 98,000 g/mol |
dissolved in 2700 mL of benzene at 30.0 °C.
A) 5.99 torr
B) 1.96 torr
4
C) 6.43 torr
D) 2.48 torr
12) The rate constant for the first order reaction A--> B+C is k-4.4 x 103 min¹ at 57 K. What is the
half-life for this reaction at 57 K?
A) 32 min
C) 9.1 min.
D) 1200 min
13) Consider the following reaction:
If the half-life for the reaction is 0.610 s, the rate constant is:
2 N₂O(g) 2 NO(g) + O2(g); rate = k[N20]
A) 1.14 s¹¹
B) 0.69 ¹
C) 0.86 s¹
B) 16 min.
D) 0.32 s¹
14) The decomposition of N₂Os(g)-NO2(g) + NO(g) proceeds as a first order reaction with a half-life of
30.0 seconds at a certain temperature. If the initial concentration [N2Oslo 0.600 M, what is the
concentration after 120 seconds?
A) 0.038 M
B) 0.100 M
C) 0.400 M
D) 0.013 M
15) Which equation below best gives the concentration of N₂Os versus time in the previous question Q14?
A) [N₂0s] =([N₂Oslo)/t12 B) [N₂0s]-[N₂O3]oek
C) [N₂O₁]=kt D) 1/[N2Os] = 1/[N2Os]o + kt
16) Given: N2(g) + 3 H₂(g) <-> 2NH₂(g)
At equilibrium at a certain temperature, the concentration of NH3(g), H₂(g) and N2(g) are 0.49 M, 1.61 M and
0.14 M, respectively. Calculate the value of Ke for this reaction.
A) 1.26
B) 0.612
D) 1.96
C) 0.411
17) Consider the following reaction: 4 PCI(g)-> P4(g) + 6 Cl₂(g)
If the initial concentration of PCI3(g) is 2.0 M, and "x" is the equilibrium concentration of P4(g), what is the
correct equilibrium relation?
A) Kc = 6x7
B) Ke=6x7/(2.0-x)* C) Ke=x²/(2.0-x)*
18) Consider the reaction represented by the equation: N₂(g) + 3H2(g) <-> 2NH3(g) Calculate the
D) Kc = (x)(6x)/(2.0-4x)"
equilibrium pressures at a certain temperature: PNH₁-2.9 x 10 atm, PN2-89x10¹ atm, PH2-2.7x 10 atm
A) 4.9 x10
B) 2.9x10
D) 7.8x104
C) 6.3x104
55
19) Consider the reaction represented by the equation: Fe" (aq) + SCN (aq) →
FeSCN²+ (aq)
6.00 M Fe³+ (aq) and 10.0 M SCN (aq) are mixed at a certain temperature and at equilibrium
the concentration of FeSCN³+ (aq) is 3 M.
A) 250x10¹
B) 95 x103
20) A particular vinegar solution has a H3O* concentration
A) 17.3
B) 12.1
C) 143x103
D) 303 x10
of 0.013 M. What is the pOH of the solution?
D) 15.8
C) 12.3
21) What is the pH of 42.0 M aqueous solution of NH3 (ammonia). It's Ks- 1.8 x 10³.
A) 12.4
B) 0.0104
C) 0.778
22) The OH concentration in a 0.089M of Ca(OH)2 solution is
A) 0.178 M
B) 0.108 M
D) 1x 10-7 M
23) A solution of 9.00 MHCHO2 is 0.77% ionized in water. Calculate the K. value for the acid (HCHO₂).
A) 2.3x104
B) 5.4x104
C) 0.2x10³
D) 0.23
24) When a weak acid is titrated with a strong base, the pH at the equivalence point is ALWAYS
A) 7
B)<7
C) >7
D) < 1
C) 1.3x10-¹2 M
D) 12.6
25) Which one of these statements about strong acid is true
A) Strong acid produce solutions with a higher pH than weak acids
B) All strong acids have H atom bonded to electronegative oxygen atom
C) Strong acids are very concentrated acids
D) Strong acids are 100% ionized in water](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbfaea92a-9638-4015-ac2a-6c50f8cc86a5%2F5294b64d-3356-4da7-9639-eeb30b31434e%2Fbu9k1vw_processed.jpeg&w=3840&q=75)
Transcribed Image Text:11) Calculate the osmotic pressure associated with 90.0 g of an enzyme of molecular weight 98,000 g/mol |
dissolved in 2700 mL of benzene at 30.0 °C.
A) 5.99 torr
B) 1.96 torr
4
C) 6.43 torr
D) 2.48 torr
12) The rate constant for the first order reaction A--> B+C is k-4.4 x 103 min¹ at 57 K. What is the
half-life for this reaction at 57 K?
A) 32 min
C) 9.1 min.
D) 1200 min
13) Consider the following reaction:
If the half-life for the reaction is 0.610 s, the rate constant is:
2 N₂O(g) 2 NO(g) + O2(g); rate = k[N20]
A) 1.14 s¹¹
B) 0.69 ¹
C) 0.86 s¹
B) 16 min.
D) 0.32 s¹
14) The decomposition of N₂Os(g)-NO2(g) + NO(g) proceeds as a first order reaction with a half-life of
30.0 seconds at a certain temperature. If the initial concentration [N2Oslo 0.600 M, what is the
concentration after 120 seconds?
A) 0.038 M
B) 0.100 M
C) 0.400 M
D) 0.013 M
15) Which equation below best gives the concentration of N₂Os versus time in the previous question Q14?
A) [N₂0s] =([N₂Oslo)/t12 B) [N₂0s]-[N₂O3]oek
C) [N₂O₁]=kt D) 1/[N2Os] = 1/[N2Os]o + kt
16) Given: N2(g) + 3 H₂(g) <-> 2NH₂(g)
At equilibrium at a certain temperature, the concentration of NH3(g), H₂(g) and N2(g) are 0.49 M, 1.61 M and
0.14 M, respectively. Calculate the value of Ke for this reaction.
A) 1.26
B) 0.612
D) 1.96
C) 0.411
17) Consider the following reaction: 4 PCI(g)-> P4(g) + 6 Cl₂(g)
If the initial concentration of PCI3(g) is 2.0 M, and "x" is the equilibrium concentration of P4(g), what is the
correct equilibrium relation?
A) Kc = 6x7
B) Ke=6x7/(2.0-x)* C) Ke=x²/(2.0-x)*
18) Consider the reaction represented by the equation: N₂(g) + 3H2(g) <-> 2NH3(g) Calculate the
D) Kc = (x)(6x)/(2.0-4x)"
equilibrium pressures at a certain temperature: PNH₁-2.9 x 10 atm, PN2-89x10¹ atm, PH2-2.7x 10 atm
A) 4.9 x10
B) 2.9x10
D) 7.8x104
C) 6.3x104
55
19) Consider the reaction represented by the equation: Fe" (aq) + SCN (aq) →
FeSCN²+ (aq)
6.00 M Fe³+ (aq) and 10.0 M SCN (aq) are mixed at a certain temperature and at equilibrium
the concentration of FeSCN³+ (aq) is 3 M.
A) 250x10¹
B) 95 x103
20) A particular vinegar solution has a H3O* concentration
A) 17.3
B) 12.1
C) 143x103
D) 303 x10
of 0.013 M. What is the pOH of the solution?
D) 15.8
C) 12.3
21) What is the pH of 42.0 M aqueous solution of NH3 (ammonia). It's Ks- 1.8 x 10³.
A) 12.4
B) 0.0104
C) 0.778
22) The OH concentration in a 0.089M of Ca(OH)2 solution is
A) 0.178 M
B) 0.108 M
D) 1x 10-7 M
23) A solution of 9.00 MHCHO2 is 0.77% ionized in water. Calculate the K. value for the acid (HCHO₂).
A) 2.3x104
B) 5.4x104
C) 0.2x10³
D) 0.23
24) When a weak acid is titrated with a strong base, the pH at the equivalence point is ALWAYS
A) 7
B)<7
C) >7
D) < 1
C) 1.3x10-¹2 M
D) 12.6
25) Which one of these statements about strong acid is true
A) Strong acid produce solutions with a higher pH than weak acids
B) All strong acids have H atom bonded to electronegative oxygen atom
C) Strong acids are very concentrated acids
D) Strong acids are 100% ionized in water
Expert Solution
Step 1
Here we have to determine the equilibrium constant of the following given reaction
N2(g) + 3H2(g) <=> 2NH3(g)
Given equilibrium concentration of NH3, H2 and N2 are 0. 49M, 1.61M, and 0.14M respectively.
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