Hint:[ (molar mass of H-1, N-14g/mol), (R-0.0821 L.atm/K.mol), (The specific heat of water is 4.184J/g. C) 1) Estimate the temperature where AG=0 for the following reaction: (Given: AH--195 kJ and AS-284.5 J/K) CAUTION: Beware of units.NH3(g) + HCl(g) →→→NH.Cl(s) A) 685 K B) 467 K C) 582 K D) 634 K 2) Consider the reaction represented by the equation: N₂(g) + 3H₂(g) <-> 2NH3(g) Calculate the equilibrium pressures at a certain temperature: PNH,-3.7 x 10 atm, PN-8.9x10 atm, PH-2.9x 10 atm A) 6.3x10* B) 2.9x104 D) 4.9 x10 3) Consider the following reaction: 2 N₂O(g) If the half-life for the reaction is 0.810 s, the rate constant is: A) 1.1 s¹¹ B) 0.86 s¹ Calculate AG for the reaction 4) COO CO2(g) CO + 1/202) A) 523 let C() +1/202) Ca+ O₂ -> CO₂(g) C) 5.3x10* 2 NO(g) + O2(g); rate=k[N₂0] C) 0.69 s¹ AG=?? AG-454.4 kJ AG-257.2 kl D) 0.32 ¹

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...
icon
Related questions
Question
Q 3 and Q 4 please
Hint: (molar mass of H-1, N-14g/mol), (R-0.0821 L.atm/K.mol), (The specific heat of water is 4.184J/g. C)
.
1) Estimate the temperature where AG=0 for the following reaction: (Given: AH--195 kJ and
AS-284.5 J/K) CAUTION: Beware of units.NH3(g) + HCl(g)->NH4Cl(s)
A) 685 K
B) 467 K
C) 582 K
D) 634 K
2) Consider the reaction represented by the equation: N₂(g) + 3H₂(g) <-> 2NH3(g) Calculate the
equilibrium pressures at a certain temperature: PNH,-3.7 x 10 atm, PN-8.9x10 atm, PH:-2.9x 10 atm
A) 6.3x10*
B) 2.9x104
C) 5.3x10
D) 4.9 x10
3) Consider the following reaction:
2 N₂O(g)
If the half-life for the reaction is 0.810 s, the rate constant is:
A) 1.1 s¹¹
B) 0.86 s¹
4) Calculate AG for the reaction
->
COⓇ
CO₂(g)
CO
C) + 1/202)
Ca) + O₂
+1/202- CO₂(g)
A) 523 kJ
2 NO(g) + O₂(g); rate=1
C) 0.69 s¹
AG=??
AG°-454.4 kJ
AG=-257.2 kJ
C) 197.2 kJ
k[N₂0]
B)-265.8 kJ
D) 651.6 kJ
5) The volume of a sample of nitrogen N₂ is 9 L at 31°C and 732 torr. What volume will it occupy at STP?
A) 6.59 L
B) 7.18 L
C) 6.90 L
D) 7.78 L
6)
Which of the following pure substances exhibits hydrogen bonding?
A) HCI
B) H₂S
C) CH₂
D) 0.32 s¹
D) H₂O
7)
A particular vinegar solution has a H₂O* concentration of 0.0185 M. What is the pOH of the solution?
A) 10.7
B) 17.3
C) 12.3
D) 15.8
8)
What mass of ethylene glycol (M.W. = 62.1 g/mol) antifreeze must be added to 8.0 liters of water to
produce a solution that freezes at -23.3 C degrees. Density of water is 1 g/ml and Kr-186° C/m.
A) 3.41 g
B) 6.22 Kg
C) 7.81 kg
=
D) 0.78 kg
11) The OH concentration in a 0.09M of Ca(OH)2 solution is
A) 0.0075 M
B) 0.18 M
9) How much heat is required to raise the temperature of 1.5 g of water from 25°C to 27°C?
A) 12.55 kJ
B) 6.27 kJ
C) 1.55 kJ
D) 40.5 kJ
10) Calculate the osmotic pressure associated with 90.0 g of an enzyme of molecular weight 98,000 g/mol
dissolved in 2900 mL of benzene at 30.0 °C.
A) 5.99 torr
B) 1.96 torr
C) 0.484 torr
D) 2.48 torr
C) 1.3x10-12 M
D) 1x107 M
12) A solution of 7.00 MHCHO2 is 0.57% ionized in water. Calculate the Ka value for the acid (HCHO₂).
A) 2.5x10-³
B) 0.2x10-³
C) 2.3x104
D) 0.23
Transcribed Image Text:Hint: (molar mass of H-1, N-14g/mol), (R-0.0821 L.atm/K.mol), (The specific heat of water is 4.184J/g. C) . 1) Estimate the temperature where AG=0 for the following reaction: (Given: AH--195 kJ and AS-284.5 J/K) CAUTION: Beware of units.NH3(g) + HCl(g)->NH4Cl(s) A) 685 K B) 467 K C) 582 K D) 634 K 2) Consider the reaction represented by the equation: N₂(g) + 3H₂(g) <-> 2NH3(g) Calculate the equilibrium pressures at a certain temperature: PNH,-3.7 x 10 atm, PN-8.9x10 atm, PH:-2.9x 10 atm A) 6.3x10* B) 2.9x104 C) 5.3x10 D) 4.9 x10 3) Consider the following reaction: 2 N₂O(g) If the half-life for the reaction is 0.810 s, the rate constant is: A) 1.1 s¹¹ B) 0.86 s¹ 4) Calculate AG for the reaction -> COⓇ CO₂(g) CO C) + 1/202) Ca) + O₂ +1/202- CO₂(g) A) 523 kJ 2 NO(g) + O₂(g); rate=1 C) 0.69 s¹ AG=?? AG°-454.4 kJ AG=-257.2 kJ C) 197.2 kJ k[N₂0] B)-265.8 kJ D) 651.6 kJ 5) The volume of a sample of nitrogen N₂ is 9 L at 31°C and 732 torr. What volume will it occupy at STP? A) 6.59 L B) 7.18 L C) 6.90 L D) 7.78 L 6) Which of the following pure substances exhibits hydrogen bonding? A) HCI B) H₂S C) CH₂ D) 0.32 s¹ D) H₂O 7) A particular vinegar solution has a H₂O* concentration of 0.0185 M. What is the pOH of the solution? A) 10.7 B) 17.3 C) 12.3 D) 15.8 8) What mass of ethylene glycol (M.W. = 62.1 g/mol) antifreeze must be added to 8.0 liters of water to produce a solution that freezes at -23.3 C degrees. Density of water is 1 g/ml and Kr-186° C/m. A) 3.41 g B) 6.22 Kg C) 7.81 kg = D) 0.78 kg 11) The OH concentration in a 0.09M of Ca(OH)2 solution is A) 0.0075 M B) 0.18 M 9) How much heat is required to raise the temperature of 1.5 g of water from 25°C to 27°C? A) 12.55 kJ B) 6.27 kJ C) 1.55 kJ D) 40.5 kJ 10) Calculate the osmotic pressure associated with 90.0 g of an enzyme of molecular weight 98,000 g/mol dissolved in 2900 mL of benzene at 30.0 °C. A) 5.99 torr B) 1.96 torr C) 0.484 torr D) 2.48 torr C) 1.3x10-12 M D) 1x107 M 12) A solution of 7.00 MHCHO2 is 0.57% ionized in water. Calculate the Ka value for the acid (HCHO₂). A) 2.5x10-³ B) 0.2x10-³ C) 2.3x104 D) 0.23
Expert Solution
Step 1

Chemical kinetics can be defined as the branch of chemistry that deals with rates of chemical reactions It tells us about speed of reaction whetther reaction is slow or fast.

steps

Step by step

Solved in 3 steps with 2 images

Blurred answer
Knowledge Booster
Thermodynamics
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY