3. The reaction 2HCN Phcn = 0.45 atm C₂N₂ + H₂ (K = 0.17) is performed with PC2N2 PH2 = 0.32 atm and a) Is reaction at equilibrium? b) If not, which way will it shift? c) What will the equilibrium pressures be? 4. Which direction would the reaction 4NH, + 30, 2N₂ + 6H₂Q (AH-1530 kJ) shift if:
3. The reaction 2HCN Phcn = 0.45 atm C₂N₂ + H₂ (K = 0.17) is performed with PC2N2 PH2 = 0.32 atm and a) Is reaction at equilibrium? b) If not, which way will it shift? c) What will the equilibrium pressures be? 4. Which direction would the reaction 4NH, + 30, 2N₂ + 6H₂Q (AH-1530 kJ) shift if:
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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Q3
![of the Clements
3. The reaction 2HCN
PHcx = 0.45 atm
a) Is reaction at equilibrium?
C₂N₂ + H₂ (K = 0.17) is performed with PC2N2 = P2 = 0.32 atm and
b) If not, which way will it shift?
c) What will the equilibrium pressures be?
4. Which direction would the reaction 4NH3 + 30₂ 2N₂ + 6H₂O (AH = -1530 kJ) shift if:
a) N₂ is added b) pressure is lowered c) temperature is raised d) O₂ is removed
5. Label the conjugate acid-base pair for each of the following:
a) HNO, + OH = NO; + H,O b) C,H,NH, +CH,CO; =CH,NH, +CH,CO,H
6. Calculate the pH of the following solutions:
a) 5.2 x 104 HNO3
b) 0.11 M solution of HC,H,O, (K = 8.0 x 10¹5)
7. A 0.10 M solution of NaOH is used to titrate 20 mL of 0.18 M HCHO₂ (K = 1.8 x104):
a) What volume of NaOH is required to reach the equivalence point?
b) What is the pH at the midpoint of the titration?
c) What is the pH at the equivalence point?
8. A buffer is made by adding 8.5 grams of formic acid (HCHO₂, K = 1.9 x 104) to 0.2 moles of its
conjugate base in 500 mL of water.
a) What is the pH of the buffer?
b) What will the pH be after 0.02 moles of NaOH, a strong base, are added?
9. What is the maximum concentration of A1³+ which can exist in a solution with a pH of 9.7 (Ksp Al(OH)
= 2 x 10-³¹)?
10. The compound MgF₂ has K= 7 x 10-¹¹. What is the solubility of MgF₂ in pure water?
11: For each of the following; give the name, geometry, coordination number for the central cation and
draw and identify any possible isomers:
a) [Cr(CN),(H₂O)]²-
b) [Ni(H₂O)₂Br₂]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7120606c-99fa-4a80-8ac4-42c015833f0a%2F91c78f05-a0c1-4f0c-8dad-36e56a5234bb%2Fjxxagibn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:of the Clements
3. The reaction 2HCN
PHcx = 0.45 atm
a) Is reaction at equilibrium?
C₂N₂ + H₂ (K = 0.17) is performed with PC2N2 = P2 = 0.32 atm and
b) If not, which way will it shift?
c) What will the equilibrium pressures be?
4. Which direction would the reaction 4NH3 + 30₂ 2N₂ + 6H₂O (AH = -1530 kJ) shift if:
a) N₂ is added b) pressure is lowered c) temperature is raised d) O₂ is removed
5. Label the conjugate acid-base pair for each of the following:
a) HNO, + OH = NO; + H,O b) C,H,NH, +CH,CO; =CH,NH, +CH,CO,H
6. Calculate the pH of the following solutions:
a) 5.2 x 104 HNO3
b) 0.11 M solution of HC,H,O, (K = 8.0 x 10¹5)
7. A 0.10 M solution of NaOH is used to titrate 20 mL of 0.18 M HCHO₂ (K = 1.8 x104):
a) What volume of NaOH is required to reach the equivalence point?
b) What is the pH at the midpoint of the titration?
c) What is the pH at the equivalence point?
8. A buffer is made by adding 8.5 grams of formic acid (HCHO₂, K = 1.9 x 104) to 0.2 moles of its
conjugate base in 500 mL of water.
a) What is the pH of the buffer?
b) What will the pH be after 0.02 moles of NaOH, a strong base, are added?
9. What is the maximum concentration of A1³+ which can exist in a solution with a pH of 9.7 (Ksp Al(OH)
= 2 x 10-³¹)?
10. The compound MgF₂ has K= 7 x 10-¹¹. What is the solubility of MgF₂ in pure water?
11: For each of the following; give the name, geometry, coordination number for the central cation and
draw and identify any possible isomers:
a) [Cr(CN),(H₂O)]²-
b) [Ni(H₂O)₂Br₂]
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Step 1: Determine the equilibrium pressures of each species:
VIEWStep 2: Explanation for predict the reaction at equilibrium or not:
VIEWStep 3: a. Calculation for reaction quotient and shift :
VIEWStep 4: C. Calculation for change in reaction:
VIEWStep 5: Calculation for equilibrium pressures:
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