Homework Answers
Question 5
Balanced equilibrium equation
N2 (g) + 3H2 (g) <=====> 2NH3 (g) + heat
1 + 3 = 4 moles 2 moles
reactants products
A:- decreasing the pressure
Explanation:
If increasing the pressure the equilibrium system will shift towards less number moles side i.e. product side (forward reaction), if decrease the pressure the equilibrium system will shift towards more number moles side i.e. reactant side (backward reaction). So by decreasing the pressure the equilibrium to shift to the left.
Add Answer to:
QUESTION 5 Which change to this reaction system would cause the equilibrium to shift to the...
QUESTION 2 Consider the following reversible reaction at equilibrium: 3H2(g) + N2(g) → 2NH3(g) + heat...
QUESTION 2 Consider the following reversible reaction at equilibrium: 3H2(g) + N2(g) → 2NH3(g) + heat Which of the following changes will shift the equilibrium towards the products (right side)? Decreasing the amount of NH3. Increasing the temperature. Adding a catalyst to the system. Decreasing the amount of H2. Increasing the volume of the system.
For the exothermic reaction 3H2(g) + N2(g) ↔ 2NH3(g) + HEAT, which of the following changes could be carried out to cause the reaction to shift to the right? Adding H2 Adding NH3 Increasing the temp...
For the exothermic reaction 3H2(g) + N2(g) ↔ 2NH3(g) + HEAT, which of the following changes could be carried out to cause the reaction to shift to the right? Adding H2 Adding NH3 Increasing the temperature Removing N2
Question 5 (1 point) Consider the following reaction at equilibrium: 2NH3(g) N2(g) + 3H2(g) Le Châtelier's...
Question 5 (1 point) Consider the following reaction at equilibrium: 2NH3(g) N2(g) + 3H2(g) Le Châtelier's principle predicts that the moles of H2 in the reaction container will increase with O a decrease in the total pressure (T constant) some removal of NH3 from the reaction vessel (V and T constant) an increase in total pressure by the addition of helium gas (V and T constant) a decrease in the total volume of the reaction vessel (T constant) addition of...
Name: 1. An exothermic reaction is allowed to reach equilibrium. If the temperature of the reaction...
Name: 1. An exothermic reaction is allowed to reach equilibrium. If the temperature of the reaction mixture is decreased, the equilibrium will shift towards the product side: True False [1pt] 2. For the reaction C(s) + H2O(g) CO(g) + H2(g) a decrease in concentration of C(s) will cause the reaction to shift to the left oTrue False [1pt] 3. Define the following terms: [1.5pts] a. Activation Energy b. Exothermic Reaction c. Equilibrium [1p) 4. Determine the equilibrium constant K C(s)...
Determine the effect on the equilibrium for the reaction below when the pressure of NH3 is...
Determine the effect on the equilibrium for the reaction below when the pressure of NH3 is increased. N2(g) + 3 H2(g) = 2 NH3(g) AH = -91.8 kJ o a. The reaction will shift to the right. b. There will be no change. c. The reaction will shift to the left. Determine the effect on the equilibrium for the reaction below when the volume of the reaction vessel is increased. N2 (€) + 3H2(g) = 2 NH3(g) AH -91.8 kJ...
1) The reaction below is exothermic 2SO2 (g) + O2(g) = 2803(g) + heat Le Châtelier's...
1) The reaction below is exothermic 2SO2 (g) + O2(g) ⇌ 2SO3(g) + heat Le Châtelier's Principle predicts that _______ will result in an increase in the number of moles of SO3 (g) in the reaction container. Which direction will the reaction shift: ? left or right A) increasing the volume of the container B) increasing the amount of SO2 C) removing some oxygen D) increasing the temperature E) decreasing the pressure 2) Consider the following reaction at equilibrium: 2SO2 (g) + O2 (g) ⇌ 2SO3 (g) + heat ΔH...
The chemical system shown below is at equilibrium. Which change in conditions will not result in...
The chemical system shown below is at equilibrium. Which change in conditions will not result in a spontaneous forward reaction? N2(g) + 3 H2(g) ⇌ 2 NH3(g) Kp = 4 × 105 adding more N2 reducing the pressure reducing the volume decreasing the NH3
Consider the reaction H2(g) + Cl2(g) ⇌ 2HCl(g) which of the following stresses will cause the...
Consider the reaction H2(g) + Cl2(g) ⇌ 2HCl(g) which of the following stresses will cause the reaction shift in the forward direction? a. decreasing the pressure b. removing some HCl(g) c. increasing the pressure d. removing some H2(g) Consider the reaction N2(g)+2O2(g)→2NO2(g), which stress will cause the reaction shift to the left a. increasing the pressure b. removing some NO2(g) c. adding a catalyst d. decreasing the pressure Phenolphthalein is an indicator with a pH range from 8.3 to 10.0....
QUESTION 18 2.5 Choose the incorrect statement regarding the reaction: N2e) 3H2(g)- 2NH3(e) + heat An...
QUESTION 18 2.5 Choose the incorrect statement regarding the reaction: N2e) 3H2(g)- 2NH3(e) + heat An increase in applied pressure will shift the equilibrium to the left. O The addition of ammonia will shift the equilibrium to the left. O The addition of H2 will shift the equilibrium to the right. An increase in temperature will shift the equilibrium to the right QUESTION 19 2.5 Which statement is a correct application of Le Châtelier's principle? The addition of a substance...
Question 16 1 pts Consider the following endothermic reaction at equilibrium: 2NH3(e) <--> N2(g) + 3H)...
Question 16 1 pts Consider the following endothermic reaction at equilibrium: 2NH3(e) <--> N2(g) + 3H) Le Chatelier's principle predicts that adding N2 (g) to the system at equilibrium will result in a decrease in the concentration of NH3 (8) a decrease in the concentration of H2(g) an increase in the value of the equilibrium constant a lower partial pressure of N2 removal of all of the H2(g)
QUESTION 2 Consider the following reversible reaction at equilibrium: 3H2(g) + N2(g) → 2NH3(g) + heat Which of the following changes will shift the equilibrium towards the products (right side)? Decreasing the amount of NH3. Increasing the temperature. Adding a catalyst to the system. Decreasing the amount of H2. Increasing the volume of the system.
Question 5 (1 point) Consider the following reaction at equilibrium: 2NH3(g) N2(g) + 3H2(g) Le Châtelier's principle predicts that the moles of H2 in the reaction container will increase with O a decrease in the total pressure (T constant) some removal of NH3 from the reaction vessel (V and T constant) an increase in total pressure by the addition of helium gas (V and T constant) a decrease in the total volume of the reaction vessel (T constant) addition of...
Name: 1. An exothermic reaction is allowed to reach equilibrium. If the temperature of the reaction mixture is decreased, the equilibrium will shift towards the product side: True False [1pt] 2. For the reaction C(s) + H2O(g) CO(g) + H2(g) a decrease in concentration of C(s) will cause the reaction to shift to the left oTrue False [1pt] 3. Define the following terms: [1.5pts] a. Activation Energy b. Exothermic Reaction c. Equilibrium [1p) 4. Determine the equilibrium constant K C(s)...
Determine the effect on the equilibrium for the reaction below when the pressure of NH3 is increased. N2(g) + 3 H2(g) = 2 NH3(g) AH = -91.8 kJ o a. The reaction will shift to the right. b. There will be no change. c. The reaction will shift to the left. Determine the effect on the equilibrium for the reaction below when the volume of the reaction vessel is increased. N2 (€) + 3H2(g) = 2 NH3(g) AH -91.8 kJ...
QUESTION 18 2.5 Choose the incorrect statement regarding the reaction: N2e) 3H2(g)- 2NH3(e) + heat An increase in applied pressure will shift the equilibrium to the left. O The addition of ammonia will shift the equilibrium to the left. O The addition of H2 will shift the equilibrium to the right. An increase in temperature will shift the equilibrium to the right QUESTION 19 2.5 Which statement is a correct application of Le Châtelier's principle? The addition of a substance...
Question 16 1 pts Consider the following endothermic reaction at equilibrium: 2NH3(e) <--> N2(g) + 3H) Le Chatelier's principle predicts that adding N2 (g) to the system at equilibrium will result in a decrease in the concentration of NH3 (8) a decrease in the concentration of H2(g) an increase in the value of the equilibrium constant a lower partial pressure of N2 removal of all of the H2(g)
Most questions answered within 3 hours.
-
Which of the following would be less likely to be used to
allocate factory overhead when...
asked 3 minutes ago -
Transverse pulses travel with a speed of 195 m/s along a taut
copper wire whose diameter...
asked 1 minute ago -
Sampling for Engineers Homework question 11.51
Suppose that Y1;Y2;Y3;Y4 denote a random sample from a
Poisson(θ)...
asked 5 minutes ago -
Which of the following is cleaved by regulated intramembrane
proteolysis (RIP)? Select any/all answers that apply....
asked 4 minutes ago -
Random characters You decide to create a program characters.py
that fills a two-dimensional list with random...
asked 16 minutes ago -
What are the major sources of error in your determination of the
molar mass? Select all...
asked 20 minutes ago -
A. Suppose your manager indicates that for a normally
distributed data set you are analyzing, your...
asked 41 minutes ago -
During the month of August, the average temperature of a lake
next to a local college...
asked 23 minutes ago -
Which of these four researchers is most likely to have made Type
1 error
Kim who...
asked 37 minutes ago -
In a performance test, each of two cars takes 8.9 s to
accelerate from rest to...
asked 38 minutes ago -
Sapphire Aerospace operates 52 weeks per year, and its cost of
goods sold last year was...
asked 41 minutes ago -
Create ER Model
Assets are resources that are used in CMS to display content.
Each asset...
asked 36 minutes ago