1. The oxidation of carbon monoxide proceeds as follows: 2CO(g) + O2(g) 2CO2(g) + 559 kJ Which

Question

Question

1. The oxidation of carbon monoxide proceeds as follows: 2CO(g) + O2(g) 2CO2(g) + 559 kJ Which

1. The oxidation of carbon monoxide proceeds as follows:

2CO(g) + O₂(g) 2CO₂(g) + 559 kJ

Which of the following will cause an INCREASEin the equilibrium concentration of CO?

a. decreasing the pressure of the system at constant temperature

b. adding more O₂to the system

c. removing CO₂from the system as it is formed

d. increasing the pressure of the system at constant temperature

e. adding a catalyst

science chemistry

Add a comment Improve this question Transcribed image text

Answer 1

Answer #1

2CO(g) + O₂(g) ---> 2CO₂(g) + 559 kJ

for the above reaction, $\Delta$ H = -559 KJ , it is an exothermic reaction.

Answer = a. decreasing the pressure of the system at constant temperature

Add a comment

Answer 2

Similar Homework Help Questions

Consider the following reaction at equilibrium. 2CO2 (g) 2CO (g) + O2 (g) ΔH° = -514...

Consider the following reaction at equilibrium. 2CO2 (g) 2CO (g) + O2 (g) ΔH° = -514 kJ Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction ________. A.) at low temperature and low pressure B.) at low temperature and high pressure C.) at high temperature and low pressure D.) in the presence of solid carbon E.) at high temperature and high pressure
Consider the following reaction at equilibrium: 2CO2(g) = 200 (g) + O2(g) AH° = -514 kJ...

Consider the following reaction at equilibrium: 2CO2(g) = 200 (g) + O2(g) AH° = -514 kJ Le Châtelier's principle predicts that a decrease in temperature will decrease the value of the equilibrium constant O increase the value of the equilibrium constant decrease the partial pressure of CO increase the partial pressure of CO2 (g) decrease the partial pressure of O2 (g) Consider the following reaction at equilibrium: 2NH3 (g) = N2 (g) + 3H2(g) AH° = +92.4 kJ Le Châtelier's...
Consider the system at equilibrium. 2 CO(g) +0,(g) = 200,(g) A. How will increasing the concentration...

Consider the system at equilibrium. 2CO(g)+O2(g)<--->2CO2(g)A. How will increasing the concentration of CO shift the equilibrium? B. How will increasing the concentration of Co, shift the equilibrium? C. How will adding a catalyst shift the equilibrium?

Question 1 Glucose metabolism can be represented by the following chemical reaction: C6H12O6(aq)+6O2(g)6CO2(g)+6H2O(l) H for...

Question 1 Glucose metabolism can be represented by the following chemical reaction: C6H12O6(aq)+6O2(g)6CO2(g)+6H2O(l) H for the reaction is -2837 kJ/mole. Is this reaction endothermic or exothermic? Write an expression for the equilibrium constant for this reaction. Given that the value of the equilibrium constant is very large, would you expect this reaction to be fast or slow? Explain the effect on equilibrium of Increasing temperature Increasing pressure by decreasing the volume Decreasing concentration of oxygen Increasing the concentration of...
For the reaction 2CO(g)+O2(g)⇌2CO2(g), the value of K at a certain temperature is 1300. Calculate [CO2]...

For the reaction 2CO(g)+O2(g)⇌2CO2(g), the value of K at a certain temperature is 1300. Calculate [CO2] at equilibrium when [CO] = 9.0×10−2 mol/L and [O2] = 0.527 mol/L
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...

At 1565K, the equilibrium constant for the reactions: (1) 2H2O(g) <----> 2H2(g) +O2(g) and (2) 2CO2(g)...

At 1565K, the equilibrium constant for the reactions: (1) 2H2O(g) <----> 2H2(g) +O2(g) and (2) 2CO2(g) <----> 2CO(g) +O2(g) are 1.6*10^-11 and 1.3*10^-10, respectively. a. what is the value of the equilibrium constant for the reaction: (3) CO2(g) + H2(g) <----> H2O(g) + CO(g) at this temperature? b. demonstrate how the calculations of equilibrium constants matches the calculations of dG0r when adding two reactions or more ; determine dG0r for reactions (1) and (2) and use these values in order...
2 SO2 (g) + O2 (g) = 2 SO3 (g) + Energy Predict the effect of...

2 SO2 (g) + O2 (g) = 2 SO3 (g) + Energy Predict the effect of each of the following changes on the number of moles of S03 present in the mixture at equilibrium Decreasing the volume of the system Adding oxygen to the equilibrium mixture Raising the temperature of the system Decreasing the pressure of the system Adding a catalyst 2 SO2 (g) + O2 (g) = 2 SO3 (g) + Energy Predict the effect of each of the...
1. a) Predict the effect of the following changes on the reaction in which SO3 decomposes...

1. a) Predict the effect of the following changes on the reaction in which SO3 decomposes to form SO2 and O2. 2 SO3(g) → 2 SO2 (g) + O2 (g) delta Ho = 197.78 kJ (1) Increasing the temperature of the reaction. (2) Increasing the pressure on the reaction. (3) Adding more O2 when the reaction is at equilibrium. (4) Removing O2 from the system when the reaction is at equilibrium. b) A person exposed to high levels of carbon...

For the equilibrium system CO (g) + 3 H_2 (g) H_2 O (g) + CH_4 (g),...

For the equilibrium system CO (g) + 3 H_2 (g) H_2 O (g) + CH_4 (g), H = - 206 kJ/mole, state whether the yield of CH_4 will increase, decrease or remain the same for the following changes: Adding some H_2, gas to the system Removing H_2 O from the system Increasing the volume of the system Decreasing the temperature on the system Adding a catalyst to the system

1. The oxidation of carbon monoxide proceeds as follows: 2CO(g) + O2(g) 2CO2(g) + 559 kJ Which

Homework Answers

Add Answer to:
1. The oxidation of carbon monoxide proceeds as follows: 2CO(g) + O2(g) 2CO2(g) + 559 kJ Which

Post as a guest

Earn Coins

Consider the following reaction at equilibrium. 2CO2 (g) 2CO (g) + O2 (g) ΔH° = -514...

Consider the following reaction at equilibrium: 2CO2(g) = 200 (g) + O2(g) AH° = -514 kJ...

Consider the system at equilibrium. 2 CO(g) +0,(g) = 200,(g) A. How will increasing the concentration...

Question 1 Glucose metabolism can be represented by the following chemical reaction: C6H12O6(aq)+6O2(g)6CO2(g)+6H2O(l) H for...

For the reaction 2CO(g)+O2(g)⇌2CO2(g), the value of K at a certain temperature is 1300. Calculate [CO2]...

1) The reaction below is exothermic 2SO2 (g) + O2(g) = 2803(g) + heat Le Châtelier's...

At 1565K, the equilibrium constant for the reactions: (1) 2H2O(g) <----> 2H2(g) +O2(g) and (2) 2CO2(g)...

2 SO2 (g) + O2 (g) = 2 SO3 (g) + Energy Predict the effect of...

1. a) Predict the effect of the following changes on the reaction in which SO3 decomposes...

For the equilibrium system CO (g) + 3 H_2 (g) H_2 O (g) + CH_4 (g),...

1. The oxidation of carbon monoxide proceeds as follows: 2CO(g) + O2(g) 2CO2(g) + 559 kJ Which

Homework Answers

Add Answer to: 1. The oxidation of carbon monoxide proceeds as follows: 2CO(g) + O2(g) 2CO2(g) + 559 kJ Which

Post as a guest

Earn Coins

Add Answer to:
1. The oxidation of carbon monoxide proceeds as follows: 2CO(g) + O2(g) 2CO2(g) + 559 kJ Which