10)The following reaction is exothermic. Which of the following will drive the reaction to theright (towards products)?CH4(g) +20₂(g) = CO₂(g) + 2 H₂O(g)A) A decrease in temperatureB) An increase in temperatureC) The removal of CH4D) The addition of CO

Le-chaterlier's principle: If reaction is reversed and at equilibrium and is subjected to change in…

10). The following reaction is exothermic. Which of the following will drive the reaction to the right (towards products)? CH4(g) + 2O2(g) =CO2(g)+2 H2O(g) A) A decrease in temperature B) An increase in temperature C) The removal of CH4 Jie

10). The following reaction is exothermic. Which of the following will drive the reaction to the right (towards products)? CH4(g) + 2O2(g) =CO2(g)+2 H2O(g) A) A decrease in temperature B) An increase in temperature C) The removal of CH4 Jie

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...

See similar textbooks

Related questions

Q: What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00…

Q: 2.A sealed container initially containing 2 moles of CO gas and 3 moles of H2 gas went through the…

A: Moles of CO=2mol Moles of H2 gas=3mol Moles of CH3OH=1mol

Q: Dinitrogen trioxide decomposes to NO and NO2 in an endothermic process (ΔrH= 40.5 kj/mol-rxn). N2O3…

A: The objective of the question is to predict the effect of adding more NO2 on the position of the…

Q: 4. In a container at 2000°C, carbon dioxide decomposes into carbon monoxide and oxygen gas. The…

A: In the given question we have to identify whether the system is at equilibrium or not and if it is…

Q: Predict the direction of the reaction; consider the equation: CO(g) + H2O(g) (double arrow) CO2(g) +…

Q: Given this unbalanced reaction, how does the system respond when the reaction vessel includes a…

A: The given reaction is as follows: CO2 (g) + H2O (l) ⇔ C6H12O (s) + O2 (g) The effect of removal of…

Q: For the reaction at equilibrium: 2 H2O (g) +2 Cl2 (g) + energy 4 HCI (g) + O2(g), If the [HCI] is…

A: Le Chatelier's principle states that when a system at equilibrium is subjected to an external…

Q: Dinitrogen trioxide decomposes to NO and NO2 in an endothermic process (DHo = + 40.5 kJ/mol)? N2O3…

A: 1) Right 2) Right 3) Left 4) Left 5) LeftExplanation:The given reaction is N2O3⇌NO2+NOand…

Q: Considering the reaction: N2O4 (g) ⇔ 2 NO2 (g) ΔH = negative Which of the following will…

A: Given following equilibrium reaction - N2O4 (g) ⇔ 2 NO2 (g) ΔH = negative It is an…

Q: Consider the reversible reaction shown below. What effect, if any, would each of the following…

A: Note - Since you have posted a question with multiple sub-parts, we are bound to solve only the…

Q: For the following reaction: CO₂ (g) + H₂(g) = CO(g) + H₂O(g) AH = +41.2 kJ Which of the following…

A: Le Chatelier’s Principle: When factors such as concentration, pressure, temperature, inert gases…

Q: The equilibrium 4 NH3(g) + 4 O2(g) ⇆ 2 N2O (g) + 6 H2O(l) ΔHo =…

A: The answer of the above questions are following 1-reducing the volume of the container 2- removing…

Q: 1) For the reaction shown below, at a particular time, the following concentrations are obtained:…

Q: The equation below shows a reaction at equilibrium. What happens to the equilibrium if the…

A: Given reaction : 2NO2(g) <====> N2O4(g) + 58.8 KJ Here , heat energy 58.8 KJ is on product…

Q: For the following reaction in equilibrium, which of the following changes will cause an increase in…

A: Step 1:Step 2:

Q: Given this reaction at equilibrium, C(s) + CO2(g) D 2CO(g) (∆H° = 119kJ), explain the changes that…

A: Given eqm rxn: C(s) + CO2(g) <=> 2CO(g) , ∆H° = 119KJ....... endothermic reaction According…

Q: 3. Which of the following is true for the following system: A⇌B; Kc>>1 Group of answer choices A,…

A: Given : 3. Which of the following is true for the following system: A⇌B; Kc>>1 4.Consider…

Q: Q > K

A: Reaction quotient(Q) is used to determine the direction of the reaction in order to achieve…

Q: For the Haber process given below, which change will shift equilibrium to the left? N2 (g) + 3 H2…

A: Le-Chatelier’s principle states that any change in pressure, volume, moles or temperature is…

Q: true

A: As we know , If we increases the pressure, equilibrium shifts in the direction where the number of…

Q: Dinitrogen trioxide decomposes to NO and NO2 in an endothermic process (ΔrH= 40.5 kj/mol-rxn). N2O3…

A: The objective of the question is to predict the effect of lowering the temperature on the position…

Q: For the reaction shown below, at a particular time, the following concentrations are obtained:…

A: Given data,Molarity of N2O4=2.00MMolarity of NO2=0.20MKc=0.2

Q: For the reaction below, indicate whether the equilibrium tends "to the left", "to the right" or "no…

A: The given reaction is, N2O4 (g) ⇋ 2 NO2 (g) According to Le chatelier's principle if we reduce the…

Q: For the reaction at equilibrium: 2 H2O (g) +2 Cl2 (g) + energy 4 HCI (g) + O2(g), If the [HCI] is…

A: Le Chatelier's Principle states that if a system at equilibrium is disturbed by an external change,…

Q: The reaction quotient for a system is 7.2 × 102. If the equilibrium constant for the system is 36,…

A: Given, reaction quotient, Q = 7.2 × 102 equilibrium constant, Keq = 36 Q > Keq

Q: 5) In the reversible reaction N¿O4 (g) gas is brown. > 2NO2(8), dinitrogen tetraoxide gas is red and…

A: Since you have posted multiple question , as per guidelines we can solve only first . If you want…

Q: For the reaction below, what will be true for the system if [NH3] = 0.30 M, [H2] = 0.15 M, and [N2]…

Q: Please use the values in the resources listed below instead of the textbook values. Nitrogen and…

A: dear student,since you have asked a question which has multiple subparts,according to guidelines we…

Q: Dinitrogen tetraoxide is a colorless gas that dissociates into nitrogen dioxide, a reddish brown…

A: Answer:When a reaction gets started and after passing of time a state is achieved where there is no…

Q: Where is the direction of equilibrium upon removal of NH3 in the reaction below: N2(g) + + 3H₂(g)…

Q: The reaction quotient (Q) for a system is 70. If Kc = 35, what will happen as equilibrium is…

Q: Dinitrogen trioxide decomposes to NO and NO2 in an endothermic process (ΔrH= 40.5 kj/mol-rxn). N2O3…

A: The objective of the question is to predict the effect of adding more N2O3 on the position of the…

Q: Consider the following exothermic reversible reaction at equilibrium: SO3 (g) + NO (g) SO2 (g) + NO2…

A: Le chatelier principle states that equilibrium will shift in such a way so as to undo the effect of…

Q: For the reaction, A(g) + 2B(g) → 3D(g), Kc = 1.50. If at some time, [A]=0.5 M, [B]=0.5 M, and…

A: Reaction Quotient Q = [D]3[A] [B]2 =(0.5)30.5 x (0.5)2 = 1 Q < Kc ; Reaction will proceed in…

Q: Using the equilibrium constants given for reactions (1) and (2), what is the equilibrium constant…

A: Given, three chemical reaction as follows,1) 2NO(g) + O2(g) → N2O4(g) Kp = 1.49 ×1013 2)…

Q: A(s) + B(g) ⇋2 C (g) For each of the statements below, identify whether it is true or false and…

A: a. False Kp = Kc (RT)Δn = Kc (p/v)Δn ∆n = 1 An increase in pressure will decrease the…

Q: For the following endothermic reaction at equilibrium: 2 NOBr(g) 2 NO(g) + Br2(l) choose the action…

A: According to Le Chatelier's principle, equilibrium adjusts forward and backward reactions to adapt…

Q: Which answer does not describe the following reaction? NO (g)+ O2 (g) 2 NO2 (g) The reaction is in…

A: A reaction that is in dynamic equilibrium means that it does not go to completion as both the…

Q: Assume that the following endothermic chemical reaction is at equilibrium. C(s) + H20(g) =H=(g) +…

A: Answer:- This question is answered by using the Le Chatelier principle which involves the change in…

Q: Refer to the following equilibrium reaction: CaCO3(s) CaO(s) + CO2(g) How would the equilibrium…

Q: 6. Consider the equilibrium below: If 1.0 mol of H₂(g) and 2.0 mol I2(g) were placed in a 2.0 L…

A: The objective of the question is to find the equilibrium concentration of HI(g) in a chemical…

Q: Consider the reversible reaction 2 A + B2 22 AB, shown in representation [3] at equilibrium. If…

A: First write the expression for equilibrium constant (K) for the given reaction; K=[AB]2[A2][B2] Now,…

Question

10)
The following reaction is exothermic. Which of the following will drive the reaction to the
right (towards products)?
CH4(g) +20₂(g) = CO₂(g) + 2 H₂O(g)
A) A decrease in temperature
B) An increase in temperature
C) The removal of CH4
D) The addition of CO

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

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

Help
If the reaction quotient, Q, is greater than the equilibrium constant, K, then O the reaction has not yet started in the forward direction. O the forward reaction must be favored. O the reaction will proceed in the forward direction. O the reaction will proceed in the reverse direction. O the reaction has gone to 100% completion and is at equilibrium.
2
The oxidation of ammonia is a reversible exothermic reaction at equilibrium that proceeds as follows: 4 NH3 (g) + 5 O2 (g) ⇋ 4 NO (g) + 6 H2O (g) If a catalyst is added, what happens to the concentration of H2O?
6. Consider the following reaction: SO3(e)* 4.00 moles of SO2 and 5.00 moles O2 are present in a 2.00 L container at 100°C and are at equilibrium. Calculate the equilibrium concentration of SO3 and the number of moles SO3 present if the Keq = 1.47 x 10 3
In which direction (Left, right, or neither direction) would the reaction below have to shift to regain equilibrium, if the reaction was disturbed from the equilibrium by the remove of some SO3 gas? Explain. 2 SO3 (g) -----> 2 SO2 (g) + O2 (g) DeltaH= +198 kJ <------
4
Reactions at Equilibrium • If Keg is very large, the concentration of the products is much greater than the eq concentration of the reactants. The reaction goes to completion. If Keg is very small, the concentration of the reactants is much greater than the eq concentration of the products. The reaction doesn't occur. 4. Consider the two reactions given below. Reaction Equation Picture REACTION A 2 0₂(g) = 3 0₂(g) O O REACTION B N₂(g) + O₂(g) = 2 NO(g) STAR
consider the following reaction at equilibrium. what will happen if O2 is added to the reaction? 4FeS2(s)+11O2(g) 2Fe2O3(s)+8SO2(g) a) the equilibrium will change in the direction of the products b) no change in equilibrium is observed c) the equilibrium constant will increase d) the equilibrium will change in the direction of the reactants e) the equilibrium constant will increase
title=q10a8 What conclusion can you make about the position of equilibrium for the following reaction? A BAG = +1.0 kJ/mol the ratio of B to A will be less than one O the ratio of B to A will be greater than one O the ratio of B toA will be exactly 1 O the ratio of B to A will be exactly -1 O no conclusions can be made about the ratio of B to A from the information given
For the following reaction, CO(g) + H₂O (g) a. Write the Kc expression for this reaction. b. If a 1.00L vessel is charged with 0.190 moles of CO, 0.190 moles of H₂0, 0.250 moles of CO₂, and 0.250 moles of H₂, what is the value of Q? → CO₂ (g) + H₂ (g) Kc = 1.845 c. In which direction does the reaction progress to establish equilibrium? d. What are the equilibrium concentration of all species?
1) For the reaction shown below, at a particular time, the following concentrations are obtained: [CO] = 0.034 M, [CO2] = 3.6 x 10-17 M. Is this reaction at equilibrium? If not, which direction will the reaction proceed and what will the concentrations be at equilibrium? 2 CO (g) C (s) + CO2 (g) K = 7.7 x 10t5