**Quiz Question: Which of these reactions, I or II is exothermic?****Graph Explanations:**- **Graph I:** - **Axes:** The x-axis represents the reaction progress, while the y-axis represents the energy. - **Curve:** The curve begins with a flat line representing the reactants (labeled R). It then rises to a peak, indicating the activation energy required for the reaction. After reaching the peak, the curve descends sharply, ending at a lower energy level, representing the products (labeled P). - **Interpretation:** The products have lower energy than the reactants, indicating that energy is released during the reaction. This reaction is exothermic.- **Graph II:** - **Axes:** The x-axis represents the reaction progress, and the y-axis represents the energy. - **Curve:** The curve starts with a flat line representing the reactants (labeled R). It then rises to a peak, indicating the activation energy required for the reaction. After the peak, the curve descends gradually but then levels off at a higher energy level, representing the products (labeled P). - **Interpretation:** The products have higher energy than the reactants, suggesting that energy is absorbed during the reaction. This reaction is endothermic.**Answer Options:**- O I- O II- O Both are exothermic- O Neither are exothermic**Correct Answer:** I

Exothermic reactions are the reaction in which energy is released.

Answered: Which of these reactions, I or II is…

Which of these reactions, I or II is exothermic? I II R P Reaction progress Reaction progress O I O II O Both are exothermic O Neither are exothermic

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

Similar questions

For the reaction AB2(s) ⇒ A²+ = (aq) + 2 B with Kc (aq) 5.7 x 10-6 If you start with initial concentrations of [A²+] = 2.0 x 10-³ M and [B] = 3.0 x 10-³ M and solid AB2 in which direction will the reaction proceed or is it already at equilibrium? reaction is at equilibrium reaction goes left reaction goes right
Consider the reversible reaction. PCl5↽−−⇀PCl3+Cl2 What substances are present at equilibrium? Cl2Cl2 PCl3PCl3 PCl5PCl5 Are the concentrations of phosphorus pentachloride, PCl5,PCl5, and phosphosphorus trichloride, PCl3,PCl3, constant or changing at equilibrium? The concentrations of both PCl5PCl5 and PCl3PCl3 are changing at equilibrium. The concentrations of both PCl5PCl5 and PCl3PCl3 are constant at equilibrium. The concentration of PCl5PCl5 is constant, and the concentration of PCl3PCl3 is changing at equilibrium. The concentration of PCl5PCl5 is changing, and the concentration of PCl3PCl3 is constant at equilibrium. How does the equilibrium change if more chlorine, Cl2,Cl2, is added to the reaction? The equilibrium shifts to the left. The equilibrium shifts to the right. The equilibrium does not shift to either the left or the right. If more phosphorus pentachloride, PCl5,PCl5, is added, how does the equilibrium change? The equilibrium…
|The three reaction systems (1, 2, and 3) depicted in the accompanying illustration can all be described by the equation 2A=B, where the blue circles are A and the purple ovals are B. Each set of panels shows the changing composition of one of the three reaction mixtures as a function of time. Which system took the longest to reach chemical equilibrium? t2 reaction system 1 reaction system 2 reaction system 3
A+BC<>AB+C WHERE A IS EQUAL TO 50, BC IS EQUAL TO 50, AB IS EQUAL TO 0 AND C IS EQUAL TO 0 What will probablyimmediately happen? 1-AB WILL FORM 2-BC WILL FORM 3- NO REACTION
How does a catalyst influence a chemical equilibrium? Choose from the choices below: It speeds up the rate of the forward and back reactions It changes the position of the equilibrium It speeds up the rate of the back reaction only It speeds up the rate of the forward reaction only
will this reaction happen or not
The following gases are in equilibrium. CO (g) +H2O (g) H2 (2) + CO2 (g) + heat Select all of the ways that you could shift the reaction to the left. Lower the temperature O Add a reactant Add a product Increase the volume of the container O Decrease the volume of the container Raise the temperature Remove a reactant Remove a product
For the following endothermic reaction equilibrium: 2S03 (g) = 2S02 (g) + 02 (g) Decide if each of the following changes will increase the value of K (T= temperature) Yes add S03 No add a catalyst No decrease the volume Yes increase the T No add NE (g) Yes decreased the T Remove S03
Consider the exothermic reaction: C2H4(g) + I2(g) = C2H412(g) In trying to maximize the amount of C2H412 produced, which of the following will not work? Assume that the reaction mixture reaches equilibrium. O increasing the temperature O decreasing the volume of the reaction vessel O increasing the amount of C2H4 O adding more l2
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
Heleppppelppppppppp
Is the forward reaction exothermic or endothermic?