For the following reaction, increasing the pressure will cause the equilibrium t
ID: 704987 • Letter: F
Question
For the following reaction, increasing the pressure will cause the equilibrium to 2NO2(g)=N2O4(g) A) shift to the right towards products B) pressure has no effect on equilibrium C) remain unchanged but the reaction mixture will get warmer D) remain unchanged but the reaction mixture will get coolerThe position of the equilibrium for system where k=4.5x10^-3 can be described as being favored to_____ the concentration of products is relatively ______ A) the right; small B) the right; large C) the left; small D) neither direction; large
Which statement best describes the way a catalyst works? A) it decreases the value Eact B) it decreases the value G. C) it increases the value Eact D) it increases the value H
For the following reaction, increasing the pressure will cause the equilibrium to 2NO2(g)=N2O4(g) A) shift to the right towards products B) pressure has no effect on equilibrium C) remain unchanged but the reaction mixture will get warmer D) remain unchanged but the reaction mixture will get cooler
The position of the equilibrium for system where k=4.5x10^-3 can be described as being favored to_____ the concentration of products is relatively ______ A) the right; small B) the right; large C) the left; small D) neither direction; large
Which statement best describes the way a catalyst works? A) it decreases the value Eact B) it decreases the value G. C) it increases the value Eact D) it increases the value H
A) shift to the right towards products B) pressure has no effect on equilibrium C) remain unchanged but the reaction mixture will get warmer D) remain unchanged but the reaction mixture will get cooler
The position of the equilibrium for system where k=4.5x10^-3 can be described as being favored to_____ the concentration of products is relatively ______ A) the right; small B) the right; large C) the left; small D) neither direction; large
Which statement best describes the way a catalyst works? A) it decreases the value Eact B) it decreases the value G. C) it increases the value Eact D) it increases the value H
Explanation / Answer
Q1. The correct answer is (A) shift to the right towards products
Q2. The correct answer is (C) the left; small
Q3. The correct answer is (A) it decreases the value Eact
Explanation
Q1. In gas phase, initially, an equilibrium is established between NO2 and N2O4 molecules when pressure is not varied. After increasing the pressure to a new value, the system is no longer at equilibrium. Now, in accordance to Le Châtelier’s Principle, the chemical equilibrium will shift in a direction that partially undoes the effects of the pressure increase. That means it will shift in the direction of more N2O4 to undo the increase of the pressure in the system. The pressure decreases as more N2O4 is formed, because the total number of molecules decreases. From ideal gas law (PV = nRT), pressure of a gas is directly proportional to number of moles (or molecules) present.
Q2. Equilibrium constant k is ratio of forward rate of reaction to backward rate of reaction. When k < 1, this means rate of backward reaction is more as compared to rate of forward reaction which means reaction proceeds more towards reactant side or in other words, left side
Q3. A catalyst works by providing an alternate pathway which has a less activation energy but all other thermodynamic variables like gibbs free energy (G) and enthalpy (H) remain same as compared to when catalyst is not there in reaction. Hence catalyst decreases the activation energy.
Related Questions
drjack9650@gmail.com
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.