In the chemical reaction where 0.1 M of N2O4 (g) is converted to 2NO2 (g), what are the concentration values of NO2 (g) in the ICE Table?
N2O4 (g) <-> 2NO2 (g)
A. Initial = 0 M, Change = 2x, Equilibrium = 0 + x
B. Initial = 0 M, Change = x, Equilibrium = 0 + x
C. Initial = 0.1 M, Change = x, Equilibrium = 0.1 M - x
D. Initial = 0 M, Change = 2x, Equilibrium = 0 + 2x
I think the answer should be D. Can someone help me out here.
its D on apex
Dr. Bob bro do you jus purposely give ppl the wrong answers my guy lmaooo it’s asking for NO2 not N2O4. You did the ICE table right but you didn’t read the question carefully smh stop misleading ppl all the time 😂
So the answer is C right. It can't be anything else.
Right. Here is the ICE chart.
......................N2O4 (g) <-> 2NO2 (g)
I.....................0.1...................0
C....................-x.....................2x
E...................0.1-x.................2x
drbob how are you so dumb
To determine the concentration values of NO2 (g) in the ICE table, we can use the stoichiometry of the chemical reaction and the given initial concentration of N2O4 (g).
In the balanced chemical equation:
N2O4 (g) <-> 2NO2 (g)
Let's assume that the initial concentration of N2O4 (g) is 0.1 M.
According to the stoichiometry of the reaction, for every 1 mole of N2O4, 2 moles of NO2 are formed. Therefore, at equilibrium, the concentration of NO2 is twice the concentration of N2O4 that reacts.
Based on this information, let's analyze the answer choices:
A. Initial = 0 M, Change = 2x, Equilibrium = 0 + x
This answer choice assumes an initial concentration of 0 M for N2O4, which is inconsistent with the given information.
B. Initial = 0 M, Change = x, Equilibrium = 0 + x
This answer choice also assumes an initial concentration of 0 M for N2O4, which is inconsistent with the given information.
C. Initial = 0.1 M, Change = x, Equilibrium = 0.1 M - x
This answer considers the initial concentration of N2O4 correctly. However, it assumes that the change in concentration of NO2 is equal to x, which is incorrect. The change in concentration of NO2 should be twice the change in concentration of N2O4 since the stoichiometry is 2:1.
D. Initial = 0 M, Change = 2x, Equilibrium = 0 + 2x
This answer choice assumes an initial concentration of 0 M for N2O4, which is inconsistent with the given information.
Therefore, the correct answer is C. Initial = 0.1 M, Change = x, Equilibrium = 0.1 M - x.
By using this ICE table and considering the stoichiometry of the reaction, you can determine the concentration values of NO2 (g) at equilibrium.
No.
In the chemical reaction where 0.1 M of N2O4 (g) is converted to 2NO2 (g), what are the concentration values of NO2 (g) in the ICE Table?
N2O4 (g) <-> 2NO2 (g)
The problem TELLS you that you start with 0.1 M. So why would you pick anything that starts with 0 M? Doesn't make sense to me. Initial means what you start with. You're starting with 0.1 M. Right?