For the reaction 2NO(g) + O_2(g) = 2NO_2(g), in which direction will a net react

Question

For the reaction 2NO(g) + O_2(g) = 2NO_2(g), in which direction will a net reaction occur if additional NO_2(g) is added to an equal mixture at the same time that the mixture is transferred from a 1-L flask to a 1.5-L flask? a) no changes b) shift open to the left c) shift to the right d) cannot be determined A reaction starts with 1.00 mol each of PCl_3 and Cl_2 in a 1.00 L flask, When Eqm is established in the reaction PCl(g) + Cl(g) = PCl_2(g) =, the amount of PCl_2 present is 0.83 mol, What is K_ for this reaction? a) 25 b) 40.5 c) 44 d) 42.5 Consider the reaction H_2(g) + I_2(g) = K_c = 54.3 at 698 K. If we start with 0.5 mol H_2(*g) and 0.5 mol of l_2(g) in a 5.25-L how many moles of HN(g) will be present at eqm? a) 0.023 b)0.107 c) 2.38 d) 5.77 What is the pH of a 0.052 M NaOH ? a) 1.28 b) 12.72 c) 5.27 d) 11.21 What is the pH of a which is 0.24 M NH_3 and 0.20 M NH_4 Cl? (k_e = 1.8 times 10^-5) a) 10.05 b0 9.34 c) 11.9 d) 11. The eqm constant for the run 2NO_2 - N_2 + O_2 is 2.4 times 10^3. If the initial come of NO_2 is 0.2 M, what are the eqm of NO_2, N_3 and O_2? a) 0.114, 0.3, 0.3 b) 0.004, 0.098, 0.098 v) 1.45, 0.66, 0.66 d) none of the above The lessthanorequalto Chatclier's principal can be applied to any reaction to predict the net direction of changes due to effects of temp, pressure or come. a0 True b) False c) sometimes d) none of the above If the value of conc eqm constant(k_) is known, the partial pressure eqm constant(kp) can be calculate at a specific temp without any knowledge of the stoichiometry

Explanation / Answer

Question 1

We have the reaction:

2NO(g) + O2(g) <-> 2NO2(g)

Note: the double arrow means that the reaction is at equilibrium (the reagents form the product but at the same time the product decomposes into the reagents).

So, if we added more NO2(g) to the reaction, we would add more product and according to Le-Chatelier principle, the equilibrium would shift to reagents, thus, the equilibrium would shift to the left.

Note: Increasing the volume of the flask doesn't affect that much because all reagents and products are gases (considering this transfer is done in vaccum so no oxygen from the air enters the flask).

Thus, the correct answer is B.

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