2 moles of H2O(g), 2.6 moles of N2(g), 2.00 moles of H2(g), and 2.00 moles of NO(g) are in equilibrium in a 2 L container. If a second 1L container with 1 mole of H2(g) is combined with the first, what is the initial reaction quotient?

2 H2O(g) + N2(g) <-----> 2 H2(g) + 2NO(g)

Here is the reaction but I'm completely lost.

Question

2 H2O(g) + N2(g) <-----> 2 H2(g) + 2NO(g)

Here is the reaction but I'm completely lost.

Wyatt Atkins · Accepted Answer

#Q_c = 1.15#

We know that the first container is #2# liters in volume, and the one filled with hydrogen is #1# liter, so the combined volume is #color(green)(3# #color(green)("L"#.

And after the #1# #"mol H"_2# is added (from the #1# #"L"#-container), there will now be #3.00# total moles of #"H"_2#.

At this moment, the concentrations of each species are

#"H"_2"O"#: #(2.00color(white)(l)"mol")/(color(green)(3)color(white)(l)color(green)("L")) = 0.667M#

#"N"_2#: #(2.60color(white)(l)"mol")/(color(green)(3)color(white)(l)color(green)("L")) = 0.867M#

#"H"_2#: #(3.00color(white)(l)"mol")/(color(green)(3)color(white)(l)color(green)("L")) = 1.00M#

#"NO"#: #(2.00color(white)(l)"mol")/(color(green)(3)color(white)(l)color(green)("L")) = 0.667M#

For this reaction, the reaction quotient expression is

#Q_c = (["H"_2]^2["NO"]^2)/(["H"_2"O"]^2["N"_2])#

After entering the concentrations mentioned above, our reaction quotient is

#Q_c = ((1.00M)^2(0.667M)^2)/((0.667M)^2(0.867M)) = color(blue)(1.15#

Cameron Andrews · Answer

undefined Initial reaction quotient (Q) is (NO)^2 / (N2)(H2)^3.

2 moles of H2O(g), 2.6 moles of N2(g), 2.00 moles of H2(g), and 2.00 moles of NO(g) are in equilibrium in a 2 L container. If a second 1L container with 1 mole of H2(g) is combined with the first, what is the initial reaction quotient?

2 H2O(g) + N2(g) <-----> 2 H2(g) + 2NO(g) Here is the reaction but I'm completely lost.

2 H2O(g) + N2(g) <-----> 2 H2(g) + 2NO(g)

Here is the reaction but I'm completely lost.