Consider the reaction N2 + O2=2 NO. At 1800 °C, this reaction has an equilibrium constant of 1.2 x 10-4. During the course of the reaction, a
sample of the reaction mixture is taken, and the concentrations of
each component are found to be as follows: [N2] = 0.045 mol dm-3,
[O2] = 0.071 mol dm-3, and [NO] = 0.004 mol dm-3. In which direction
must the reaction proceed for it to reach equilibrium?
=
Select one:
O The reaction is already at equilibrium.
O The reaction must proceed from left to right.
O The reaction must proceed from right to left.
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Will give brainliest it is a lab from k12 here is the linkfor each metal that participated in a chemical change, write the type of metal it is, based on your examination of the periodic table. type your answer here. (score for question 3: of 5 points) were there any metallic compounds that did not react with either the acid or the base? write the type of metal, based on your examination of the periodic table. type your answer here. (score for question 4: of 5 points) make a general statement about the reactivity of the metals in this experiment. type your answer here.

Electric charge is what ? a. kinetic energy b. radiation c. discovery d. electricity

Consider the four elements above. which one of these elements will combine with oxygen in a 1: 1 ratio?