1. The balanced reaction for the combustion of methane;

CH_4(g) + 2O_2(g) --> CO_2(g) + 2H₂O_(l)

Consider mixing 1.50 mol of methane with 1.80 mol of oxygen. Assume there is no carbon dioxide or water present in the initial mixture.

2. Which of the following ICE Tables (I or II) make sense assuming the initial amounts above and that the reaction goes to completion.

Table I: Based on assuming all the CH₄ reacts

Table II: Based on assuming all the O₂ reacts

Table makes the most sense;

briefly explain your reasoning.

3. The balanced reaction for the synthesis of ammonia;

N_2(g) + 3H_2(g) --> 2NH_3(g)

Consider mixing 0.50 mol of nitrogen with 2.10 mol of hydrogen. Assume there is no ammonia present in the initial mixture.

4. Which of the following ICE Tables (III or IV) make sense assuming the initial amounts above and that the reaction goes to completion.

Table III: Based on assuming all the N₂ reacts

Table IV: Based on assuming all the H₂ reacts

Table makes the most sense;

briefly explain your reasoning

5. Write the balanced equation that best describes the change/reaction that occurs in the containers below.

The equation is

6. Is there anything about the questions that you feel you do not understand? List your concerns/questions.

7. If there is one question you would like to have answered in lecture, what would that question be?