4 nh 3 g 5 o 2 g 4 nog 6 h 2 og suppose this reaction

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4 NH 3 (g) + 5 O 2 (g) ® 4 NO(g) + 6 H 2 O(g) Suppose this reaction is carried out in the apparatus shown below. When the valve separating the bulbs is opened, the gases mix and the reaction goes to completion. Assume that the final volume is 3.00 L and the temperature is constant throughout the process. Calculate the partial pressure of each of the gases that will be present when the reaction is completed. (HINT: As long as all 4 substances are gases, the result does not depend on the temperature.) T is constant, so n is proportional to PV. So I am going to work this out using L atm in place of moles – I did a problem like this in class, and I hope a number of them will realize that is the easiest way. It also works if you pick a T as long as you use the same T throughout. At the start, we have 1.00 L atm of NH 3 and 1.50 L atm of O 2 . Comapring with the 5:4 ratio in the reaction, we can see that the NH 3 will be the LR. That means at the end we will have products (NO and H 2 O) present along with left over O 2 . ࠵? ࠵? ࠵?࠵?࠵? ࠵?࠵? ࠵? × ࠵? ࠵?࠵?࠵? ࠵?࠵? ࠵? ࠵?࠵?࠵? ࠵?࠵? ࠵? = ࠵? ࠵? ࠵?࠵?࠵? ࠵?࠵? ࠵? ࠵? ࠵?࠵?࠵? ࠵?࠵? ࠵? × ࠵? ࠵?࠵?࠵? ࠵? ࠵? ࠵? ࠵? ࠵?࠵?࠵? ࠵?࠵? ࠵? = ࠵?. ࠵? ࠵? ࠵?࠵?࠵? ࠵? ࠵? ࠵? ࠵? ࠵? ࠵?࠵?࠵? ࠵?࠵? ࠵? × ࠵? ࠵?࠵?࠵? ࠵? ࠵? ࠵? ࠵?࠵?࠵? ࠵?࠵? ࠵? = ࠵?. ࠵?࠵? ࠵? ࠵?࠵?࠵? ࠵? ࠵? ࠵?࠵?࠵?࠵?࠵?, ࠵?࠵? ࠵?. ࠵?࠵? – ࠵?. ࠵?࠵? = ࠵?. ࠵?࠵? ࠵? ࠵?࠵?࠵? ࠵?࠵?࠵?࠵? Divide all those L atm numbers by 3 L total V to get partial P’s: ࠵? ࠵?࠵? = ࠵? ࠵? ࠵?࠵?࠵? ࠵? ࠵? = ࠵?. ࠵?࠵?࠵? ࠵?࠵?࠵? = ࠵?࠵?࠵? ࠵?࠵?࠵?࠵? ࠵? ࠵? ࠵? ࠵? = ࠵?. ࠵? ࠵? ࠵?࠵?࠵? ࠵? ࠵? = ࠵?. ࠵?࠵?࠵? ࠵?࠵?࠵? = ࠵?࠵?࠵? ࠵?࠵?࠵?࠵? ࠵? ࠵? ࠵? = ࠵?. ࠵?࠵? ࠵? ࠵?࠵?࠵? ࠵? ࠵? = ࠵?. ࠵?࠵?࠵? ࠵?࠵?࠵? = ࠵?࠵? ࠵?࠵?࠵?࠵?
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