have a flask filled with phosphorus pentachloride (PCl5) at a high enough temperature that it is entirely in gaseous form. You know that it can decompose into chlorine gas (Cl2) and phosphorus trichloride gas (PCl3) in an equilibrium reaction. You start with 1 atm of PCl5 in your flask. After equilibrium is achieved, you notice that the new total pressure is fifty percent higher than the starting pressure. Your friend is studying the same reaction at the same temperature. She has combined 1 atm of each of the three gases in a flask and is now wondering what will happen.
You have a flask filled with phosphorus pentachloride (PCl5) at a high enough temperature that it is entirely in gaseous form. You know that it can decompose into chlorine gas (Cl2) and phosphorus trichloride gas (PCl3) in an equilibrium reaction. You start with 1 atm of PCl5 in your flask. After equilibrium is achieved, you notice that the new total pressure is fifty percent higher than the starting pressure.
Your friend is studying the same reaction at the same temperature. She has combined 1 atm of each of the three gases in a flask and is now wondering what will happen.
In order to answer the final questions below, it may help to think about the following: What is the equilibrium constant, Kp, of your reaction? What is the value of Q in your friend’s experiment?
Questions
a) Do you predict that the pressure in her (your friend's) flask will go up, go down, or remain the same? Please explain.
b) Do you predict that the molecules in your friend's reaction will generally be “social” (go through synthesis) or “antisocial (go through decomposition)? In other words, will the reaction shift forward or reverse
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