QUESTION 1
1. |
the reaction will move to the right |
2. |
The reaction will move to the left |
3. |
PCl3 will increase |
4. |
PCl3 will decrease |
5. |
Cl2 will increase |
6. |
Cl2 will decrease |
QUESTION 2
1. |
the reaction will move to the right |
2. |
The reaction will move to the left |
3. |
PCl5 will increase |
4. |
PCl5 will decrease |
5. |
Cl2 will increase |
6. |
Cl2 will decrease |
1. |
the reaction will move to the right |
2. |
The reaction will move to the left |
3. |
PCl5 will increase |
4. |
PCl5 will decrease |
5. |
PCl3 will increase |
6. |
PCl3 will decrease |
QUESTION 4
1. |
the reaction will move to the right |
2. |
The reaction will move to the left |
3. |
Carbon dioxide will increase |
4. |
Carbon dioxide will decrease |
5. |
Bicarbonate ion will increase |
6. |
Bicarbonate ion will decrease |
QUESTION 5
1. |
the reaction will move to the right |
2. |
The reaction will move to the left |
3. |
Carbon dioxide will increase |
4. |
Carbon dioxide will decrease |
5. |
Bicarbonate ion will increase |
6. |
Bicarbonate ion will decrease |
7. |
Hydrogen ion will increase |
8. |
Hydrogen ion will decrease |
1. |
the reaction will move to the right |
2. |
The reaction will move to the left |
3. |
Carbon dioxide will increase |
4. |
Carbon dioxide will decrease |
5. |
Bicarbonate ion will increase |
6. |
Bicarbonate ion will decrease |
QUESTION 1 In the reaction: PCl5 <----> PCl3 + Cl2 When the amount of PCl5 is...
For the reaction PCl3 + Cl2 --> (reversible) PCl5 + heat What will happen to the amount of PCl5 created if heat is removed? What symbol is missing in the following nuclear equation: 2311Na + 21H --> __?__ + 11H HELP!!! Can't get these questions right!
PCl5 decompose into PCl3 and Cl2 when heated. A 0.72-mol sample of PCl5 is put into a 1.00-L vessel and heated. At equilibrium, the vessel contains 0.40 mol of PCl3(g) and 0.40 mol of Cl2(g). Calculate the value of the equilibrium constant for the decomposition this decomposition reaction at this temperature.
Phosphorus pentachloride decomposes at higher temperatures. PCl5(g) ⇄ PCl3(g) + Cl2(g) An equilibrium mixture at some temperature consists of 5.93 g PCl5, 208.23 g/mol 4.86 g PCl3, 137.33 g/mol 3.59 g Cl2, 70.91 g/mol in a 1.00-L flask. If you add 1.31 g of Cl2, how will the equilibrium be affected and what will the concentration of PCl5 be when equilibrium is reestablished? _shift left _shift right _no shift will occur [PCl5] =? mol/L
5. For the reaction: PCl5(g) ⇌ PCl3(g) + Cl2(g), what will happen when the temperature is increased? (Hint: Do you think a decomposition reaction is endothermic or exothermic?)
The equilibrium constant Kp for the reaction PCl5(g) <---> PCl3(g) + Cl2(g) is 1.15 at 25 degrees Celsius. The reaction starts with a mixture of 0.177 atm PCl5, 0.223 atm PCl3, and 0.111 atm Cl2. When this mixture comes to equilibrium at 25 degrees Celsius, what are the equilibrium pressures of each component?
The equilibrium constant Kc for the reaction: PCl3(g) + Cl2(g) PCl5(g) is 490 at 230°C. If 0.70 mol of PCl3 is added to 0.70 mol of Cl2 in a 1.00-L reaction vessel at 230°C, what is the concentration of PCl3 when equilibrium has been established? (show work)
The gas-phase reaction for the production of PCl5 from PCl3 and Cl2 at 250°C has an equilibrium constant Kp of 24.2. 1st attempt Part 1 (1 point)See Periodic Table If the initial pressure of PCl5 in a reaction vessel is 1.41 atm, what is the partial pressure of PCl5 when equilibrium is achieved? atm
Equilibrium for a gas mixture is established according to the reaction: PCl3 (g) + Cl2 (g) ⇌ PCl5 (g) Will the amount of Cl2 present in the system increase when the mixture is expanded to twice the original volume? True or false
Consider the reaction. PCl5(g)↽−−⇀PCl3(g)+Cl2(g)?c=0.0420 PCl 5 ( g ) ↽ − − ⇀ PCl 3 ( g ) + Cl 2 ( g ) K c = 0.0420 The concentrations of the products at equilibrium are [PCl3]=0.270 M [ PCl 3 ] = 0.270 M and [Cl2]=0.180 M [ Cl 2 ] = 0.180 M . What is the concentration of the reactant, PCl5 PCl 5 , at equilibrium? [PCl5]= [ PCl 5 ] =
1) A reaction vessel is found to contain 0.0225 mol PCl3, 0.0181 mol PCl5, and 0.105 mol Cl2. The vessel is at equilibrium and has a volume of 6.18 L. Calculate K eq for the following reaction. PCl5 (g) = PCl3 (g) + Cl2 (g) 2) Consider the following reversible reaction system: FeO (s) + CO (g) = Fe (s) + CO2 (g). At a certain temperature, the equilibrium constant (Kc) for this system is 0.676. The equilibrium concentration of...