Summary:
This lab involves three separate experiments. Before you conduct any of them, however, you should put on goggles and aprons, as well as gloves.
For the first part, place the FeCl3 solution into the watch glass, and add a few drops of KSCN. Record any changes you might see. Then, ask Dr. Karraker to add a KSCN crystal to the watch glass, and again record any changes. Add drops of Na3PO3 and record any changes, then add FeCl3 and record those changes too. After you are done, dump the contents of the watch glass into the waste beaker, and wash it with tap water and distilled water.
For part B, add distilled water into a test tube and add NaCl. The goal is to saturate the water completely with salt. Shake the tube, and after it is well …show more content…
Create a hot bath with a separate styrofoam cup by adding hot water from the cafeteria. Then, measure CuSO4 and KBR and add them to a beaker, and mix it well, noting the original and changed colors. Then, split the beaker’s contents into three test tubes. Place one tube in the ice bath, one in the hot bath, and leave one at room temperature. Allow the tubes to sit for a while, then compare the tubes and record any differences. If there is enough time, allow the tubes to warm/cool down to room temperature and record any observations. Dispose of the chemicals into the proper …show more content…
CaCO3(s) ⇄ CaO(s) + CO2(g)
Adding CaCO3 to the container will do absolutely nothing to the system, as it is a solid and is not taken into account when calculating the equilibrium constant.
Increasing the pressure by adding argon gas will not affect the system. First of all, argon is an inert gas, which means it will not react with anything involved in this reaction. Since it does not react, it cannot affect the equilibrium constant.
Increasing the pressure by decreasing the volume of the container will change the system by causing more solid CaCO3 to form. In order for the system to counteract the change of pressure, it needs to remove moles of gas from the system, according to PV=nRT. This is achieved by forming more CaCO3, as it can be seen that the reactants side has one mole of substance, while the products side has two.
Removing carbon dioxide from the system will change the system by causing more products to form. The reaction quotient will grow smaller than the equilibrium constant as CO2 is removed, speeding up the reaction creating products. The end result will be a smaller amount of CaCO3, a larger amount of CaO, and an equal amount of
This lab involves three separate experiments. Before you conduct any of them, however, you should put on goggles and aprons, as well as gloves.
For the first part, place the FeCl3 solution into the watch glass, and add a few drops of KSCN. Record any changes you might see. Then, ask Dr. Karraker to add a KSCN crystal to the watch glass, and again record any changes. Add drops of Na3PO3 and record any changes, then add FeCl3 and record those changes too. After you are done, dump the contents of the watch glass into the waste beaker, and wash it with tap water and distilled water.
For part B, add distilled water into a test tube and add NaCl. The goal is to saturate the water completely with salt. Shake the tube, and after it is well …show more content…
Create a hot bath with a separate styrofoam cup by adding hot water from the cafeteria. Then, measure CuSO4 and KBR and add them to a beaker, and mix it well, noting the original and changed colors. Then, split the beaker’s contents into three test tubes. Place one tube in the ice bath, one in the hot bath, and leave one at room temperature. Allow the tubes to sit for a while, then compare the tubes and record any differences. If there is enough time, allow the tubes to warm/cool down to room temperature and record any observations. Dispose of the chemicals into the proper …show more content…
CaCO3(s) ⇄ CaO(s) + CO2(g)
Adding CaCO3 to the container will do absolutely nothing to the system, as it is a solid and is not taken into account when calculating the equilibrium constant.
Increasing the pressure by adding argon gas will not affect the system. First of all, argon is an inert gas, which means it will not react with anything involved in this reaction. Since it does not react, it cannot affect the equilibrium constant.
Increasing the pressure by decreasing the volume of the container will change the system by causing more solid CaCO3 to form. In order for the system to counteract the change of pressure, it needs to remove moles of gas from the system, according to PV=nRT. This is achieved by forming more CaCO3, as it can be seen that the reactants side has one mole of substance, while the products side has two.
Removing carbon dioxide from the system will change the system by causing more products to form. The reaction quotient will grow smaller than the equilibrium constant as CO2 is removed, speeding up the reaction creating products. The end result will be a smaller amount of CaCO3, a larger amount of CaO, and an equal amount of