# cocl2 6h2o + hcl equation

1 Answer. Examples of complete chemical equations to balance: Fe + Cl 2 = FeCl 3; KMnO 4 + HCl = KCl + MnCl 2 + H 2 O + Cl 2; K 4 Fe(CN) 6 + H 2 SO 4 + H 2 O = K 2 SO 4 + FeSO 4 + (NH 4) 2 SO 4 + CO; C 6 H 5 COOH + O 2 = CO 2 + H 2 O Two drops of HCl are added to each well in column 1; four in column 2, six in column 3, eight in column 4, and ten in column 5. Le Chatelier's principle is that when a system is at equilibrium it will shift in order to restore that equilibrium. A decrease in temperature in an endothermic would cause a shift to the left towards the reactants as there is not enough heat to continue the forward reaction. This would lead to a shift to the left. Any color changes are recorded. Five drops of CoCl2 are dropped in each well. it thpresence a lot of alcohol it converts into the blue ion [Co(Cl-)4]-2 One stress taken into account is a change in concentration. The opposite is also true, when there is a decrease in reactants or an increase in products there is a shift left made by the system. 6. 3. b) Water added to this solution would would have no affect on the equilibrium because it is a liquid. The purpose of this lab is to find the effects made by different stresses on a system at equilibrium. Answer Save. Create your own unique website with customizable templates. Relevance. Any color change is recorded. 10. When HCl is added to a pink solution, it turns blue. The addition and removal of heat depends on whether the reaction is endothermic or exothermic. This means that the products are greater than the reactants. 1. A decrease of temperature in an exothermic reaction would result in a shift to the right. The AgNO3 added would react with the Cl- to form AgCl, a solid, and therefore decrease the concentration of Cl-, a reactant, which then shifts the reaction to the left. 8. An increase in temperature, which is released by the reaction as a product, would cause a shift left. Two drops of HCl are added to each well in column 1; four in column 2, six in column 3, eight in column 4, and ten in column 5. 2. e) A decrease in temperature would shift it left. This would result in slightly skewed color change interpretations as their concentrations would not be what it is labeled as. The color change is recorded. This reaction takes place at a temperature of 160-170°C in a flow dry HCl. Any solid or liquid added or taken away will not affect equilibrium or cause a shift. AgNO3 added resulted in a precipitate and a very light pink color for every well showing a shift left as well. These well are the mixed with a clean toothpick. In an exothermic reaction the opposite is true. This increase of Cl- ions would be an increase in the concentration of the reactants and then shift the reaction more forward to reestablish equilibrium. Limiting reagent can be computed for a balanced equation by entering the number of moles or weight for all reagents. Five drops of CoCl2 are dropped in each well. The color change is recorded. b) The addition of water would increase the concentration of water, which is a product. 1. A source of error may have come from the use of tap water instead of distilled water. Freezing Point Depression with Antifreeze. 4. Temperature is the only thing that causes a change in Kc or Kp value, for concentration and pressure respectively. These well are the mixed with a clean toothpick. CoCl 2 •6H 2 O CoCl 2 + 6H 2 O. 3. These well are the mixed with a clean toothpick. Info: CoCl2*6H2O(heat) might be an improperly capitalized: COCl2*6H2O(HeAt), CoCl2*6H2O(HeAt) Instructions and examples below may help to solve this problem You can always ask for help in the forum Instructions on balancing chemical equations: Enter an equation of a chemical reaction and click 'Balance'. c) The addition of AgNO3 would shift it left. If Concentrated Hydrochloric Acid Is Added To Thissolution, The Following Equilibrium Is Established: [CoCl (H2O)5]+ +Cl- [CoCl2 (H2O)2 ]+3H2O ΔH0 Where [CoCl2 (H2O)2 ] Is Alsosoluble In Water. Explanations (including important chemical equation): The following equilibrium is observed: Co(H 2 O) 6 2+ (aq) + 4 Cl-(aq) <=> CoCl 4 2-(aq) + 6 H 2 O(g) The Co(H 2 O) 6 2+ complex is pink, and the CoCl 4 2- complex is blue. 1 decade ago. a) The addition of HCl would shift it right, b) The addition of water would shift it left. The color change is recorded. This increase in Cl- concentration, a reactant, would cause the forward reaction rate of the system to increase in order to reach equilibrium. Steve O. Lv 7. Temperature is another stress which a system will shift in order to accommodate. K values are calculated by placing products raised to their coefficients in a reaction over the reactants raised to their coefficients. There may also have been human error in placing the correct number of drops of each compound in the wells. NaCl separates into ions, so with its addition there would be an increase in Cl- ions. when CoCl2*6 H2O dissoves in water it makes the pink ion [Co(H2O)6]+2.