Consider the reaction shown below. If the reaction is placed in a hot water bath, what...
Consider the reaction shown below. If the reaction is placed in a hot water bath, what color would the reaction be at equilibrium? [Cu(H2O)6]2+ + 4 Br1- -> 6 H2O + [CuBr4]1- The reaction is endothermic [CuBr4]1- has a green color [Cu(H2O)6]2+ has a blue color
Homework Answers
It may be the Blue color because the Crystal field stabilization energy is more for the H2O ligand. The formation of Cu with water ligand may be the more.
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Consider the reaction shown below. If the reaction is placed in
a hot water bath, what...
Experience teaches us that most solids are more soluble in warm water than in cold water....
Experience teaches us that most solids are more soluble in warm water than in cold water. Does the solid utility of Mg(OH)_2 fit this pattern? Briefly explain. Cobalt chloride is used in many weather-forecasting devices. Based on your observations in the laboratory, explain how an alcohol solution of CoCl_2 could be used to predict rain. A student is studying the equilibrium described by the net ionic equation shown in Equation 18. [Cu(H_2O)_6]^2+ (aq, blue) + 4 Br^-(aq) CuBr_4^2+(aq, green) +...
EQUL 404: Studying Chemical Equilibris and Applying Le Chateliers Pricipale Using Microscale Lechnique Post-Laboratory Questions (Use...
EQUL 404: Studying Chemical Equilibris and Applying Le Chateliers Pricipale Using Microscale Lechnique Post-Laboratory Questions (Use the spaces provided for the answers and additional paper if necessary.) 1. Experience teaches us that most solids are more soluble in warm water than in cold water. Does the sol ubility of Mg(OH), fit this pattern? Briefly explain (2) The student draws some of the blue solution into the bulb ola Beral pipet. The pipet is placed, bulb down, in a hot-water bath....
Question 8 (1 point) For this reaction, consider the auto-ionization reaction of water (shown below) -...
Question 8 (1 point) For this reaction, consider the auto-ionization reaction of water (shown below) - this reaction is endothermic (AHRXN>0). Based on this information, identify how would the pH of pure H20 change due to a decrease in temperature (T)? H2O(1) + H20(1) OH"(aq) + H30(ag) the pH of pure H20 would not change just by decreasing temperature the pH of pure H20 would increase with a decrease in T the pH of pure H20 would decrease with a...
4. A 200.0mL flask of an unknown gas was placed in a hot water bath. The...
4. A 200.0mL flask of an unknown gas was placed in a hot water bath. The temperature of the bath was found to be 99°C. The pressure of the flask was 733mmHg. The flask with the unknown gas in it had a mass of 126.593g. The same flask weighed 125.623g when it was empty. Determine the mass of the unknown gas in the flask. Determine the Molar Mass of an unknown gas. Assume that the Ideal Gas Law is obeyed...
2. Consider the following equilibrium represent by the reversible equation below: Cu?"(aq) + 4 NH OH(aq)...
2. Consider the following equilibrium represent by the reversible equation below: Cu?"(aq) + 4 NH OH(aq) = [Cu(NH3)4]?" (aq) + 4 H2O(1) Blue Colorless Navy blue Predict the shift (explain why) and indicate the color of the solution when a. Drops of strong acid is added b. H2S gas is bubbled in the solution. Note: H2S reacts with transition metal cations. c. Water is added to the mixture at equilibrium.
one of the test tubes will be put in the cold water bath(ice,on scoop of salt...
one of the test tubes will be put in the cold water bath(ice,on scoop of salt and water in a 250ml beaker)for five minutes.one of the test tubes will be put in a 60 degrees celcius warm water bath for 5 minutes.Put all three test tubes in 125 ml erlenmeyer flasks to stand them up,and compare the colors,below is the equillibrium equation that governs the reaction. Bases on this,determine if the reaction is exothermic or endothermic. [Co(H2O)6]2+ +4HCL------[CoCL4]2- + 6h20
2. Consider the following equilibrium represent by the reversible equation below: Cu2+(aq) + 4 NH4OH(aq) =...
2. Consider the following equilibrium represent by the reversible equation below: Cu2+(aq) + 4 NH4OH(aq) = [Cu(NH3)4]2+(aq) + 4 H2O(1) Blue Colorless Navy blue Predict the shift (explain why) and indicate the color of the solution when a. Drops of strong acid is added b. H2S gas is bubbled in the solution. Note: H2S reacts with transition metal cations. c. Water is added to the mixture at equilibrium.
2. Consider the following equilibrium represent by the reversible equation below: Cu2+(aq) + 4 NH4OH(aq) =...
2. Consider the following equilibrium represent by the reversible equation below: Cu2+(aq) + 4 NH4OH(aq) = [Cu(NH3)4]2+(aq) + 4 H2O(1) Blue Colorless Navy blue Predict the shift (explain why) and indicate the color of the solution when a. Drops of strong acid is added b. H2S gas is bubbled in the solution. Note: H2S reacts with transition metal cations. c. Water is added to the mixture at equilibrium.
Part I Color changes of Methyl Violet. We will study the following reaction: HMV (aq) +...
Part I Color changes of Methyl Violet. We will study the following reaction: HMV (aq) + MV (aq) + H* (aq) yellow greenish-blue violet Step 1. Place about 4 mL of distilled water in a regular test tube. Add two drops of methyl violet indicator. Record the color of the solution. Violet Next, add drop by drop, add 6M HCI. This forces equilibrium to be shifted to the left or right-circle the right answer). Adding HCl changes color from to...
Determine if the system shifted toward reactants or products for each of the changes. Explain how...
Determine if the system shifted toward reactants or products for each of the changes. Explain how each change affected the equilibrium in terms of Le Châtelier’s principle. For the forward reaction, is the system endothermic or exothermic? Fe+3(aq) + SCN–(aq) ⇋ Fe(SCN)+2(aq) a. The addition of KSCN b. The addition of Fe(NO3)3 c. The addition of NaF (s) d. hot water bath e. ice water bath [CoCl4]–2(alcohol) + 6 H2O(ℓ) ⇋ [Co(H2O)6]+2(aq) + 4 Cl–(aq) a. addition of HCl b....
Experience teaches us that most solids are more soluble in warm water than in cold water. Does the solid utility of Mg(OH)_2 fit this pattern? Briefly explain. Cobalt chloride is used in many weather-forecasting devices. Based on your observations in the laboratory, explain how an alcohol solution of CoCl_2 could be used to predict rain. A student is studying the equilibrium described by the net ionic equation shown in Equation 18. [Cu(H_2O)_6]^2+ (aq, blue) + 4 Br^-(aq) CuBr_4^2+(aq, green) +...
EQUL 404: Studying Chemical Equilibris and Applying Le Chateliers Pricipale Using Microscale Lechnique Post-Laboratory Questions (Use the spaces provided for the answers and additional paper if necessary.) 1. Experience teaches us that most solids are more soluble in warm water than in cold water. Does the sol ubility of Mg(OH), fit this pattern? Briefly explain (2) The student draws some of the blue solution into the bulb ola Beral pipet. The pipet is placed, bulb down, in a hot-water bath....
Question 8 (1 point) For this reaction, consider the auto-ionization reaction of water (shown below) - this reaction is endothermic (AHRXN>0). Based on this information, identify how would the pH of pure H20 change due to a decrease in temperature (T)? H2O(1) + H20(1) OH"(aq) + H30(ag) the pH of pure H20 would not change just by decreasing temperature the pH of pure H20 would increase with a decrease in T the pH of pure H20 would decrease with a...
4. A 200.0mL flask of an unknown gas was placed in a hot water bath. The temperature of the bath was found to be 99°C. The pressure of the flask was 733mmHg. The flask with the unknown gas in it had a mass of 126.593g. The same flask weighed 125.623g when it was empty. Determine the mass of the unknown gas in the flask. Determine the Molar Mass of an unknown gas. Assume that the Ideal Gas Law is obeyed...
2. Consider the following equilibrium represent by the reversible equation below: Cu?"(aq) + 4 NH OH(aq) = [Cu(NH3)4]?" (aq) + 4 H2O(1) Blue Colorless Navy blue Predict the shift (explain why) and indicate the color of the solution when a. Drops of strong acid is added b. H2S gas is bubbled in the solution. Note: H2S reacts with transition metal cations. c. Water is added to the mixture at equilibrium.
2. Consider the following equilibrium represent by the reversible equation below: Cu2+(aq) + 4 NH4OH(aq) = [Cu(NH3)4]2+(aq) + 4 H2O(1) Blue Colorless Navy blue Predict the shift (explain why) and indicate the color of the solution when a. Drops of strong acid is added b. H2S gas is bubbled in the solution. Note: H2S reacts with transition metal cations. c. Water is added to the mixture at equilibrium.
2. Consider the following equilibrium represent by the reversible equation below: Cu2+(aq) + 4 NH4OH(aq) = [Cu(NH3)4]2+(aq) + 4 H2O(1) Blue Colorless Navy blue Predict the shift (explain why) and indicate the color of the solution when a. Drops of strong acid is added b. H2S gas is bubbled in the solution. Note: H2S reacts with transition metal cations. c. Water is added to the mixture at equilibrium.
Part I Color changes of Methyl Violet. We will study the following reaction: HMV (aq) + MV (aq) + H* (aq) yellow greenish-blue violet Step 1. Place about 4 mL of distilled water in a regular test tube. Add two drops of methyl violet indicator. Record the color of the solution. Violet Next, add drop by drop, add 6M HCI. This forces equilibrium to be shifted to the left or right-circle the right answer). Adding HCl changes color from to...
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