The deep blue compound Cu(NH3)4SO4 is made by the reaction of copper(II) sulfate and ammonia. CuSO4(aq) + 4NH3(aq) → Cu(NH3)4SO4(aq) If you use 47.0 g of CuSO4 and excess NH3, what is the theoretical yield of Cu(NH3)4SO4? If you isolate 38.2 g of Cu(NH3)4SO4, what is the percent yield of Cu(NH3)4SO4? ______ g Cu(NH3)4SO4 _______ %
moles CuSO4= 47g/159.6096g/mol= 0.294mol
1 mol of CuSO4 produces 1 mol of Cu(NH3)4SO4, so, 0.294 mol of CuSO4 will produce 0.294 mol of Cu(NH3)4SO4.
mass Cu(NH3)4SO4= 0.294 mol x 227.612g/mol= 66.92g (this is the theoretical yield).
%yield= mass obtained/theoretical yield x100 = 38.2g/66.92g x 100 = 57%
The deep blue compound Cu(NH3)4SO4 is made by the reaction of copper(II) sulfate and ammonia. CuSO4(aq)...
The deep blue compound Cu(NH)4SO4 is made by the reaction of copper(ll) sulfate and ammonia Cu(NHs)4SO4 (aq) CuSO4(aq) 4 NHs (aq) > If you use 18.0 g of CuSO4 and excess NH3. what is the theoretical yield of Cu(NHs)4SO4? g Cu(NHs)4SO4 If you isolate 15.3 g of Cu(NH3)4SO4, what is the percent yield of Cu(NH3)4S04?
4 A common method for analyzing for the nickel content of a sample is to use a precipitation reaction. Adding the organic compound dimethylglyoscime to a solution con- taining Nions precipitates a red solid Wwe care Derive the empirical formula for the red solid based on the following composition: Ni, 20.315%; C, 33.258%; H, 4.884%; 0,22.151%, and N, 19.392%. (95) . The reaction of methane and water is one way to y prepare hydrogen for use as a fuel CH...
Choose the equation that correctly represents the reaction between copper(II) sulfate and sodium hydroxide. CuSO4(aq) + 2 NaOH(aq) --> Cu(OH)2(s) + Na2SO4(aq) CuSO4(aq) + 2 NaOH(aq) --> Cu(OH)2(aq) + Na2SO4(s) CuSO3(aq) + 2 NaOH(aq) --> Cu(OH)2(s) + Na2SO3(aq) CuSO4(aq) + NaOH(aq) --> CuOH(s) + NaSO4(aq)
1.25 g of CuSO4.5 H2O is treated with excess ammonia, when a deep blue solution is obtained. To this solution 5 mis of ethanol is added and the solid copper sulfate tetramine sulfate is obtained on filtration using a Buchner filter. On drying, the mass of the filter paper (085g) and compound is found to be 1.12 grams Calculate the percent yield? [6]
2. Consider the following equilibrium: Cu2+(aq) pale blue + 4NH3(aq) +[Cu(NH3)4]2+ (aq) colorless deep purple Would you expect to see an increase, no change, or a decrease in the purple color when: (a) the temperature of the system is increased (the reaction is endothermic). (b) a catalyst is added. (c) more aqueous NH3 is added to the equilibrium. (d) the pressure is increased. NaOH(aq) is added to the system, resulting in the precipitation of Cu(OH)2(s). _(1) (f) the volume of...
40. Concentrated aqueous ammonia is added to a solution of copper(II) sulfate. A white precipitate forms. The precipitate dissolves as more ammonia is added, generating an intensely blue solution. Which combination of net ionic equations, in the appropriate order, describes this chemistry?! I Cu?* (aq) + 2OH(aq) Cu(OH)2 (19) II Cu?" (aq) + 2OH(aq) = Cu(OH)2 (8) III Cu(OH)(aq) + 4 NH, (aq) Cu(NH3),?* () + 2OH(aq) IV Cu(OH)2 (8) + 4NH, (aq) Cu(NH3)*(14) + 2OH(aq) V NH3(aq) + H20...
Consider the insoluble compound copper(II) hydroxide , Cu(OH)2 . The copper(II) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of Cu(OH)2 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Cu(NH3)42+ , Kf = 6.8×1012 . Use the pull-down boxes to specify states such as (aq) or (s). + + K = Submit Answer Voit needed for this question. Consider the insoluble...
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The salt copper(II) sulfate dissolves in water according to the reaction: CuSO4(s) ----->Cu2+(aq) + SO42-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the following data: CuSO4(s) = -771.4 kJ mol-1 Cu2+(aq) = 64.8 kJ mol-1 SO42-(aq) = -909.3 kJ mol-1 ______kJ (b) Calculate the temperature reached by the solution formed when 18.3 g of CuSO4 is dissolved in 0.195 L of water at 24.2 °C. Approximate the heat capacity of the solution by the heat capacity...