What is the % of Cu (MM = 63.55 g/mol) in Cu(CH3COO)2.H2O (MM = 199.65 g/mol)
% of an element in the compound = [mass of that element in the compoundx100 ]/ molar mass
So
% of Cu in given Cu(CH3COO)2.H2O = mass due to Cu x100/its molar mass
= 63.55g x100 /199.65 g
= 31.83%
What is the % of Cu (MM = 63.55 g/mol) in Cu(CH3COO)2.H2O (MM = 199.65 g/mol)
10 g of glucose (mm=180.2g/mol) is dissolved in 70 mL of H2O at 25 degrees. 1. What is the Vapor pressure of H2O?
Please Help: Calculate the formation constant for the formation of [Cu(en)(H2O)4]2+ from [Cu(H2O)6]2+, given that ΔG∘ is −60.1kJ⋅mol−1 at 298 K. Express your answer numerically to three significant figures.
Part B: Calculate the formation constant for the formation of [Cu(NH3)4(H2O)2]2+ from [Cu(H2O)6]2+, given that ΔG∘ is −74.2kJ⋅mol−1 at 298 K. Express your answer numerically to three significant figures. Part C: Consider the formation of [Ni(en)3]2+ from [Ni(H2O)6]2+. The stepwise ΔG∘ values at 298 Kare ΔG∘1 for first step=−42.9 kJ⋅mol−1 ΔG∘2 for second step=−35.8 kJ⋅mol−1 ΔG∘3 for third step=−24.3 kJ⋅mol−1Calculate the overall formation constant (Kf) for the complex [Ni(en)3]2+. Express your answer numerically to three significant figures.
If 320.18 g of Cu at 155.19 degrees C is added to 500 g of H2O at 25 oC, what is the final temperature of the copper and water? (Sp. H of Cu = 0.382 J/g oC)
NH3(g) and CuO(s) react to form Cu(s), H2O(l) and N2(g). What is the theoretical yield of Cu(s) in moles if the percent yield of Cu(s) is 86.0% and 7.00 grams of Cu(s) forms?
What is the pH of a solution containing 0.342 mol L-1 CH3COOH and 0.428 CH3COO- mol L-1 ? Round your answer to 2 decimal places.
Determine the order of the 3 ligands; [Cu(en)2(H2O)2]2+, [Cu(H2O)6]2+, Cu(EDTA)2- in the electrochemical species.
A solution is made using 80.1 g of toluene (MM = 92.13 g/mol) and 80.0 g of benzene (MM = 78.11 g/mol). What is the molality of the toluene in the solution?
For the following process: H2O(g) + Cl2O(g) à 2HOCl(g) Ho(H2O(g))= 242KJ/mol Ho(Cl2O(g))=80KJ/mol Ho(HOCl(g))= -80KJ/mol So(H2O(g))= 0.189 KJ/K So(Cl2O(g))=0.266 KJ/K So(HOCl(g))= 0.237 KJ/K A) Calculate ΔHo, ΔSo and ΔGo B)Calculate ΔG at 100K and P(H2O)=P(Cl2O)= P(HOCL)=10atm
At 1000 °C, for the reaction: 2 H2O(g) ↔ 2 H2(g) + O2(g) Kc = 7.32 x 10-18, what will be the [H2(g)] at equilibrium if 1.00 mol of H2O(g) are placed in a 10.0 L vessel?