Material Engineering
Suppose 1 g of copper as Cu2+ is dissolved in 1000 g of water to produce an electrolyte. Calculate the electrode potential of the copper half-cell in this electrolyte. Assume T = 25oC. Express your answer in volts and to three significant figures. Tolerance ±0.2.
For getting one moles of Cu in 1000ml water gives rise to 1M of solution
Atomic mass of Cu= 63.54 gm
Concentration of 1 g= 1/63.54 M= 0.015738
From Nerst Equation
E= Eo-0.0592/n log (Cu+2]
Where n= number of electrons=2
E= 0.34-0.0592/2ln (1/0.0157)=0.34+ 0.0592/2 log(0.0157) =0.34-0.053=0.287V
Material Engineering Suppose 1 g of copper as Cu2+ is dissolved in 1000 g of water...
*A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II), [Cu(NH3)4]2+. If a standard hydrogen electrode is used as the cathode, the cell potential, Ecell, is found to be 0.070 V at 298 K. A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II), [NH. If a standard hydrogen electrode is used as the cathode, the cell potential,...
A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(I), [Cu(NH). If a standard hydrogen electrode is used as the cathode, the cell potential, Ecell, is found to be 0.074 V at 298 K Constants Periodic Table Use the standard reduction potentials shown here to answer the questions Reduction half-reaction E (V) Cu2+ (aq) 2e Cu(s) 0.337 2H + (aq) + 2e →H, (g) | 0.000 ▼ Part A...
Suppose 27.0 g of ice at -10.0 C is placed into 300.0 g of water in a 200.0-g copper calorimeter. The final temperature of the water and copper calorimeter is 18.0° C 1) What was the initial common temperature of the water and copper? (Express your answer to three significant figures.)
And a copper electrode with 0.500 M Cu?' as the second half cell Cu2+ (aq) + 2 e Cu(s) Eºred= 0.337 V The measured cell potential when the water sample was placed into the silver side of the cell was 0.0905 V. Write the balanced equation for the overall reaction in acidic solution. AgCl(s) + Cu2+ (aq) + 3 e → Ag(s) + Cu(s) + CI+ (aq) 04- 03. 02. + 2 O 4+ 1 2 3 4 5 6...
O SOO mol Al is dissolved in 1000 g of pure water at 25. The density of the solutions 105 ml Determine the eve of the solution. (Write down your final answer with the correct significant figures) В
3a. Calculate the molar mass (in g/mol) of an unknown 1:1 electrolyte if 0.482 g dissolved in 223.1 mL of water at 74.75 °C has an osmotic pressure of 54.4 mmHg. R = 0.082058 L⋅atm⋅mol−1⋅K−1. 1.00 atm = 760 mmHg. Report your answer to THREE significant figures. 3b. Calculate the required mass of an unknown nonelectrolyte (ℳ = 131.5599 g/mol) dissolved in 140.1 g of solvent that gives a solution that boils at 36.04 °C. The boiling point of the...
Suppose 3.03 g of copper(II) nitrate is dissolved in 200. mL of a 72.0 m M aqueous solution of sodium chromate. Calculate the final molarity of copper(II) cation in the solution. You can assume the volume of the solution doesn't change when the copper(II) nitrate is dissolved in it. Round your answer to 2 significant digits. Пм x 6 ?
please help! Suppose 7.65 g of copper(II) acetate is dissolved in 350 ml of a 71.0 m M aqueous solution of sodium chromate. Calculate the final molarity of copper(II) cation in the solution. You can assume the volume of the solution doesn't change when the copper(II) acetate is dissolved in it. Be sure your answer has the correct number of significant digits. M
Calculate the molar mass (in g/mol) of an unknown 1:1 electrolyte if 0.45 g dissolved in 199.2 mL of water at 49.72 °C has an osmotic pressure of 34.4 mmHg. R = 0.082058 L⋅atm⋅mol−1⋅K−1. 1.00 atm = 760 mmHg. Report your answer to THREE significant figures.
plz answer and show work Suppose 0.193 g of copper(II) nitrate is dissolved in 350. mL of a 17.0 m M aqueous solution of sodium chromate. Calculate the final molarity of copper(II) cation in the solution. You can assume the volume of the solution doesn't change when the copper(II) nitrate is dissolved in it. Be sure your answer has the correct number of significant digits. Ом 01