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Calculate the Z for the fourth ionization of Ti when it requires 425.6 kJ of energy to ionize 0.185 moles of Ti^3+ to Ti^4+ ( The electron being removed is in the outermost valence orbital of Ti^3+ ground state, therefore n = 3)
Can someone please help me with this problem. I'm not sure what to do with the moles that we are given or if we even need them.
The temperature of the entire system rose from 25.30 °C to 26.59 °C. Calculate the heat of reaction, in kJ, per mole of KOH(aq).
Calculate how many whole drops (.05 mL/drop) of 6 M HCl are required to dissolve this. (I found this to be 11.59 drops
Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb2+ and 0.0050 M Ag+. [Ksp (PbI2) = 1.4 × 10-8; Ksp (AgI) = 8.3 × 10-17] Calculate the Ag+ concentration when PbI2 just begins to precipitate.
Calculate deltaS, deltaStotal, and deltaSsurroundings when the volume of 84.0g of CO initially at 298K and 1.00bar increases by a factor of four in (a) an adiabatic reversible expansion, (b) an expansion againt Pexternal=0, and (c) an isothermal r..
Determine the concentration of the total available acid of the apple juice express your answer in moles/L?
Draw the Lewis Dot Structure for both substances b. Determine the electron pair geometry c. Determine the molecular geometry d. Compare the F - C - F bond angle to the H - S - H bond angle e
The dried precipitate weighs 10.3g. Calculate the amunt of MgCl2 in the original sample (in weight percent).
The concentration of phosphoric acid in Coke is approximately 106.0 mg/mL. Assuming phosphoric acid is the only acid in Coke, calculate the pH of a 355 mL can of Coke.
Circle the form in which a peptide bond is typically found. Describe how the structure of a peptide bond affects protein structure.
What is the equilibrium constant Kc of this reaction? Use an ICE table with numbers.
We performed this lab, but I'm having trouble taking the data collected and calculating the total concentration of both Ca2+ and Mg2+, along with the individual concentration of each.
find the percent composition of a compound that contains 1.94g of C, 0.48-g of H and 2.58-g of S in a 5.00-g S sample of the compound
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