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(a) Using data in Appendix C, estimate the temperature at which the free-energy change for the transformation from I2(s) to I2(g) is zero.What assumptions must you make in arriving at this estimate?
(b) Use a reference source, such as Web Elements (www.webelements.com), to find the experimental melting and boiling points of I2.
(c) Which of the values in part (b) is closer to the value you obtained in part (a)? Can you explain why this is so?
If the temperature required for this process is 1600°C, what observations would you make considering the fact that the reaction occurs in biological processes
Problem- If I have 300mL of a solution of 25 g/mL. I want to dilute it to a concentration of 5 g/mL. What do I do? Please illustrate work and any conversions to assist me better understand.
Calculate the final temperature of 204 mL of water initially at 35 degrees C upon absorption of 18kJ of heat.
How much heat is required to warm 223 g of ice from -46.3°C to 0.0°C, melt the ice, warm the water from 0.0°C to 100.0°C, boil the water, and heat the steam to 173.0°C?
a water scientist determined the concentrations of calcium and magnesium ions in a sample by titration with 0.06500 m
some ice cubes at 0 degrees c with a total mass of 379g are placed in a microwave oven and subjected to 750. w 750.
An aqueous solution of NaCl has a mole fraction of 0.30. What is the mass of NaCl dissolved in 185.9 mL of solution
Use Lewis structures and bond energies to calculate the enthalpy change of the following reaction: HCN(g) + 2H2(g) => CH3NH2(g) a. 158 kJ b. -158 kJ c. -590 kJ d. 590 kJ e. none of these
What minimum OH- concentration must be attained (for example adding NaOH) to decrease the Mg2+ concentration in a solution of Mg(NO3)2 to less than 1.1e-10 M
What is the pH (to nearest 0.01 pH unit) of a solution prepared by mixing 52.0 mL of 0.125 M HF and 78.0 mL of 0.0465 M NaOH
How many moles of NaF must be added to 100.00mL of 0.15 M HF to prepare a buffer with pH=3.30. Ka(HF)=7.1*10^-4
A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba^2+. When the concentration of F^- exceeds __________ M, BaF2 will precipitate. Neglect volume changes. For BaF2, K sp = 1.7 X 10^-6.
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