Using the Cu-Ni phase diagram (Callister, Chap.9, pp. 288) estimate the following quantities for a nominal    composition of 55%Ni – 45% Cu:

a) Liquidus Temperature,

b) Solidus Temperature,

c) The composition of the liqiud and solid phases present in alloy at 1300°C,

d) Using the inverse lever rule, find the amount (by weight) of liquid and

solid phases present in alloy.

1. If you can read at an average rate of 5.15 words per second, how long will it take you to read a 505 page book that has an average of 995 words per page?

2. Let’s say you need to make 12.0 dozen cookies. You decide to make these cookies in batches of 24.0 cookies each. Each batch of cookies requires 27.0 mL of vanilla extract. Each bottle of vanilla extract contains 150. mL of liquid. How many bottles of vanilla extract will you need to make all of your cookies?

3. The label on a bottle of orange juice says that each serving of juice provides you with 480. mg of potassium. The label also says that a serving size is 8.00 fluid ounces and that there are two servings per container. In addition, the label says that 480. mg of potassium is 14.0% of the recommended daily amount of potassium that you ingest in a 2000. calorie diet. How many servings of orange juice do you need to ingest to get 100.% of the recommended daily amount of potassium?

4. My car burns oil at a rate of 1.00 quart every 895 miles. If I travel an average of 83,454 km per year, how many liters of oil do I burn in 11.0 years?

5. If my back yard has an area of 75.5 square zzbts, what is the area in square oobts?

1.00 oobt = 3.43 qvsts

1.00 qvst = 15.4 zzbts

Calculate the thermodynamic favorability of aerobic Mn(II) oxidation and aerobic Fe(II) oxidation at pH 2 and 7. Is it likely that an organism could get “enough” energy to grow from each of these four processes? ​

Consider the titration of 42.8 mLmL of 0.265 MM HFHF with 0.185 MM NaOHNaOH. Calculate the pHpH at each of the following points.

Part A

How many milliliters of base are required to reach the equivalence point?

Express your answer using three significant figures.

Part B

Calculate the pHpH after the addition of 10.7 mLmL of base

Express your answer using two decimal places.

Part C

Calculate the pHpH at halfway to the equivalence point.

Express your answer using two decimal places.

Part D

Calculate the pHpH at the equivalence point.

Express your answer using two decimal places.

Part E

Calculate the pHpH after the addition of 85.6 mLmL of base.

Express your answer using two decimal places.

I would really appreciate it if you could explain this problem step by step, in as much detail as possible, as I am having a difficult time trying to understand it. Thank you :)

How many liters of CO2 can be produced by combustion of 5.80 g butane with 15.0 liters of oxygen . All gases measured at STP.

I appreciate your help!

1. Distinguish between reverse phase and normal phase separations. 2. What is the dynamic range for absorbance spectroscopy? What is the dynamic range for fluorescence spectroscopy? Which has the lowest LOD and why? 3. What types of molecules fluoresce? What is quenching and what makes a good quencher? 4. What is the underlying equation for all partition chromatography methods? Why?

Arrange the 0.15 M solutions of the following compounds in order of increasing acidity (least acidic first).

NH₄I                B. CH₃COONH₄          C. CH₃COOK           D. KCl                 E. CH₃COOH          

         F. KF                   G. HBr                          H. CHCl₂COOH        I. NH₃                  J. CF₃COOH

      ammonia,    K_b = 1.80

What is the key difference in the biosynthesis of purine ribonucleotides vs. the biosynthesis of pyrimidine ribonucleotides?

At a certain temperature, 0.4011 mol of N2 and 1.581 mol of H2 are placed in a 1.50L container. N2(g) + 3H2(g) −⇀↽− 2NH3(g) At equilibrium, 0.1401 mol of N2 is present. Calculate the equilibrium constant, Kc.

Calculate the molar solubility of magnesium fluoride in each of the following solutions:
a) pure water
b) 0.010 M potassium fluoride solution
c) 0.050 M solution of magnesium nitrate
d) Why are the results of parts (a) thru (c) different?

A). A mixture of methane and argon gases is maintained in a 8.34 L flask at a pressure of 2.24 atm and a temperature of 66 °C. If the gas mixture contains 3.59 grams of methane, the number of grams of argon in the mixture is............ g

. B). A mixture of xenon and hydrogen gases, in a 5.89 L flask at 13 °C, contains 12.5 grams of xenon and 0.288 grams of hydrogen. The partial pressure of hydrogen in the flask is.............. atm and the total pressure in the flask is............. atm.

what intermolecular forces are present in each of the substances?

EXAMPLES OF THERMODYNAMIC STATE FUNCTION WITH DEFINITION

A 1.000-L vessel contains a mixture of hydrogen, carbon monoxide and methane gases in unknown proportions at 23.3-bar and 25 °C. The gaseous mixture is found to have a mass of 13.70-g and a higher heating value of 494.90 kJ/mol. What is the composition of the gas?