A student conducts an experiment boiling water in a 3.96L pot. The Diameter of the base of the pot is 7-3/4” and the height is 5-1/8”.

2 Liters of water @ 23°C takes 11 minutes to boil. 500mL of water at 23°C are added to the boiling water. Producing 3-1/4” height of water and 88°C mixture temperature. It then takes till 11:29 for the water mixture to resume boiling. The whole operation takes 1 hour and 26 minutes from start to the pot boiled dry. How much energy was required for this process?

8. An experiment is conducted to compare the effects of weathering on paint of three different types. To do so, identical surfaces are coated with some paint of each type that has been exposed to four different environments. Measurements of the degree of deterioration we made for each surface. The data set is uploaded to Moodle. What can you say about the different paint types and different environments and their effects on the paint degradation?

   Deterioration	Paint Type	Environment
   9.42	A	1
   9.14	A	1
   10.82	A	2
   11.82	A	2
   8.51	A	3
   7.4	A	3
   10.08	A	4
   10.11	A	4
   11.37	B	1
   12.43	B	1
   13.56	B	2
   11.31	B	2
   11.14	B	3
   10.55	B	3
   14.7	B	4
   14.35	B	4
   9.85	C	1
   11.84	C	1
   12.13	C	2
   11.34	C	2
   10.09	C	3
   9.03	C	3
   10.87	C	4
   12.7	C	4

   I am trying to do this in Excel but the "Anova: two-factor with replication" test won't work and I can't figure out what I'm doing wrong. I keep getting an error that says "Anova: Two-Factor With Replication - Each sample must contain the same number of rows." Some explanation and help would be greatly appreciated. Thanks.

In a double-slit experiment, if the slit separation is increased by a factor of two, what happens to the interference pattern shown on the screen? What happens if the wavelength is halved? What happens if the distance to the screen is double?

Two small forward-facing speakers are 2.50 m apart. They are both emitting, in phase with each other, a sound of frequency 1100 Hz in a room where the speed of sound is 344 m/s. A woman is standing opposite the midpoint between the speakers and is initially 35.0 m from the midpoint. As she slowly walks parallel to the line connecting the speakers, at what angle ? (relative to the centerline coming outward from the midpoint between the speakers) will she first hear no sound?

A factorial experiment was designed to test for any significant differences in the time needed to perform English to foreign language translations with two computerized language translators. Because the type of language translated was also considered a significant factor, translations were made with both systems for three different languages: Spanish, French, and German. Use the following data for translation time in hours.

Test for any significant differences due to language translator system (Factor A), type of language (Factor B), and interaction. Use a=.05

Complete the following ANOVA table (to 2 decimals, if necessary). Round your p-value to 4 decimal places.

During the experiment of shell and tube heat exchanger by using this equipment the Source of the water was from the water tap that is mean it is open feed water

To explain more:    the lab engineer used a drink water that supply it from the water tap directly to the heat exchanger equipment

And then he discharge the water to the sink that is not correct way ? I do not have a scientific answer in this but what i think the water from tap is not laminer and the temperature

is not fixed . so I need a real explanation in mechanical and chemical engineering about this

CAN you explain why the way of supplying water like this to the equipment is not good ?

and what the engineer used ?

which type of liquid shall he used ? And why and how it will improve

think about salt in the normal water as well as the bacteria, Think about fouling factor , cleaning heat exchanger regularly,

Determine the indicated probability for a binomial experiment with the given number of trials n and the given success probability p. Then find the mean, variance, and standard deviation.

A student performed an experiment similar to the one that you will perform, but using different solutions from the ones that you will use. The student's data are presented in Table 4 below.

1.) Is a 0.1 M solution of NaNO2 acidic or basic?

2.) What experimental evidence supports your answer?

3.) List the solutions studied by the student that are basic.

4.) What experimental evidence supports your answer?

Table 4 Student data for estimating the PH of solutins

   indicator color

5.) Using these data, compare the relative basicity of the Ca(OH)2 and C2H5NH2 solutions. Briefly explain on what basis you can or cannot make this comparison.

6.) List the basic solutions in order of increasing basicity.

7.) What experimental evidence supports your answer?

In a similar experiment to the one you have performed a student is measuring the equilibrium for an organic acid that is soluble in water and in cyclohexane, a nonpolar organic solvent. When shaken with the solution of water and cyclohexane, it distributes between the organic and aqueous phase. The two phases are separated and titrated with 0.12 M NaOH. Calculate the equilibrium constant for an acid where the titration of the aqueous phase requires 9.9 mL of the base and the organic phase requires 4.76 mL of the base.

I can't figure out how to solve this problem. We did something similar in my lab but i can't remember. Show all work please.

Experiment 2: Using the Secondary Standard to Determine the Concentration of an Acid

1. In an Erlenmeyer flask, add 25 mL of Unknown #1 concentration of acetic acid (CH₃COOH) and 2 drops of phenolphthalein indicator.

2. Coarse Titration:

(a) Take a burette from the Containers shelf and place it on the workbench. Fill the burette with 50 mL of the standardized sodium hydroxide solution. Record the initial burette reading. Place the Erlenmeyer flask on the lower half of the burette.

(b) Perform a coarse titration, adding large increments of the sodium hydroxide solution from the burette by pressing and holding the black knob at the bottom of the burette. Each time you add the sodium hydroxide solution, check the volume remaining in the burette. As the sodium hydroxide is added to the acetic acid solution the pH increases. Watch for a change of the phenolphthalein color in the Erlenmeyer flask. The pink color will appear in Erlenmeyer flask when the endpoint is either reached or crossed. Record the burette volume at which this occurs.

(c) Place the Erlenmeyer flask and the burette in the recycling bin.

3. Fine Titration:

(a) Set up the tiration as before: (i) An Erlenmeyer flask filled with 25 mL of unknown #1 concentration of acetic acid and 2 drops of phenolphthalein indicator. (ii) A burette filled with 50 mL of the standardized sodium hydroxide solution. Record the initial burette reading. (iii) Place the Erlenmeyer flask on the lower half of the burette.

(b) Click and hold the black knob of the burette to quickly add enough standard sodium hydroxide solution to just get into the range of the coarse titration: 1 mL BEFORE the pink endpoint. This is near, but not yet at, the titration's endpoint.

(c) Add sodium hydroxide solution in small increments, down to one drop at a time, record the volume of the pink endpoint.

(d) Place the Erlenmeyer flask and the burette in the recycling bin.

4. Repeat the titration two more times for a total of three trials. Use 30mL of acetic acid for trial 2 and 35mL for trial 3. Calculate the acid concentration of each trial.
[If you run out of NaOH, simply prepare a second solution as described in step 2 of Exp. 1. You don’t need to standardize it a second time. Assume the standardized concentration is the same as before.]

Need help with the following!

Trial 1              Trial 2              Trial 3

a) Volume of acid (mL)                                     25.1mL             30.1mL            35.1mL

b) Volume of NaOH titrated (mL)                     _____              _____              _____

c) Moles of NaOH titrated                                 _____              _____              _____

d) Moles of acid                                               _____              _____              _____

e) Concentration of acid (M)                             _____              _____              _____

f) Average acid concentration (M)                                             _____

Using your Trial 1 data, show you work for calculating each of the following:

Moles of NaOH titrated

Moles of acid

Concentration of acid

Questions

1. Similar to other acids you've encountered in this class (HCl, HNO₃, etc.), benzoic acid is monoprotic (HA), meaning that only one of its hydrogens dissociates in water. With this in mind, write the net ionic equation for the reaction performed during this titration (as discussed in lecture).  

2. After dissolving the acid with water, a student noticed some undissolved solid, but continued with the titration as instructed by the procedure. He titrated until the pink color persisted for 30 seconds and recorded the volume of titrant required. Preparing for the second determination, he set the reaction solution aside and added some more NaOH to the buret. He was about to pour the reaction solution down the drain, so he could rinse and reuse the flask, when he saw that the pink color had disappeared!

a) What happened?

b) What can the student do to correct this error and salvage this trial, so he doesn't have to redo it? What corrections or modifications will have to be made to his recorded data?

3. Another student began adding titrant to the acid solution, but stopped when she suddenly realized that she forgot to add the 3 drops of phenolphthalein. When she did, the solution immediately turned dark red!

a) What happened?

b) What can the student do to correct this error and salvage this trial, so she doesn't have to redo it? What corrections or modifications will have to be made to her recorded data?