REDOX REACTION:
C6H12O6 + 6O2 ---> 6CO2 + 6H2O + Energy
-Could you tell me which compound is oxidized and which compound is reduced and why? I would really appreciate if you drew it out step-by-step and showed the calculations for each oxidation number.
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1. For each of the following circumstances, indicate wheter the calculated molarity of NaoH would be lower, higher, or unaffected. Explain your answer in each case.
a. The inside of the pipet used to transfer the standard HCl
solution was wet with water.
b. You added 40 mL of water to the titration flask rather than 25
mL.
c. The buret, wet with water, was not rinsed with NaOH solution
before filling the buret with NaOH with solution.
d. Five (5) drops of phenolphthalein were added to the solution to
be titrated rather than three (3) drops.
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In our chem lab, we were testing for an unknown equilibrium "k" value using the absorbency rates of various concentrations, how am i supposed to find the k value if none of our samples ever reached equilibrium. Our prof said to calculate the absorbency of each sample, but all the values are obviously different.
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If anyone can show me how these are solved I would appreciate it, answers included though please.
16.) Which of the follow conatin the GREATEST number of MOLES of OXYGEN. Show your work.
0.50 mol P4010, 1.5mol P2O5, 2.5mol CO2, 2.0mol N2O4
20.) Ibuprofen has a chemical formula C13H1802.
When the equation is properly balanced what is a correct mole ratio
of CO2 to H2O in the reaction?
21.) 4Al(s) + 3O2(g) ---> 2 Al2O3 (s) If 10.0
mol of aluminum is converted to Al oxide, how many moles of Al2O3
are produced?
23.) What MASS of NaOH is need to make 450mL of a 2.0 M solution. SHOW your work.
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Explain how a molecule can have polar bonds but have no molecular polarity. Name the compounds that have bond polarity but no molecular polarity ( out of CH4, CF4, NH3, NF3, H2O, OF2, CO2, CH2F2).
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Determine the pH of (a) 0.20 M sulfuric acid (b) 0.20 M hydrochloric acid, (c) 0.20 M sodium hydroxide, (d) 0.20 M acetic acid, and (e) 0.20 M solution of NH3 at 25 oC.
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Q#1. Draw a simple schematic of the electron energy levels
for:
a) an atom of H and a dimer (2 atoms) of H
b) an atom of Li, a dimer of Li, and a solid of Li. To what
extent
the valence band is filled in solid Li?
Label each energy level/band (ie, 1s, 2s, etc.)
Reading:Materials Science and Engineering,An Introduction by William D.Callisler Ch. 18
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a 2.00 l container holds 4.00 moles of o2 and 2.70 moles of he at 293 k. What is the partial pressure of o2? He? what is the total pressure?
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“When a strong base is gradually added dropwise to a weak acid, the pH changes at each addition. When the appropriate quantity of base has been added to react with all of the acid, the pH changes sharply, indicating the endpoint of the titration. A plot of pH versus volume of base added gives what is known as a titration curve”.
Consider the titration of 25.00 mL of 0.1000 M benzoic acid with 0.1000 M NaOH,.
Write a balanced chemical equation for the titration reaction using C6H5COOH for benzoic acid’s formula.
Determine the volume of NaOH solution required to reach the endpoint.
The chart on the next page has entries for several steps along the titration curve. To calculate the pH at each step, you first must understand the chemistry at that step, and then you can decide the appropriate method to calculate the pH. For each volume listed, (i) list the major species in solution, (ii) determine whether the Ka equation, Kb equation, buffer equation, or solution equilibrium equation is appropriate for the calculation of the solution [H3O+] and pH, and (iii) complete the calculations.
|
Volume NaOH Added (mL) |
Major Species |
Appropriate Equation |
[H3O+] |
pH |
|
0.00 |
||||
|
5.00 |
||||
|
12.50 |
||||
|
20.00 |
||||
|
25.00 |
||||
|
30.00 |
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- 25.0-L tank contains 295 g N2, 135 g O2, and 24.0 He gases. Calculate the partial pressure of each gas and the total gas pressure at 20.0oC.
(Answer: PN2 = 10.1 atm; PO2 = 4.06 atm; PHe = 5.77 atm; Ptotal = 19.9 atm)
- A 5.0-gallon gas tank contains N2 and H2 gas, such that the partial pressure of H2 is three times that of N2 gas. If the total gas pressure is 2.4 atm at 25oC, how many grams of N2 and H2, respectively, are present? (Answer: 13 g of N2 and 2.8 g of H2)
Thank you for your your help, if you can help me showing me the process to learn about it at least of one I will appreciate
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1. Calculate the moles of product produced in the ractions, if 4.00g of the hydrate was used in the reaction
FeCl2 * 4H2O(aq) + H2C2O4(aq) -> FeC2O4 * 2H2O(s) +2H2O(I) + 2HCl(aq)
Ni(NO2)2 * 6H2O(aq) +H2C2O4(aq) -> NiC2O4 * 2H2O(s) + 4H2O(I) + 2HNO3(aq)
MnSO4 * H2O(aq) + H2C2O4(aq) + 2H2O(I) -> MnC2O4 * 3H2O(s) + 3H2O(I) + H2SO4(aq)
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a statement of the first law of thermodynamics is that a. in a spontaneous process, the entropy of the universe increases b. there is no disorder in a perfect crystal at 0 k. c. the total energy of the universe is constant. d. the totla energy of the universe is constant. e. mass and energy are conserved in all chemical reactions
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A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C under each of the following conditions.
Part A standard conditions
Part B [Fe3+]=1.9×10−3 M ; [Mg2+]=1.80 M
Part C [Fe3+]=1.80 M ; [Mg2+]=1.9×10−3 M
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1. How many grams of helium must be released to reduce the pressure to 69 atm assuming ideal gas behavior?
2. If the pressure exerted by ozone, O3, in the stratosphere is 3.0×10−3atm and the temperature is 251 K , how many ozone molecules are in a liter?
3. Carbon dioxide makes up approximately 0.04% of Earth's atmosphere. If you collect a 3.0 L sample from the atmosphere at sea level (1.00 atm) on a warm day (29 ∘C), how many CO2 molecules are in your sample?
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