1) Calculate scattering particles off of a single crystal of nickel. The Ni lattice spacing is 2.15 x 10-10 m. Compute the angle for the first order diffraction feature assuming you bombard the system with:
a. X-ray photons of energy 18.0 keV.
b. Electrons with kinetic energy 18.0 keV.
c. Neutrons with kinetic energy 18.0 keV.
d. What do you conclude from your results above?
In: Chemistry
calculate pH from 75 ml of 0.1M CH3COOH and 25 ml of 0.1 M Ca(OH)2
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Consider the following reaction:
2NO(g)+O2(g)→2NO2(g)
Estimate ΔG∘ for this reaction at each of the following
temperatures and predict whether or not the reaction will be
spontaneous. (Assume that ΔH∘ and ΔS∘ do not
change too much within the give temperature range.)
A)298 K
B)735 K
C)855 K
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50 mL of 0.060 M K2CrO4 is mixed with 50 mL of 0.080 M AgNO3. Calculate the following:
a. The solubility of Ag2CrO4 (Ksp = 1.9 X 10-12) in the solution in moles per liter.
b. The concentrations of the following ions Ag+, CrO4-2, K+, and NO3-.
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A little stuck, could you please show working out?
Which of the following processes represents an oxidation reaction?
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1. ?Mg(s) -> Mg2+(aq) |
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2. ?2H+(aq) -> H2(g) |
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3. ?Cu2+(aq) -> Cu(s) |
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4. ?I2(s) -> 2I-(aq) |
Which one of the following processes represents a reduction reaction?
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1. ?Zn(s) -> Zn2+(aq) |
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2. ? ?2Cl-(aq) -> Cl2(g) |
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3. ? ?H2(g) -> 2H+(aq) |
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4. Cu2+(aq) -> Cu(s) |
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50lbs of gas with the specific gavity of .88(treat as real gas) is in a tank at p=1384 psig and at T=320F what is volume of the tank in ft^3 This question is in oilfield units
In: Chemistry
In: Chemistry
Using a table of standard electrode potentials, decide which of the following statements is completely true.
A. Cu2+ can oxidize H2, and Fe can reduce Mn2+ .
B. Ni2+ can oxidize Cu2+, and Fe2+ can reduce H+ .
C. Fe2+ can oxidize H2, and Fe2+ can reduce Au3+ .
D. Br2 can oxidize Ni, and H2 can reduce Mn2+ .
E. H + can oxidize Fe, and Ni can reduce Br2.
Answer: E.. but why? can you explain why A-D are incorrect and why E is right. I know it has something to do with how they are positioned on the standard reduction potential list, but I dont understand the concept, which I will need to know for my exam. thank you!
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Under the topic of aqueous chemical equilibria, outline the quantitative treatment of a single acid in solution. Indicate in your answer, where a mass balance expression is utilised.
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Please write (For each) the resulting reactions, molecular equations, ionic equatons, and net ionic equations. No need to show work. Thank you!
[1] copper(II) sulfate + sodium hydroxide
[2] copper(II) sulfate + sodium carbonate
[3] copper(II) sulfate + lead(II) nitrate
[4] copper(II) sulfate + barium chloride
[5] copper(II) sulfate + sodium phosphate
[6] sodium carbonate + sulfuric acid
[7] sodium carbonate + hydrochloric acid
[8] cadmium(II) chloride + sodium sulfide
[9] cadmium(II) chloride + sodium hydroxide
[10] nickel(II) chloride + sodium acetate
[11] nickel(II) chloride + silver(I) nitrate
[12] nickel(II) chloride + sodium carbonate
[13] sulfuric acid + sodium hydroxide
[14] sulfuric acid + sodium acetate
[15] ammonium chloride + sodium hydroxide
[16] barium chloride + sodium phosphate
[17] lead(II) nitrate + sulfuric acid
[18] lead(II) nitrate + sodium sulfide
[19] sodium sulfide + hydrochloric acid
[20] potassium chloride + sodium nitrate
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A mixture of gases contains 8.23 g of N2, 8.80 g of H2, and 6.96 g of NH3. If the total pressure of the mixture is 3.05 atm, what is the partial pressure of each component?
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At 650 K, the reaction MgCO3(s)?MgO(s)+CO2(g) has Kp=0.026. A 12.8L container at 650 K has 1.0g of MgO(s) and CO2 at P = 0.0260 atm. The container is then compressed to a volume of 0.900L .
Find the mass of MgCO3 that is formed.
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Consider the titration of a 27.3 −mL sample of 0.125 M RbOH with 0.105 M HCl. Determine each of the following.
1. the initial pH
2. the volume of added acid required to reach the equivalence point
3.the pH at 5.6 mL of added acid
4. the pH at the equivalence point
5. the pH after adding 4.9 mL of acid beyond the equivalence point
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You add 0.535 g of NaOH to 100.0 mL of water at 25
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An organic compound contains carbon, hydrogen, and sulfur. A sample of it with a mass of 2.712 g was burned in oxygen to give gaseous CO2, H2O, and SO2. These gases were passed through 311.2 mL of an acidified 0.0200 M KMnO4 solution, which caused the SO2 to be oxidized to SO42-. Only part of the available KMnO4 was reduced to Mn2+. Next, 31.12 mL of 0.0300 M SnCl2 was added to 31.12 mL portion of this solution, which still contained unreduced KMnO4. There was more than enough added SnCl2 to cause all of the remaining MnO4- in the 31.12 mL portion to be reduced to Mn2+. The excess Sn2+ that still remained after the reaction was then titrated with 0.0100 M KMnO4, requiring 0.02095 L of the KMnO4 solution to reach the end point. Based upon all this data, the percentage of sulfur in the original sample of the organic compound that had been burned is___%.
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