MnO2 (s) + 2 CO (g) → Mn (s) + 2 CO2 (g)
5. Calculate ΔG at 298K if MnO2 = 0.150 mol, Mn = 0.850 mol, CO = 0.250 M and CO2 = 0.500 M in a 1.25 L flask.
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This question has already been answered, but there was not as much detail as i needed to understand what exactly to do and i need to understand it quick... could you please walk me through how to do this, but specifically A and B please plug in all numbers and state where they came from , thank you so much!
Calculate the potential in the following cell
Pb|Pb2+(1.00M)|| Ag+(1.00M) |Ag
a. right at the beginning when you start using this voltaic cell,
b. when 50% of the Ag+ ions have been consumed,
c. when 99% of the Ag+ ions have been consumed, and
d. when 99.99% of the Ag+ ions have been consumed. Keep in mind that both, the Pb2+ and the Ag+ concentrations are changing.
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The Henry's law constant (kh) for Ar in water at 20°C
is 0.0015 mol/(L atm). How many grams of gas will dissolve in 2.78
L of H2O in contact with pure Ar at 1.6 atm?
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describe the actuve location (S) of hemoglobin and myoglobin. How does the former function to transport 02 from the lungs to the cells where it is used?
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What is the silver ion concentration in a solution prepared by mixing 413 mL 0.356 M413 mL 0.356 M silver nitrate with 453 mL 0.438 M453 mL 0.438 M sodium phosphate? The KspKsp of silver phosphate is 2.8×10−18.
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The reaction A → B + C is known to be first order in A. Below are data showing the concentration of A as a function of reaction time.
| Time, h | [A], M |
| 0.5 | 5.00 x 10-2 |
| 1 | 4.51 x 10-2 |
| 2 | 4.06 x 10-2 |
| 3 | 3.30 x 10-2 |
| 4 | 2.18 x 10-2 |
| 5 | 1.77 x 10-2 |
| 6 | 1.44 x 10-2 |
(a) What is the average rate of reaction between 0.5 and 2 h? Report the units as well as the numbers.
(b) Plot the data above, showing the concentration of A as a function of the time. From your graph, determine the instantaneous rate of reaction at 4 h. Report the units as well as the numbers.
(c) Plot ln [A] versus time. Estimate the rate constant for this first-order reaction from your graph. Report the units as well as the numbers.
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A student is examining a bacterium under the microscope. The E. coli bacterial cell has a mass of m = 1.80 fg (where a femtogram, fg, is 10−15g) and is swimming at a velocity of v = 2.00 μm/s , with an uncertainty in the velocity of 5.00 % . E. coli bacterial cells are around 1 μm ( 10−6 m) in length. The student is supposed to observe the bacterium and make a drawing. However, the student, having just learned about the Heisenberg uncertainty principle in physics class, complains that she cannot make the drawing. She claims that the uncertainty of the bacterium's position is greater than the microscope's viewing field, and the bacterium is thus impossible to locate. Part A What is the uncertainty of the position of the bacterium
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Answer the following questions based on HSAB theory. If using Fajans Rules, give the rule number and explain why it applies.
1. Explain why aluminum perchlorate is less soluble than aluminum cyanide. This is unusual since perchorates tend to be very soluble.
2. Explain why the Ksp for FeBr2 is 4.1 x 10–4 and the Ksp for FeF2 is 3.2 x 19–7.
3. Explain why the Ksp for Fe(OH)3 is 1.2 x 10–36 and the Ksp for Fe(OH)2 is 7.8 x 10–16.
4. Explain why VS is more soluble than NiS.
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How do I identify HOMO and LUMO when given orbitals
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A 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of a 0.05832 M EDTA solution. The solution is then back titrated with 0.02380 M Zn2 solution at a pH of 5. A volume of 18.49 mL of the Zn2 solution was needed to reach the xylenol orange end point. A 2.000-mL aliquot of the Cu2 and Ni2 solution is fed through an ion-exchange column that retains Ni2 . The Cu2 that passed through the column is treated with 25.00 mL 0.05832 M EDTA. This solution required 23.22 mL of 0.02380 M Zn2 for back titration. The Ni2 extracted from the column was treated witn 25.00 mL of 0.05832 M EDTA.
How many milliliters of 0.02380 M Zn2 is required for the back titration of the Ni2 solution?
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Silver bromide is used to coat ordinary black-and-whitep hotographic film, while high-speed film uses silver iodide.
(a) When 96.0 mL of 5.0 g/LAgNO3 is added to a
coffee-cup calorimeter containing 96.0 mL of 5.0 g/L NaI, with both
solutions at 25°C,what mass of AgI forms in gram?
(b) Use Appendix B tofind ΔH°rxn. in kJ
(c) What is ΔTsoln (assume thevolumes are
additive and the solution has the density and specific heat
capacity of water)? in K
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Dinitrogen pentoxide (N2O5) decomposes in chloroform as a solvent to yield NO2 and O2. The decomposition is first order with a rate constant at 45 oC of 1.0 x 10–5 s–1. Calculate the partial pressure (in atm) of O2 produced from 1.00 L of 0.600 M N2O5 solution at 45 oC over a period of 20.0 h if the gas is collected in a 10.0-L container. (assume that the products do not dissolve in chloroform.)
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The combustion of acetylene C2H2 is a spontaneous reaction given by the equation: 2C2H2 (g) + SO2(g) --> 4CO2 (g) + 2 H2O(l)
As expected for a combustion the a combustion the reaction is exothermic.
a.) What is the sign of Delta H?
b.) What do you expect for the sign of Delta S?
c.) Explain the spontaneity of the reaction in terms of the enthalpy and entropy changes.
Please show work and explain
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Suppose you titrate 80.0 mL of 2.00 M NaOH with 20.0 mL of 4.00 M HCl. What is the final concentration of OH- ions.
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In a study designed to prepare new gasoline-resistant coatings, a polymer chemist dissolves 6.077 g poly(vinyl alcohol) in enough water to make 100.0 mL of solution. At 25
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