4) The equilibrium constant for the reaction shown below is 4.63 x 10-3 at 527oC.
COCl2(g) ó CO(g) + Cl2(g)
a)Write the equilibrium constant expression in terms of the chemical concentrations.
b)What is the equilibrium constant for the reverse reaction?
c)If 0.50 mol of COCl2 is placed in a 2.0 L flask, what will the concentration of all of the reactants and products be when the reaction reaches equilibrium at 527oC?
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A desert experiences much wider daily temperature variations than does a humid environment. Explain why this occurs.
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Please answer in atleast 1 paragraph...
1. Please explain the principle of affinity chromatography and then provide many (two or three) specific examples.
2. Describe the difference b/t step-gradient and the linear gradient. What are the advantages and the disadvantages in each?
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8.81) How many moles of a gas will occupy a volume of 0.61 L at a temperature of 331 K and a pressure of 3.0 atm ?
8.112) Part A. When fully inflated, a hot-air balloon has a volume of 1.6×105L at an average temperature of 395 K and 0.967 atm . Assuming that air has an average molar mass of 29 g/mol, what is the density of the air in the hot-air balloon?
Part B) How does this compare with the density of air at STP? It's less dense than at STP. It's more dense than at STP.
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I) Approximately 10 g of iron filings has been placed into a waste container of approximately 2L of 6M HCl.
1. Assuming 1 mole of H2 evolved will have the volume of 22.4L, how many liters of hydrogen gas will have been produced if the reaction forming hydrogen gas and iron (III) chloride were to go to completion? (Show calculations) (5 pts)
2. What are some of the hazards of this reaction? (5 pts)
3. What minimum container size would be necessary to fully neutralize the acid solution using 3M NaOH? Assume none of the hydrochloric acid has yet reacted. (Show calculations) (5 pts)
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Calculate the molar absorptivity of crystal violet using the absorbance value of the crystal violet solution determined in the lab and Beer’s law. How does this value compare with the value of 87,000 M-1 cm-1 at 590 nm reported in literature?
Absorbance value used in lab: 590 nm.
If not enough information to solve, please explain how I would go about solving this.
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A cylinder with a movable piston is filled at 24oC with a gas that occupies 36.2cm3. If the maximum capacity of the cylinder is 65.2cm3, what is the highest temperature to which the cylinder can be heated at constant pressure without having the piston come out?
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A 125.0 −mL sample of a solution that is 2.8×10−3 M in AgNO3 is mixed with a 220.0 −mL sample of a solution that is 0.10 M in NaCN . After the solution reaches equilibrium, what concentration of Ag+(aq) remains?
I have tried different ways and come up with these answers, all incorrect:
[Ag+] = 5.5e-15 M
[Ag+] = 1.9e-15 M
[Ag+] = 1.3e-22 M
Please show work.
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Calculate the Eocell for: Fe(s) + Br2(g) → Fe2+(aq) +Br-(aq) ; is this electrolytic or voltaic?
| A. | -1.52V ; voltaic | |
| B. | 1.52V ; electrolytic | |
| C. | -1.52V ; electrolytic | |
| D. | 1.52V ; voltaic |
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You are given a 5M solution and you need to make the following dilutions: 1 M, 100 mM, and 25 mM.
4A. What is the dilution factor for each of these dilutions?
4B. If you need 5 mL of each of the diluted solutions, how much of the 5M stock would you use, and how much water would you add? Show your work.
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The Kc for the following reaction at 225 ∘C is 1.7×102.
3H2(g)+N2(g)⇌2NH3(g)
If the equilibrium mixture contains 0.22 M H2 and 0.017 M N2, what
is the molar concentration of NH3?
Express your answer to two significant figures and include the appropriate units.
Enter your answer using dimensions of chemical concentration.
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Among Gas Chromatography, NMR spectroscopy, and distillation, which is better at identifying the unknown solvents? Which is better at determining % composition? Explain your answers about why is one better than other two and why the other two is not good?
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A fajans titration of a 0.9628 g sample containing chloride required 31.32 ml of 0.1001 M AgNO3. Express the result of this analysis in terms of the percent AlCl3 (FW= 133.34) in the sample.
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5. In Procedure II of Part 2 of the lab you will add the correct ratio of water to ice so that the final temperature of the water in the calorimeter is 0°C. Suppose you do this and get the following data: Mass of ice 23.5 g Mass of water originally in the calorimeter 73.79 g Initial temperature of water 25°C Final temperature of water and melted ice 0°C Determine ?Hfusion of water given these data. ----->5.92 kJ/mol
6. Given that ?Hfusion of water = 6.0 kJ/mol, determine the percent error with these data
__________%
7. In Procedure I of Part 2 of the lab, you add ice to more water than the minimum required. Questions 7-10 address this portion of the lab. Which of the following best describes what is in the calorimeter when the system reaches equilibrium?
a. There is only water in the calorimeter and the water is greater than 0°C.
b. There is a mixture of water and ice in the calorimeter and the temperature of the system is less than 0°C.
c. There is a mixture of water and ice in the calorimeter and the temperature of the system is 0°C.
d. There is a mixture of water and ice in the calorimeter and the temperature of the system is greater than 0°C.
e. There is only water in the calorimeter and the water is 0°C.
f. There is only water in the calorimeter and the water is less than 0°C.
8. So, you take ice out of the freezer and add it to room temperature water in a calorimeter (more than enough to just melt the ice). We can determine the ?Hfusion of water by assuming we can account for all energy transfer and that “heat lost” is equal to “heat gained”. We can assume that “heat lost” is due to which of the following? Check all that apply. Select all that are True.
a. Raising the temperature of ice to 0°C.
b. Cooling the calorimeter.
c. Melting the ice.
d. Raising the temperature of the melted ice from 0°C to the final temperature.
e. Cooling the water originally in the calorimeter.
9. We can assume that “heat gained” is due to which of the following? Check all that apply. Select all that are True.
a. Melting the ice.
b. Raising the temperature of the melted ice from 0°C to the final temperature.
c. Cooling the calorimeter.
d. Raising the temperature of ice to 0°C.
e. Cooling the water originally in the calorimeter.
10. We will use 29.1 g of ice and add it to 128.04 g of water at 25°C. Let’s assume that the ice starts at 0°C (we will allow the ice to sit out for a bit of time and “dry it” so we will make this assumption). For this PreLab assignment, let’s also assume we have a perfect calorimeter (you will judge this assumption in Part 1 of the lab). So, we have “heat lost” = “heat gained” as Cooling the 128.04 g of water originally in the calorimeter from 25°C to the final temperature = melting the 29.1 g of ice + raising the temperature of 29.1 g of the melted ice from 0°C to the final temperature. Given that ?Hfusion of water = 6.0 kJ/mol, determine the theoretical final temperature of the water left in the calorimeter when the system reaches equilibrium._____ °C
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