1.
The equilibrium constant is given for one of the reactions
below. Determine the value of the missing equilibrium
constant.
2 HD(g) ↔ H2(g) + D2(g) Kc = 0.28
3 H2(g) + 3 D2(g) ↔ 6 HD(g) Kc = ?
2.
The reaction A(g)⇌2B(g) has an equilibrium constant of K = 0.070. What is the equilibrium constant for the reaction B(g)⇌12A(g)?
3.
Consider the reaction:
SO2Cl2(g)⇌SO2(g)+Cl2(g)
Kp=2.91×103 at 298 K
In a reaction at equilibrium, the partial pressure of SO2 is 158
torr and that of Cl2 is 307 torr .
Part A
What is the partial pressure of SO2Cl2 in this mixture?
PLEASE EXPLAIN HOW YOU GOT TO EACH ANSWER IN DETAIL. THANK YOU IN ADVANCE!
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A 6.00 g sugar cube (sucrose: C12H22O11) is dissolved in a 350 mL teapot containing 80∘ C water (density of water at 80∘ C= 0.975 g/mL). What is the molality of the sugar solution?
Express the molality with the appropriate units.
Calcium chloride, CaCl2, is commonly used as an electrolyte in sports drinks and other beverages, including bottled water. A solution is made by adding 8.50 g of CaCl2 to 60.0 mL of water at 25∘C. The density of the solvent at that temperature is 0.997 g/mL. Calculate the mole percent of CaCl2 in the solution.
Express your answer as a percent to three significant figures.
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Can someone please explain what a aug-cc-pVDZ basis set is in Physical chemistry using Gaussian?
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A 2.687 gram sample containing an unknown amount of arsenic trichloride and the rest inerts was dissolved into a NaHCO3 and HCl aqueous solution. To this solution was added 1.900 grams of KI and 50.00 mL of a 0.00895 M KIO3 solution. The excess I3– was titrated with 50.00 mL of a 0.02000 M Na2S2O3 solution. What was the mass percent of arsenic trichloride in the original sample?
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Complete the following table:
| Mass | Mol | Volume | ||
| Solute | Solute | Solute | Solution | Molarity |
| KNO3 | 23.5g | _____ | 127.0mL | _____ |
| NaHCO3 | _____ | _____ | 260.0mL | 0.150M |
| C12H22O11 | 57.38g | _____ | _____ | 0.120M |
Part A
Complete the row for KNO3.
Enter your answers numerically separated by a comma.
Part B
Complete the row for NaHCO3.
Enter your answers numerically separated by a comma.
Part C
Complete the row for C12H22O11.
Enter your answers numerically separated by a comma.
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1.What is the solubility of CoCO3(s) in solution that is well-buffered at pH 4.0?
(CoCO3: Ksp=1X1010, H2CO3: Ka1 = 4.45 x 10-7; Ka2= 4.69 X 10-11)
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Hydrogen chloride can be made in the labatory by the reaction of sodium chloride and sulfric acid!
___NaCl(s)+______H2SO4(aq)____HCl(aq)_____Na2SO4(aq)
Blance the above equation
If 35. g of NaCl are used , How many grams of H2SO4 are required for a complete reaction
If 35. g of NaCl are used , and only 8.6g of HCl are isolated what is the percentage yield of HCl
If only 8.6 g of HCl are obtained , How many grams of Na2SO4, must have been formed.
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What initial volume (in mL) will 0.00660 mol of hydrogen gas occupy at a pressure of 0.907 atm and a temperature of 9°C? If you heat the sample up to 45°C and maintains a constant pressure, what is the final volume (in mL)?
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You have 25.00 mL of a 0.250 M aqueous solution of the weak base CH3NH2 (Kb = 5.00 x 10-4). This solution will be titrated with 0.250 M HCl.
(a) How many mL of acid must be added to reach the equivalence point?
(b) What is the pH of the solution before any acid is added?
(c) What is the pH of the solution after 5.00 mL of acid has been added?
(d) What is the pH of the solution at the equivalence point of the titration?
(e) What is the pH of the solution when 30.00 mL of acid has been added?
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How does sodiums structure determine its properties?
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A volume of 6.0 mLs of 4.0 N NaOH (FW = 40g/mol) is added to a solution containing 2.50g of tri-protonated Lysine Acid (FW = 147 g/mol). What is the pH of the final solution?
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A mixture of 0.750 atm ClF3 , 0.554 atm F2 , and 0.394 atm ClF is heated in a closed vessel to 700 K .
ClF3(g)↽−−⇀ClF(g)+F2(g)Kp=0.140 at 700 K
Calculate the equilibrium pressure of each gas at 700 K .
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Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of a 0.10 M solution of aspirin (acetylsalicic acid, Ka = 3.0 × 10–4) solution.
| A. |
2.9 |
|
| B. |
10.5 |
|
| C. |
4.1 |
|
| D. |
3.5 |
|
| E. |
1.8 |
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Calculate the amount of heat that must be absorbed by 50.0 grams of ice at -12.0oC to convert it to water at 20.0oC. (specific heat capacity of ice = 2.09 J/g.K; specific heat capacity of liquid water = 4.18 J/g.K; specific heat capacity of water vapor = 1.84 J/g.K; heat of fusion of ice = 334 J/g
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Some NH4I is palced in a reaction placed in a closed container, which is then heated to 400 deg. C. If the total pressure in the container is (7.47x10^2) , mm Hg, what is the value of Kp. Remember to convert the pressures to atm's.
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