Oxygen therapy uses various devices to provide oxygen
to patients having difficulty getting sufficient amounts from air
through normal breathing.
Among the devices are nasal cannula, which transport oxygen through
small plastic tubes from a supply tank to prongs placed in the
nostrils.
Consider a specific configuration in which the supply tank (volume
= 3.00 ft3) was filled to a pressure of 2100.0 psig at a
temperature of -30.0°F.
The patient is in an environment where the ambient temperature is
40.0°F.
When the tank is used, the pressure begins to decrease as oxygen
flows at 5.00 L/min through a tube to the cannula where it is
discharged into the nostrils.
Estimate the original mass of oxygen in the tank using the compressibility-factor equation of state. (kg O2)
What is the initial pressure when the temperature is 40.0°F? (atm absolute)
How long will it take for the gauge on the tank to read 50.0 psig at an atmospheric pressure of 1 atm and the stated discharge? (.... x 10^3 min)
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To 1.0 L of a 0.34 M solution of HClO2 is added 0.15 mol of NaF. Calculate the [HClO2] at equilibrium.
PLEASE show ALL work!!
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A 1.08×103-mg sample of impure potassium carbonate was titrated with 46.09 mL of 0.2770 M perchloric acid. Calculate the percentage ofpotassium carbonate in the sample.
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What information about the progress of the synthesis of acetaminophen could be inferred from the TLC?
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In IR spectroscopy, why do heavier atoms have IR absorptions at lower frequencies?
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Calculate the amount (in mL) of 0.0462M calcium hydroxide that would be required to completely react with 126.25 mL of a 0.0182M HCl solution. do not enter the unit mL in your answer.
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Write a short account on the chemical and IR spectroscopic evidence for the existence of benzyne.
Despite the expense and time commitment, the total synthesis of large natural products continues to be of great use. Give two reasons why.
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In each situation below, we are adding aqueous solutions of HNO3 to NH3, and the calculating the PH of solution formed. (For ammonia Kb=1.8x10^-5)
a)Write the reaction that describes what happens when HNO3 is added to NH3. Do not include spectator ions.
b)What is the pH if 52.0mL of 0.120 M HNO3 added to 50.0mL of 0.120 M NH3?
c)What is the pH if 50.0mL of 0.120 M HNO3 added to 50.0mL of 0.120 M NH3?
Could you please explain each step rather than simply giving me the answer, I am trying to understand the concepts.
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You have a solution that contains 25 g of an unknown non-ionizing polymer in a 250 mL solution of chloroform (CHCl3 ). The osmotic pressure of this solution at 25 ◦C is found to be 0.056 atm. What is the molecular weight of the unknown solid?
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Choose a False statement:
| Allosterity can not be negative |
| none of the answers are correct |
| Homotropic regulation occurs when a normal ligand of the protein is the allosteric regulator |
| Heterotropic regulation occurs when a different ligand affects binding of the normal ligand |
| Positive cooperativity corresponds to positive homotropic regulation |
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The weak acid HZ has a Ka of 2.55 x 10-4. Calculate the pH of a 0.235 M solution.
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A 6.00-L sample of C 2 H 4 (g) at 2.00 atm and 293 K is burned
in 6.00 L of oxygen
gas at the same temperature and pressure to form carbon dioxide and
liquid water.
If the reaction goes to completion, what is the final volume of all
gases at 2.00 atm
and 293 K?
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Solid carbon can react with gaseous water to form carbon monoxide gas and hydrogen gas. The equilibrium constant for the reaction at 700.0 K is K p =1.60× 10 −3 . If a 1.55- L reaction vessel initially contains 157 torr of water at 700.0 K in contact with excess solid carbon, find the percent by mass of hydrogen gas of the gaseous reaction mixture at equilibrium.
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1. Calculate the change in total internal energy for a system that releases 2.38 × 104 kJ of heat and does 6.80 × 104 kJ of work on the surroundings. Enter your answer in scientific notation.
2. In a gas expansion, 69 J of heat is absorbed by the system, and the energy of the system decreases by 114 J.
Calculate the work done.
3. Be sure to answer all parts. Given the thermochemical equation for photosynthesis, 6H2O(l) + 6CO2(g) →C6H12O6(s) + 6O2(g) . ΔH = +2803 kJ/mol. Calculate the solar energy required to produce 8503 g of C6H12O6.
4. In a constant-pressure calorimetry experiment, a reaction gives off 23.8 kJ of heat. The calorimeter contains 150 g of water, initially at 25.4 c. What is the final temperature of the water? The heat capacity of the calorimeter is negligibly small.
5. A piece of silver with a mass 4.10 ×102 g has a
heat capacity of 97.2 J/° C. What is the specific heat of
silver?
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