lab004_diffusion01

Calculate the height of a column of water equivalent to 1.00 bar. The density of water is 1.00 g/cm3; the density of mercury is 13.53 g/cm3. Physical Chemistry 1  please provide complete solution.

nto each of two containers of water you place 1 mole each of two substances A and B. Both substances mix well and dissolve in H2O. A has a molecular weight of 450 and B of 100. Which container will have the faster diffusion rate?

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The rate of diffusion of an unknown gas was determined to be 92 times greater than that of NH3. What is the approximate molar mass of the unknown gas? show your solution

A student constructs a simple constant volume gas thermometer and calibrates it using the boiling point of water, 100°C, and the freezing point of a specific brine solution, -17°C. The pressures measured at the calibration points are 1.366 atm and 0.9267 atm, respectively.   **when explaining please use math symbols & equations rather than typing it out, gets confusing if something is in a fraction or whatnot. Thank you!

Why would you expect the rate of diffusion to increase with temperature? Can you give an example, such as the fact that you can dissolve sugar more rapidly in hot water?

What is the root mean speed in m/s of Krat 15°C? (write the solution without decimals)

What is the root mean speed in m/s of I2 at 15°C? (write the solution without decimals)

Use Boyle's law, P1V1 = P2V2, to calculate the volume, in mL, of the dry H2 at room pressure.  Please enter your volumes using three decimal places and do not use scientific notation.   partial pressure of the dry H2 in Torr = 734.7 torr moles of magnesium and moles of hydrogen gas produced in each trial -  trial 1 - 0.003188 trial 2 - 0.003225 trial 3 - 0.003163

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7. On your own: In our lives, we rarely experience temperatures that are above 373 K (100 °C) or below 273 K (0 °C). Investigate how much diffusion rates differ between these two temperatures. Describe the results of your experiments below.

A solution is made by mixing 128. g of acetic acid (HCH3CO₂) and 34. g of acetone ((CH3)₂CO). Calculate the mole fraction of acetic acid in this solution. Round your answer to 3 significant digits. 0 Ś

1.) Compound X is an unknown hydrocarbon (a compound made up of only carbon and hydrogen) and is 82.64% carbon. Compound X effuses at a rate 0.525 slower than that of methane gas, CH4. What is the molecular weight (in g/mole) of Compound X? What is the empirical formula of Compound X? What is the molecular formula of Compound X? Please show the solution.

I need solutions for all parts

14. From the following gases: N₂ (MM = 28.02) CO₂ (MM = 44.01) He (MM = 4.00) Kr (MM = 83.80) (a) Which gas will diffuse faster than CO (MM = 28.01)? (b) Which gas will diffuse at about the same rate as CO? (c) The rate of diffusion of CO is square root of three (√3) as the rate of diffusion of an unknown gas. Which gas satisfies this condition?

What happened to the water inside the bottle?

200 ml in 1 m3 is how many PPM? 75 L of vapor in 2000 ft3 of vapor is how many PPM?

Can anybody help me? Thanks. The partial pressure of oxygen in the lungs is about 150 mm of Hg. (The partial pressure is the pressure of the oxygen alone, if all other gases were removed.) This corresponds to a concentration of 5.3×10^24 molecules per m^3. In the oxygen-depleted blood entering the pulmonary capillaries, the concentration is 1.4×10^24 molecules per m^3. The blood is separated from air in the alveoli of the lungs by a 1-μm -thick membrane. Assume the diffusion coefficient for oxygen in tissue is 2×10^−11m^2/s. 1.) What is the rate of transfer of oxygen to the blood through the 5×10^−9  surface area of one alveolus? Give your answer in molecules/s. Give your answer to 1 significant figure. 2.) What is the same rate of transfer in μmol/s? Give your answer to 1 significant figure.

Suppose a student repeated Lab 1 using a different divalent metal X. The molar mass of metal X is 43.8 g/mol. An unknown mass of metal X was reacted with excess HCI (1 mole of Metal X produces 1 mole of H2 gas). The volume of H, gas produced was 26.53 mL. The reaction was performed at an atmospheric pressure of 547.6 mm Hg and at 18.0 °C. Calculate the mass of metal X that was used in the reaction. (Ignore the water vapour pressure (pH,O)) L-mm Hg R=62.4 7mol-K Answer:

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In the vacuum of space, the air pressure is so low, that water boils and freezes at the same time. At what pressure is the boiling point of water the same as its freezing point? Use the same experimental P1 and T1 values as in the previous calculations, but this time use T2 as the freezing point of water. Make sure your units cancel. P1= 1500 torr T1= 400 P2 (Freezing Point)= 351.4

Can you help me with the number 4 question? Can you explain step by step including the formula (Boyle’s law)? I need to plug in the fraction to give the correct answer.

Watch the demonstration of Gay-Lussac’s Law and answer questions pertaining to it: https://www.youtube.com/watch?v=1pVVZGOBIVg When the Gay Lussac’s device was inserted in boiling water, what was the pressure that was recorded? What happened to the pressure of the gas in the Gay Lussac’s apparatus when it was dipped in mixed water bath (regular water + boiling water)? Did it increase or decrease?  In this experiment which of the following relationships are being tested? Relationship between Volume and Temperature Relationship between Volume and Pressure Relationship between Pressure and Temperature

What is the concentration of propane (in units of grams per liter) dissolved in water at 25°C, when the C3Hg gas over the solution has a partial pressure of 399 mm Hg? k for C3Hg at 25°C is 1.44x10-4 mol/L.atm. Submit Answer g/L ccess important values if needed for this question. Retry Entire Group 8 more group attempts remaining Cengage Learning Cengage Technical Support Previous Next Save and Exit

Workers in underwater caissons or diving suits necessarily breathe air at greater than normal pressures. If they are returned to the surface too rapidly, N2, dissolved in their blood at the previously higher pressure, comes out of solution and may cause emboli, bends, and decomposition sickness. Blood at 37 °C and 1 atm pressure dissolves 1.3 mL of N2 gas per 100 mL of blood. Compute the volume of N2 likely to be liberated from the blood of a caisson worker who is returned to 1 atm pressure after prolonged exposure to air pressure at a depth of 300 m of water. The total blood volume of the average adult is 4.8 L. Also note that air contains 78% N2 by volume. 6.

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