Calculate the partial pressure of helium gas for a volume of 1.0 × 106 m3 of 206Rn gas after 14 minutes. The radon gas was originally placed in an evacuated container at 1 atm, and the temperature remains constant at 0°C. (t,2 = 5.67 min for 206Rn.) 0.18 X atm What is the partial pressure of the radon gas after this time? atm

When a student reacted magnesium with HCl in a eudiometer, 37.60 mL of hydrogen gas was collected. The water level in the eudiometer was 2.08 cm below the water level in the beaker. The room atmosphere pressure in the lab was 764.12 mm Hg. At the time of collection, the lab was 23.4 C a) What is the corrected pressure of the dry hydrogen gas? b) What is the volume of the dry hydrogen gas at STP conditions? c) How many moles of hydrogen gas were collected?

A student completes the experiment The Universal Gas Constant and obtains the following data for one trial. mass of magnesium (g): Initial gas volume (ml): Final gas volume (ml): Temperature (°C): Atmospheric pressure (inHg): 30.39 Calculate the universal gas constant, R, for this trial. Assume that the water levels inside and outside the eudiometer tube are the same; that is, assume Ah = 0.00 cm water. Give your answer to two decimal places in the units of L-torr-mol-1. K-¹. 1 in Hg = 25.4 mmHg 1 cm water = 0.735559 mmHg 1 mol Mg = 24.305 g Mg on i TABLE D-4 TEMP DEGA C T 0 1 2 3 4 amm 14.579 4.612 4.646 | 4.660 4.714 4.924 4.959 4.9955.031 15.068 5.291 5.329 5.367 5.406 15.445 15.683 5.723 | 5.7645.805 5.146 16.100 1 6.143 6.1866.2306-274 1 6.318 10.6 I 0.7 J L 1 LI 1 4.7484.783 4.818 1 4.853 I 4.888 1 5.104 | 5.141 | 5.178 5.216 | 5.253 5.484 5.523 5.563 1 5.60215.647 I 5.888 | 5.930 | 5.972 1 6.014 1.6. 7_1 5.363 | 6.407 6.453 I 6.498 1 6.823 | 6. 871 6.919 1 6.967 1 1 | 6.544 |…

A balloon flying a long distance contains 1.2 x 107 L of helium. If the helium pressure is 737 mmHg at 25 ̊C, what mass of helium (in grams) does the balloon contain?

A student collected 500. mL of nitrogen at a temperature of 20.°C. The next day the student found that the volume had changed to 525 mL. What was the new temperature of the gas?

6. If excess carbon is present in a container that originally has 1:1 of CO and CO2 and no other gases, please explain the change of CO:CO2 ratio with increasing temperature.

8. A gas mixture contains Ar, He, and Kr at partial pressures of 125, 175, and 225 mmHg, respectively. If Ne is added until the total pressure is 623 mmHg, what is the partial pressure of Ne?

d) A 30.0 L sample of nitrogen gas inside a rigid, metal container at 20 °C is placed inside an oven whose temperature is 50 °C. The pressure inside the container at 20 °C was 3.00 atm. Determine the pressure of the nitrogen gas after its temperature is increased to 50.0 °C.

Time Left:0:55:00 A student completes the experiment The Universal Gas Constant and obtains the following data for one trial. mass of magnesium (g): Initial gas volume (ml): Final Volume (mL): Temperature (°C): Atmospheric pressure (inHg): Ah (cm of water): F3 80 모 Calculate the partial pressure of hydrogen, PH2, for this trial. Give your answer in torr (mmHg). 1 in Hg = 25.4 mmHg 1 cm water = 0.735559 mmHg 1 mol Mg = 24.305 g Mg TABLE D-4 TEMP 1_DEG₁_C_1 1 3 I 1 1 Q F4 0 1 = 2 3 4 5 6 7 8 10 11 12 13 14 0.0 0.1 0.0326 0.00 35.30 21.3 30.21 16 17.13 F5 6.100 | 6.143 1 6.544 1 6.589 0.2 1 VAPOR PRESSURE OF HATER 0-30 DEG. C IN MM HG 1 4.579 4.612 4.646 | 4.924 | 4.959 4.995 15.291 4.660 4.714 5.0315.068 5.329 5.367 5.406 5.445 4.7484.783 4.818 5.104 | 5.141 | 5.178 5.484 5.523 5.563 5.888 5.930 6.230 16.274 6.318 5.363 15.683 15.723 | 5.764 | 5.8051 5.146 6.186 6.636 5.972 1 6.0141 6.057 1 6.407 1 6.453 6.498 1 6.82 | 6.729 6.776 6.823 | 6.871 | 6.919 | 6.967 1 T T 1 I T I 1 17.0167,064…

A 9.00 L tank at 1.5 °C is filled with 7.53 g of chlorine pentafluoride gas and 18.2 g of carbon monoxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas mole fraction ? chlorine pentafluoride carbon monoxide