5. Calculate the density of CO₂ in grams per liter (g/L) at a pressure of 752 mmHg and a temperature of 55°C. Use the molar masses: C = 12.01; O = 16.00. 34

Calculate the total pressure (in atm) of a mixture of 3.00 x 10-2 mol of helium, He, and 4.00 x 10- mol of oxygen, 02, in a 4.00 L flask at 20.°C. Assume ideal gas behavior. Total pressure = atm

9. a) You have determined experimentally that at standard temperature and pressure (0 °C and 1 atm) that you have a gas weighing 0.1977 g in a 100 mL sealed container. What is the molecular weight of the unknown gas?

A sample of nitrogen gas has a volume of 167.0 mL at STP. What volume (in mL) does the gas occupy if the temperature is increased by 55.3 ºC and the pressure is doubled? 200.0 mL of 3.96 M hydrochloric acid is added to 100.0 mL of 4.60 M barium hydroxide. After the reaction goes to completion, what is the concentration (in mol/L) of the excess H+(aq) or OH–(aq) that remains in solution? Assume that the volumes are additive. Aqueous solutions of the following reactants are mixed. After the reaction goes to completion, calculate the concentration (in mol/L) of silver ions in solution. 160.0 mL of 3.50 M AgNO3 are mixed with 150.0 mL of 1.50 M CaCl2. Consider the following reaction: 2 NH3 (g)   +   3 Cl2 (g)   →   N2 (g)   +   6 HCl (g) A mixture is prepared from 15.0 mol of ammonia and 15.0 mol of chlorine gas. Determine the total moles of gas in the container after the reaction has gone to completion.

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 |…

1. Calculate the density of oxygen, O2, under each of the following conditions: STP 1.00 atmatm and 10.0  ∘C 2. To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 3.8-L bulb, then filled it with the gas at 1.70 atm and 20.0 ∘C and weighed it again. The difference in mass was 7.5 g . Identify the gas. Express your answer as a chemical formula.

5. You are given 1.56 g of a mixture of KClO3 and KC1. When the mixture is heated the oxygen gas liberated displaces 327 mL of water at a temperature of 19°C. The total pressure of the gas in the collection flask is 735 mmHg. What is the percentage of KClO3 in the mixture?

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.

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…