Nitrogen gas in a steel container is under a pressure of 150. atm at 27 °C. What will the pressure in the tank be if the tank is left in the sun and the internal temperature rises to 55 °C?

What is the experimental molar mass (that is, calculated from the data given and not taken from the periodic table) of magnesium if 0.0327 grams of magnesium generates 34.85 mL of hydrogen at 24.1 °C with a hydrogen partial pressure of 715.2 torr? Note that the partial pressure of water vapor has already been subtracted from the total pressure.   A 19.5 g/mol   B 26.2 g/mol   C 22.4 g/mol   D 24.3 g/mol   E 26.0 g/mol

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?

Air entering the lungs ends up in tiny sacs called alveoli. It is from the alveoli that oxygen diffuses into the blood. The average radius of the alveoli is 0.0041 cm, and the air inside contains 14 percent oxygen. Assuming that the pressure in the alveoli is 1.0 atm and the temperature is 37 °C, calculate the number of oxygen molecules in one alveolus. For calculation purposes, assume that the average alveolus is a perfect sphere. Be sure your answer has the correct number of significant digits. Note: Reference the Fundamental Constants table for additional information. 8.486 x 10 10° | molecules x10

Jj.200.

HCl(g) can be made by the direct reaction of H2 and Cl2 in the presence of light. 6.00 g of H2 and 1.50 x 102 g Cl2 are mixed in a 5.00 L flask at 28.0 °C. What are the partial pressures of gases after the reaction has completed. Given Information:             > Temperature and volume remains constant at 28.0 °C             > Wavelength of light needed for the reaction is 340 nm.

Magnesium  metal reacts with molecular  chlorine  gas to form  magnesium   chloride . A closed container of volume  3 .00 x 103 mL contains  chlorine  gas at  2.26  °C and  6.52  x 105 Pa. Then  7.68  g of solid magnesium  is introduced, and the reaction goes to completion. What is the final pressure (in bar) if the temperature rises to  95.06  °C?

A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.

Given the reaction: 2 Al (s) + 6 HCI (ag) --> 2 AICI3 (aq) + 3 H2 (g) A strip of aluminum of unknown mass is reacted with excess hydrochloric acid. When the hydrogen gas is collected over water, it is done so at a temperature of 22.0 °C and fills a flask of volume 32.5 mL. The pressure inside the collection tube is 756.1 mmHg and the water vapor pressure at 22.0 °C is 19.83 torr. Determine the mass of the aluminum strip in milligrams (mg).

A 34.0 L metal cylinder stores a sample of gas at 26 °C under 1.42 atm. The temperature of the storage unit rises to 96 °C, causing the gas to decompose and doubling the number of moles in the cylinder.