+ 6 HCl(aq) 2 AlCl3 (aq) + 3H₂(g) gas produced by this reaction is typically collected via water displacement. During this process, the hydrogen gas rated with water vapor. If 245.0 mL of gas with a total pressure of 1.43 atm is collected via water displacement at t is the partial pressure of the hydrogen gas in the sample? The vapor pressure of water at 29.4 °C is 30.75 torr. atm rams of aluminum must have reacted to produce this quantity of hydrogen gas? ninum: g

A 35.0 L sample of gas collected in the upper atmosphere at a pressure of 48.6 torr is compressed into a 150.0 ml. container at the same temperature. (a) What is the new pressure, in atmospheres? (b) To what volume would the original sample have had to be compressed to exert a pressure of 10.0 atm?

A sample of oxygen gas was collected via water displacement. Since the oxygen was collected via water displacement, the sample is saturated with water vapor. If the total pressure of the mixture at 26.4 °C is 791 torr, what is the partial pressure of oxygen? The vapor pressure of water at 26.4 °C is 25.81 mm Hg.

A flask of volume 0.753 L contains a sample of chlorine gas, Cl2, with a pressure of 198 Torr at 25.8 degrees C What mass of sodium, in grams, is required to completely react with the chlorine to make sodium chloride? 2 Na (s) + Cl (g) - - > 2 Na C1 (s)

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).

Enter your answer in the provided box. A piece of sodium metal reacts completely with water as follows: 2 Na(s)+2H2O(l)->2NaOH(aq)+H2(g)The hydrogen gas generated is collected over water at 23.0\   deg C. The volume of the gas is 291 mL measured at 0.965 atm. Calculate the number of grams of sodium used in the reaction. (The vapor pressure of water at 23.0\deg C=0.027 atm.)

Please don't provide handwritten solution ....

The van der Waals constants for HCl are a = 3.67 atm·liter2·mole–2, and b = 40.8 cc·mole–1. Find the critical constants of this substance.

0.300 mol of O2 gas is held at an a 5.00 L container at 45.0 °C. Determine the following:(a) the volume this gas occupies at ST (in L).(b) the pressure of this gas if the temperature isincreased to 60.0 °C assuming the volume does notchange.(c) the volume of NO2 (in L) expected from complete combustion of the excess N2 in O at STP.Hint: Use answer from (a) as a starting point.