Hydrogen gas is produced by the reaction between metallic aluminum and aqueous hydrochloric acid.   2Al(s)+6HCl(aq)⟶2AlCl3(aq)+3H2(g) The hydrogen gas produced by this reaction is typically collected via water displacement. During this process, the hydrogen gas becomes saturated with water vapor. If 283.3 mL of gas with a total pressure of 1.45 atm is collected via water displacement at 29.4 ∘C, what is the partial pressure of the hydrogen gas in the sample? The vapor pressure of water at 29.4 ∘C is 30.75 torr. How many grams of aluminum must have

1) Calculate the volume of 1.62g of Helium gas at 25.670C and 872 mmHg. (R = 0.0821 atm.L/mol.K)    2)   Given the following reaction of Ca(s) in HCl(aq): Ca(s)    +     2 HCl(aq)     -->     CaCl2(aq)     +    H2(g)  If 32.7g of calcium solid are placed in this reaction and at the end of the experiment, hydrogen gas is produced at 25.000C and with a pressure of 790. mmHg. Calculate the volume of hydrogen gas produced.  3)   An unknown gas with a mass of 1.211g occupies a volume of 677 mL. The temperature is 230C and the air pressure is 0.987 atm. Calculate the molar mass of the gas.

For many purposes we can treat butane (C,H10) as an ideal gas at temperatures above its boiling point of – 1. °C. 3 Suppose the pressure on a 8.0 m° sample of butane gas at 11.0°C is reduced to one-third its initial value. O yes Is it possible to change the temperature of the butane at the same time such that the volume of the gas doesn't change? olo O no If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C. Explanation Check © 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility

Dry ice is solid carbon dioxide. A 1.47−g sample of dry ice is placed in an evacuated 4.37−L vessel at 27.0°C. Calculate the pressure inside the vessel after all the dry ice has been converted to CO2 gas.

An unknown mass of aluminum is added to HCl solution. The aluminum metal is completely dissolved in the solution and generates hydrogen gas. See the balanced equation for the gas evolution reaction: 2 Al(s) + 6 HCl(aq) ---> 2 AlCl3(aq) + 3 H2(g) The following data is collected: Mass of Al sample:                             unknown  g Volume of gas collected                     45.38 mL Barometric pressure                            754.8 mmHg Temperature                                        23.5OC Vapor pressure of H2O at 23.5OC       21.65 mmHg Hydrogen gas is collected over water. The reaction proceeds until all the amount of aluminum is consumed in the gas-evolution reaction (aluminum is the limiting reactant). (a) Calculate the mole number of the hydrogen gas generated in the reaction: Convert the volume of the collected gas to L:  45.38 mL = ___________ L Calculate the pressure exerted by H2 gas (= dry hydrogen gas):          Pressure of the dry hydrogen gas          =…

Consider the following situation:  You have a 50 L tank of compressed air at 15 atm and 100 ºC.  You then pass the compressed air through a "titanium getter" which contains fragments of hot titanium metal.  The purpose of the "getter" is to remove oxygen gas from the sample as Ti reacts with oxygen to form solid TiO2 (known as titania).  Once the purified air is passed through the getter is it cooled back down to  100 ºC and fills another 50 L storage tank.  If air typically contains about 20% oxygen, what could the pressure in the storage tank be?     Question 2 options:   A)  12 atm   B)  15 atm   C)  18 atm   D)  24 atm

A tank was filled with 18 g of oxygen (O2), 75 g of nitrogen (N2) and 4 g of carbon dioxide(CO2). At 25°C the pressure of the tank was 8.5 atm. If the partial pressure of CO2 in the tank is x atm, what is the value of x?

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).

Use the ideal gas equation to calculate the number of moles of hydrogen gas produced from a reaction between hydrochloric acid, HCl, and magnesium metal in which 12.0 liters of gas was collected at 22.0 C with a barometric pressure of 761.09 torr. The gas was collected over water with a vapor pressure pf 19.83 torr. R= 82.1 atm mL/mol K     or       R= 0.0821 atm mL/mol K