A 500mL sample of O2 gas at 24 degrees Celsius was prepared by decomposing a 3% aqueous solution of hydrogen peroxide, H2O2, in the presence of a small amount of manganese catalyst by the reaction: 2H2O2(aq) -------> 2H2O(g) + O2(g)   The oxygen thus prepared was collected by displacement of water. The total pressure of gas collected was 755 mm Hg. What is the partial pressure of O2 in the mixture? How many moles of O2 are in the mixture? Please note that the vapor pressure of water at 24 degrees Celsius is 23 mm Hg.

Using stoichiometry, calculate the volume of O2 gas at 1.25 atm and 18.0 ̊C, which forms when 10.5 g KClO3 decomposes according to the reaction:2 KClO3 → 2 KCl + 3 O2

What is the percent yield when 0.0506 mole of H2O2 decomposes and experimentally produces 375 mL of O2 gas measured at 42 degrees Celsius and 1.52 atm 2H2O2(aq) --> 2H2O(l) + O2(g)

A 0.6333 g sample of a metal carbonate was reacted with hydrochloric acid. The carbon dioxide gas generated was collected over water at a temperature of 26.0°C and pressure of 103.80 kPa. The final volume of carbon dioxide gas collected was 125.0 mL.  XCO₃(s) + 2HCl(aq) → XCl₂(aq) + H₂O(l) + CO₂(g)   Find the moles of the metal carbonate reacted.

At 287 K and 1.43*10^-2 atm, the density of a gas is 1.37*10^-5 g/cm^3. (a) Find the Vrms for the gas molecules. (b) Find the molar mass of the gas.

Hydrogen gas generated from the reaction of aluminum with hydrochloric acid was collected over water at 20°C. If 18.5 mL of gas was collected at an atmospheric pressure of 0.826 atm, how many mmol (millimoles) of aluminum reacted? The vapor pressure of water at 20°C is 17.55 torr. Give your answer to 3 sig figs.   2 Al(s) + 6 HCl(aq) -> 2 AlCl3(aq) + 3 H2 (g)

A sample of 3.42 mol of xenon is confined at low pressure in a volume at a temperature of 86 °C. Describe quantitatively the effects of each of the following changes on the pressure, the average kinetic energy per molecule in the gas, and the root-mean-square speed. (a) The temperature is increased to 199 °C (b) The volume is tripled. (c) The amount of xenon is decreased to 1.87 mol Give each answer as a decimal factor of the form: new value factor old value. A factor of 1 means no change. ChangeP KEavgms

Please answer questions 1-3 Please refer to the picture below:

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).

The ideal gas law, PV = nRT is independent of the kind of gas. In other words, the pressure exerted by a given number of ideal gas particles is the same whether the sample consists of all one type of particle or a mixture of different kinds of particles. Air is about 78.0% nitrogen molecules and 21.0% oxygen molecules. Several other gases make up the remaining 1% of air molecules. Therefore, the pressure exerted by a mixture of gases can be expressed as follows: Part A Tota RT Ptotal = V What is the partial pressure of nitrogen in air at atmospheric pressure (101 kPa)? Assume ideal behaviour. A partial pressure is the pressure exerted by just one type of gas in a mixture. A partial pressure is calculated using only the number of moles of that particular gas, instead of the total number of moles: Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) RT P = V P = nRT P= nRT etc. The sum of the partial pressures is equal to the total…