Hydrogen is produced by a complete reaction of 6.24 g of sodium with an excess of gaseous hydrogen chloride, according to the balanced chemical reaction equation below.  How many liters of hydrogen gas will be produced if at a temperature of 50.0 °C and a pressure of 0.850 atm?   2 Na(s) + 2 HCl(g) → 2 NaCl(s) + H2(g)

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

for this question. Sodium metal reacts with water to produce hydrogen gas according to the following equation: 2Na(s) + 2H,0(1)→2NAOH(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 20 °C and a pressure of 759 mm Hg. If the wet H, mol. The vapor gas formed occupies a volume of 9.89 L, the number of moles of Na reacted was pressure of water is 17.5 mm Hg at 20 °C.

A sample of gas contains 0.1500 mol of CH₁ (g) and 0.3000 mol of O₂(g) and occupies a volume of 19.3 L. The following reaction takes place: CH4 (9) +202(g) → CO₂(g) + 2H₂O(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. Volume = L

Suppose you are performing a gas-producing reaction to experimentally determine the molar volume of the gas. MgCl₂ (aq) + H₂(g) Mg(s) + 2 HCl(aq) A sample of Mg produces 21.5 mL of H₂ gas. The gas is collected over water at an atmospheric pressure of 768.6 mm Hg at 22 °C, at which the vapor pressure of water is 19.8 mm Hg. What is the experimental value for the molar volume of the hydrogen gas in L/mol?

A mixture of He and CO2  is placed in a 7.5L flask at 22C. The partial pressure of the He is 2.2 atm and the partial pressure of the CO2 is 1.9 atm. What is the mole fraction of He?

You conducted an experiment in which you measured the molar volume of an ideal gas at STP. In this experiment, you formed hydrogen gas by reacting magnesium metal with hydrochloric acid: Mg (s) + 2 HCl (aq)àMgCl2 (aq) + H2 (g).The hydrogen gas was collected in a tube that contained the metal sample and which was submerged in the solution. a) Explain why hydrogen gas is a good choice of gas to use in an ideal gas experiment such as this. b) (i) Explain why the pressure of the hydrogen gas collected in the tube is not equal to the surrounding atmospheric pressure and (ii) describe the mathematical correction(s) that must be made to obtain the correct pressure.

a gas mixture contains sulfur hexaflouride at a pressure of 2.64 atms and diphosphorus pentoxide at a pressure of 1.58 atms. what is the mole fraction of diphosphorus pentoxide in this mixture?

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.

assume all reactions involving gases proceed at STP:  2 Li + 2 H2O  2 LiOH +H2.    If 4.4247 moles of Li are reacted,  how many moles of LiOh will be produced?