2S(s)+3O2(g)+2H2O(l)⟶2H2SO4(aq)2S(s)+3O2(g)+2H2O(l)⟶2H2SO4(aq) The chemical reaction shown above is carried out in a movable container at 312.4 K and a pressure of 4.5 atm.  What volume of O2O2 gas would be needed if the reaction is started with 135.3 grams of water, H2OH2O.  Round your answer to two decimal places. The molar mass of H2OH2O is 18 g/mol. R=0.0821L⋅atmmol⋅KR=0.0821L⋅atmmol⋅K R=62.4L⋅mmHgmol⋅KR=62.4L⋅mmHgmol⋅K Equation: PV=nRT

Gaseous iodine pentafluoride, IF₅, can be prepared by the reaction of solid iodine and gaseous fluorine: I₂(s) + 5F₂(g) → 2IF₅(g) A 10.00 L flask is charged with 15.0 grams of I₂ and 2.00 atm of F₂ at 25°C. The flask is heated to 100°C until one of the reagents is completely consumed. What will be the percentage of IF₅ (by mole) in the final product mixture? (Assume ideal gas behavior).

Ammonia burns in oxygen in the presence of a platinum catalyst to produce nitrogen monoxide and water by the following reaction: 4NH3(g) +50₂ (g) 4NO (g) + 6H₂O (1) If 9.00 g of ammonia is burned in excess oxygen, what is the mass of water that will be produced and the volume of NO gas if the reaction was carried out at 25 °C under a pressure of 100 kPa? K Periodic Table of the Elements -=||||2||×||2||81|41| Be Ca Sc Ba Fr Ra 67-71 09-103 22 Ti IN 23 24 25 41 25 27 28 29 30 Cr Mn Fe Co Ni Cu Mal 40 41 445 47 Zr Nb Mo Tc Ru Rh Pd Ag Hf Ta Series La La "Ac Th Pa Symbol Albe Viety Re Os Pt Au Hg Malay Alkaline Transition Basic Esth 13 13. Now Al Si 14 Ga Ge Noble Bas Tl Pb Bi Po At Rn 104 105 105 107 108 109 110 111 112 Rf Db Sg Bh Hs Mt Ds Rg Cn Uut "FI Uup "Lv Uus Uuo Sn Sb La The mass of water is 8.2 g and the volume of gas is 7.6 L. The mass of water is 6.4 g and the volume of gas is 11.1 L. LIBUR Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Es Fm Md No 100 102. Np Pu Am Cm Bk The mass…

A small amount of oxygen gas may be prepared in the laboratory by the decomposition of potassium chlorate, KClO3, according to the following equation: 2KClO3(s)  2KCl(s) + 3O2(g) A 1.54-g sample of KClO3 is completely decomposed and the oxygen gas produced is collected over water at 25oC and at a total pressure of 757.0 torrs. (a) If the vapor pressure of water at 25oC is 23.8 torr, what is the partial pressure of O2 collected? (b) How many milliliters (mL) of O2 gas are collected under the stated condition? What is the volume of O2 gas if collected at STP?

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 292.0 mL of gas with a total pressure of 1.33 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. ?H2=---- atm How many grams of aluminum must have reacted to produce this quantity of hydrogen gas? mass of aluminum:

What pressure (in torr) of carbon dioxide gas can be produced by the combustion of 1.00 g of benzene (C6H6) in a closed, 25.0 L container at a temperature of 15°C?   2C6H6(l)+15O2(g)-->12CO2(g)+6H2O(l)

The chlorination of methane occurs in a number of steps that results in the formation of chloromethane and hydrogen chloride. The overall reaction is 2CH,(g)+3Cl,(g)–2CH,CI(g)+2HCI(g)+2CI(g) Suppose that a chemist combines 257 mL of methane and 599 mL of chlorine at STP in a 2.00 L flask. The flask is then allowed to stand at 298 K. If the reaction reaches 87.2% completion, (a) What is the partial pressure of CH;CI? (b) What is the partial pressure of HCI? (c) What is the partial pressure of CI? (d) What is the partial pressure of Cl,? (e) What is the partial pressure of CH,? (f) What is the total pressure?

If 3.62 L of O2(g) is required to react completely with a 5.50 g sample of C(s) at 48°C, what was the pressure of the O2 gas?   2 C(s) + O2 (g) ----> 2 CO(g)

5.89.) A 150.0 mL flask contains 0.391 g of a volatile oxide $1.2 of sulfur. The pressure in the flask is 750 torr and the BH temperature is 22°C. Is the gas SO₂ or SO3? 2 5

When chromium metal is added to nitric acid, the following reaction takes place Cr (s) + 6 HNO₃ (aq) → Cr(NO₃)₃ (aq) + 3 H₂O (l) + 3 NO₂ (g) Calculate the volume of NO₂ gas collected over water at 40.0 °C when 28.3 g of chromium is added to excess nitric acid if the total pressure is 675 torr. The vapor pressure of water at 40.0 °C is 55.3 torr.