If 5.505.50 L of water vapor at 50.2 °C50.2 °C and 0.1210.121 atm reacts with excess iron, how many grams of iron(III) oxide will be produced?   2Fe(s)+3H2O(g)⟶Fe2O3(s)+3H2(g)

5. A homeowner uses 4.00 x 10³ m³ of natural gas in a year to heat a home. Assume that natural gas is 100% methane, CH4, and that methane is behaving as a perfect gas, in this scenario. What is the mass of gas used? (Assume 1.00 atm pressure and 20°C)

The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine 1580 L of nitrogen gas and 4240 L of hydrogen gas at STP, heat the mixture to run the reaction, then separate the ammonia from the reaction mixture. What volume of reactant, measured at STP, is left over? Assume the reaction goes to completion. N₂ (g) + 3 H₂ (g) → 2 NH₃ (g)

Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. 2 Suppose the CO₂ gas evolved by a certain chemical reaction taking place at 40.0 °C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 51.0 mL. g x10 X 歐 Sketch of a gas-collection apparatus S collected gas Calculate the mass of CO₂ that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about 2 the reaction conditions and the nature of the gases. water chemical reaction

A sample of gas contains 0.1700 mol of CH4(g) and 0.1700 mol of H2O(g) and occupies a volume of 19.2 L. The following reaction takes place:CH4(g) + H2O(g)3H2(g) + CO(g)Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.

A 15.9 mL sample of liquid ethanol (C₂H5OH, density = 0.789 g/mL) was injected into a 10.0 L cylinder containing O₂ at a pressure of 4.50 atm and a temperature of 25 °C. The cylinder was heated to 125 °C and a spark was used to ignite the ethanol, which was completely combusted. What was the final total pressure in the cylinder (in atm) after the reaction, while it was still at 125 °C?

give the explanation of formula and calculations.

Nitesh

You set up a reaction with Gallium metal in excess hydrochloric acid at 28 degrees Celsius. It reacts in the following: 2Ga(s)+6HCl(aq)→2GaCl3(aq)+3H2(g) You collect 157 mLs and 0.951 atm of hydrogen over water. How many moles of Ga reacted? The partial pressure of water at 28 degrees is 0.0372 atm.