Ethylene oxide is produced from the reaction of ethylene and oxygen at 270-290°C and 8-20 atm. In order to prevent potentially dangerous pressure buildups, the container in which this reaction takes place has a safety valve set to release gas when the pressure reaches 25 atm. If a 75-m3 reaction vessel contains 3.5 ✕ 104 moles of gas, at what temperature will the pressure reach 25 atm? (There are 103 L per m3.)

A reaction between liquid reactants takes place at 29.0 °C in a sealed, evacuated vessel with a measured volume of 5.0 L. Measurements show that the reaction produced 49. g of sulfur hexafluoride gas. Calculate the pressure of sulfur hexafluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Be sure your answer has the correct number of significant digits. pressure: atm ?

Pls help ASAP.

A mass of 8.92 g carbon monoxide is reacted with 7.18 g hydrogen to form methanol.   CO(g) + 2 H2(g) → CH3OH(g) The reaction is performed in a 5.00 L flask at 85.0 °C and proceeds to completion. What is the partial pressure (in mmHg) of each of the three species following completion of the reaction? What is the total pressure in the flask?   CO: ___  mmHg H2 : ____ mmHg CH3OH : ____ mmHg Total: ____  mmHg

A 2.20 L container at 53.6 °C contains 6.21g N2⁢O3⁡(g). The N2⁢O3 gas decomposes completely, producing NO2⁢(g) and NO(g). Assuming the container volume and the temperature do not change, calculate the pressure of the gas mixture after the complete decomposition of N2O3.

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

Some N, gas is mixed with some O, gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 1100. torr. key carbon hydrogen dlo nitrogen sulfur oxygen chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 4 significant digits. You may assume each gas behaves as an ideal gas. gas mole fraction partial pressure N2 torr O2 torr

A sample of gas contains 0.1100 mol of CH4 (9) and 0.1100 mol of H₂O(g) and occupies a volume of 13.1 L. The following reaction takes place: CH4 (9) + 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. Volume =

(Incorrect) Consider the reaction below P4(g) + 6 Cl₂(g) → 4 PC13(g) If 0.246 moles of P4 is mixed with 0.354 moles of Cl₂ in a 9.77-L rigid reaction vessel, what is the final pressure in the vessel after the reaction goes to completion? The final temperature is 350. °C. Assume 100% yield. 2.89 atm 1.24 atm (Your answer) 0.694 atm 2.21 atm (Correct answer) 5.15 atm