Consider the reaction below P4(g) + 6 Cl2(g) → 4 PCl3(g) If 0.766 moles of P4 is mixed with 1.86 moles of Cl2 in a 1.39-L rigid reaction vessel, what is the final pressure in the vessel after the reaction goes to completion? The final temperature is 486. °C. Assume 100% yield.

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)

A mass of 7.16 g carbon monoxide is reacted with 6.84 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? mmHg mmHg CO H₂ CH3OH Total Submit Submit Answer mmHg mmHg Show Approach Show Tutor Steps Try Another Version 2 item attempts remaining

The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine 1583 L of nitrogen gas and 4571 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 in liters? Assume the reaction goes to completion. N₂ (g) + 3 H₂ (g) → 2 NH₃ (g)

SF6 can be synthesized by the reaction:                                SO2(g) + 3 F2(g) → SF6(g) + O2(g)A 1.25-L reaction vessel, initially at 26°C, contains sulfur dioxide gas at a partial pressure of 184 mmHg and fluorine gas at a partial pressure of 511 mmHg. Identify the limiting reactant and determine the theoretical yield of SF6 in grams.

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).

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 =

Gaseous ammonia is synthesized from nitrogen and hydrogen by the reaction N2(g) + 3H2(g)→ 2NH3(g) Assume you take 355 L of H2 gas at 25.0 °C and 542 mm Hg and combine it with excess N2 gas. a )What is the theoretical yield of NH3 gas? b) If this amount of NH3 gas occupies a 125-L tank at 25.0 °C, what is its pressure?

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