A sample of gas contains 0.1600 mol ofHBr(g) and 0.08000 mol ofCl₂ (g) and occupies a volume of 10.4 L. The following reaction takes place:2HBr(g) + Cl₂(g) → 2HCl(g) + Br₂ (g)Calculate the volume of the sample after the reaction takes place, assuming that thetemperature and the pressure remain constant.Volume =L

As per Dalton's law, volume and number of moles are directly proportional to each other.

A sample of gas contains 0.1600 mol of HBr(g) and 0.08000 mol of Cl₂ (g) and occupies a volume of 10.4 L. The following reaction takes place: 2HBr(g) + Cl₂(g) → 2HCl(g) + Br₂ (9) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. Volume = L

A sample of gas contains 0.1600 mol of HBr(g) and 0.08000 mol of Cl₂ (g) and occupies a volume of 10.4 L. The following reaction takes place: 2HBr(g) + Cl₂(g) → 2HCl(g) + Br₂ (9) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. Volume = L

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

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
0.17 moles of hydrogen gas and 0.33 moles of nitrogen gas are created from thereaction 2NH3 (g) → 3H2 (g) + N2 (g). The final total pressure in the reaction vessel is0.75 atm. Calculate the partial pressure of the hydrogen gas at the end of the reaction.Assume the number of moles of NH3 (g), left after the reaction occurs, is negligible.
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.
An ideal gas in a sealed container has an initial volume of 2.65 L.2.65 L. At constant pressure, it is cooled to 17.00 ∘C,17.00⁢ ∘C, where its final volume is 1.75 L.1.75 L. What was the initial temperature?
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
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.
give the explanation of formula and calculations.
A sample of gas contains 0.150 mol of N₂(g) and 0.300 mol of H₂(g) and occupies a volume of 21.4 L. The following reaction takes place: N₂(g) + 2H₂(g)-N₂H4(9) Calculate the volume of the sample after the reaction takes place (assume temperature and pressure are constant).
A sample of Oz with a pressure of 1.42 atm and a volume of 280 mL is allowed to react with excess CO at 107 °C. 2 CO (g) + 0, (g) 2 CO, (g) Calculate the pressure of the CO, produced in the reaction if it is transferred to a 2.00-L flask and cooled to 33 °C. atm
A reaction between liquid reactants takes place at −5.0 °C in a sealed, evacuated vessel with a measured volume of 50.0 L. Measurements show that the reaction produced 8.0 g of boron trifluoride gas. Calculate the pressure of boron trifluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Round your answer to 2 significant digits. pressure: atm x10 X Ś
7a
(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