Liquid nitrogen trichloride is heated in a 1.75-L closed reaction vessel until it decomposes completely to gaseous elements. The resulting mixture exerts apressure of 769. mmHg at 88.0 °C. What is the partial pressure of each gas in the container? (1 mmHg 1 torr.) Round each of your answers to 3 significantfigures.=Part 1 of 2Pressure of N2:Part 2 of 2torr☐ x10☑Pressure of Cl₂:torr☐ x10☑

Pressure of N2: 192 torr Pressure of Cl2: 577 torrExplanation:

Answered: Liquid nitrogen trichloride is heated…

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...

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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
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a. A 3.00-LL flask is filled with gaseous ammonia, NH3NH3. The gas pressure measured at 23.0 ∘C is 2.45 atm . Assuming ideal gas behavior, how many grams of ammonia are in the flask? b. If 1.00 mol of argon is placed in a 0.500-L container at 23.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.345(L2⋅atm)/mol2a=1.345(L2⋅atm)/mol2 and b=0.03219L/molb=0.03219L/mol. Express your answer to two significant figures and include the appropriate units.
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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
Liquid nitrogen trichloride is heated in a 3.00-L closed reaction vessel until it decomposes completely to gaseous elements. The resulting mixture exerts a pressure of 858 mmH at 94°C. What is the mass of the original sample?
#14
Calculate the final pressure of the gas. Round your answer to 3 significant digits.
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
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