If 4.67 g of Ag2O is sealed in a 75.0-mL tube filled with 760torr of N2 gas at 28 °C, and the tube is heated to 310 °C,the Ag2O decomposes to form oxygen and silver.Part AWhat is the total pressure inside the tube assuming the volume of the tube remains constant?Express your answer to three significant figures and include the appropriate units.HAPtotValueSubmitRequest AnswerProvide Feedback?Units

Step 1:Given,Mass of Ag2O = 4.67gVolume of tube = 75.0 mL = 0.075 LInitial pressure of N2 gas = 760…

Answered: If 4.67 g of Ag2O is sealed in a…

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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CHEMWORK A sample of 52.0 g of neon gas is placed in a balloon with a volume of 10.3 L at 25.0 °C. If 28.9 g of neon is then added to the balloon at constant temperature and pressure, what would be the new volume of this balloon? Volume = L ogress Submit Show Hints Submit Answer Retry Entire Group 8 more group attempts remaining Previous Next Save
Constants | Periodic Table A gas of unknown molecular mass was allowed to effuse through a small opening under constant-pressure conditions. It required 105 s for 1.0 L of the gas to effuse. Under identical experimental conditions it required 29 s for 1.0 L of O2 gas to effuse. ▾ Part A Calculate the molar mass of the unknown gas. (Remember that the faster the rate of effusion, the shorter the time required for effusion of 1.0 L; that is, rate and time are inversely proportional.) Express your answer in grams per mol to two significant figures. M = Ο ΑΣΦ Submit Request Answer 3+ < Return to Assignment Provide Feedback a % ? g/mol MacBook Pro 曲 C
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The volume of fluorine gas required to react with 5.34 g of calcium bromide to form calcium fluoride and bromine at 45.0 °C and 2.20 atm is ________ mL.
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When chromium metal is added to nitric acid, the following reaction takes place Cr (s) + 6 HNO₃ (aq) → Cr(NO₃)₃ (aq) + 3 H₂O (l) + 3 NO₂ (g) Calculate the volume of NO₂ gas collected over water at 40.0 °C when 49.3 g of chromium is added to excess nitric acid if the total pressure is 675 torr. The vapor pressure of water at 40.0 °C is 55.3 torr.
A reaction between liquid reactants takes place at 34.0 °C in a sealed, evacuated vessel with a measured volume of 25.0 L. Measurements show that the reaction produced 11. g of carbon dioxide gas. Calculate the pressure of carbon dioxide 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 Continue Submit Assignment 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility MacBook Air 80 888 F1 F2 DD F3 F4 F5 F6 F7 F8 F9 F10 11 & 2 6 7 8 8 L5 00 S14 73
The mass of an evacuated 255 mL flask is 143.197 g The mass of the flask filled with 272 torr of an unknown gas at 35 °C is 144.277 g . Part A Calculate the molar mass of the unknown gas. Express your answer to three significant figures. > g/mol Molar mass = Submit Request Answer Provide Feedback
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When chromium metal is added to nitric acid, the following reaction takes place Cr (s) + 6 HNO₃ (aq) → Cr(NO₃)₃ (aq) + 3 H₂O (l) + 3 NO₂ (g) Calculate the volume of NO₂ gas collected over water at 40.0 °C when 28.3 g of chromium is added to excess nitric acid if the total pressure is 675 torr. The vapor pressure of water at 40.0 °C is 55.3 torr.

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