Oxygen is a product of the decomposition of mercury(II) oxide as shown below. 2 Hg0(s) → 2 Hg(8) + O2(g) You have determined that 0.006926 moles of O2(g) were produced in this reaction. What volume in L of O2 will be produced from the decomposition of 3.0 g of HgO assuming a pressure of 1.5 atm and a temperature of 122°C? Remember the gas constant, R, is 0.08206 L·atm/mol·K.
Oxygen is a product of the decomposition of mercury(II) oxide as shown below. 2 Hg0(s) → 2 Hg(8) + O2(g) You have determined that 0.006926 moles of O2(g) were produced in this reaction. What volume in L of O2 will be produced from the decomposition of 3.0 g of HgO assuming a pressure of 1.5 atm and a temperature of 122°C? Remember the gas constant, R, is 0.08206 L·atm/mol·K.
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter19: The Representative Elements
Section: Chapter Questions
Problem 92CWP
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