When mercury(II) oxide is heated it decomposes to make liquid mercury and release oxygen. What is the pressure of O2 generated in a 10 liter container at 1000K when 2 moles of HgO decomposes?
2HgO (s) ⟶ 2Hg (l) + O2 (g)
Group of answer choices
about 4 atm
about 1 atm
about 16 atm
about 8 atm
Answers
Answer:
The answer will be about 4 atm.
Answer:
The pressure of O2 generated in the 10-liter container at 1000 K when 2 moles of HgO decomposes is about 8 atm.
Explanation:
The balanced chemical equation for the decomposition of mercury(II) oxide is:
2HgO (s) ⟶ 2Hg (l) + O2 (g)
We are given that 2 moles of HgO decompose. According to the balanced equation, this will produce 1 mole of O2 gas.
Using the Ideal Gas Law, we can calculate the pressure of the O2 gas generated in the 10-liter container at 1000 K. The Ideal Gas Law is given by:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
We can rearrange this equation to solve for P:
P = nRT/V
Substituting the values we know:
n = 1 mole
R = 0.0821 L·atm/K·mol (the gas constant)
V = 10 L
T = 1000 K
P = (1 mol)(0.0821 L·atm/K·mol)(1000 K)/(10 L)
P = 8.21 atm
Therefore, the pressure of O2 generated in the 10-liter container at 1000 K when 2 moles of HgO decomposes is about 8 atm.
Answer: about 8 atm.
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