Answer:
The correct answer is 10.939 mol ≅ 10.94 mol
Explanation:
According to Avogadro's gases law, the number of moles of an ideal gas (n) at constant pressure and temperature, is directly proportional to the volume (V).
For the initial gas (1), we have:
n₁= 1.59 mol
V₁= 641 mL= 0.641 L
For the final gas (2), we have:
V₂: 4.41 L
The relation between 1 and 2 is given by:
n₁/V₁ = n₂/V₂
We calculate n₂ as follows:
n₂= (n₁/V₁) x V₂ = (1.59 mol/0.641 L) x 4.41 L = 10.939 mol ≅ 10.94 mol
Answer: Oxygen.
Explanation: The -ate is used for the ion that has the largest number of Oxygen atoms. The -ite would be used for the ion with the smaller amount of oxygen atoms.
173.1f is the answer I believe, please let me know if I'm wrong then I would try to make up for it
The pressure of the gas is 1.0 bar.
<em>pV</em> = <em>nRT</em>
<em>T</em> = (0 + 273.15) K = 273.15 K
<em>p</em> = (<em>nRT</em>)/<em>V</em> = (2.0 mol × 0.083 14 bar·L·K⁻¹mol⁻¹ × 273.15 K)/44.8 L = 1.0 bar
Answer:
a. mixtures are created through physical changes and compounds are created through chemical reactions
Explanation: