The approximate partial pressure of oxygen at 1500 m is 0.18 atm.
<h3>Pressure of the air</h3>
From barometric pressure table;
1500 m = 85 kPa
1 kPa = 0.0099 atm
85 kPa = ?
= 0.84 atm
Oxygen percentage in air = 21%
<h3>Partial pressure of oxygen in air</h3>
P = 0.21 x P(total)
P = 0.21 x 0.84 atm
P = 0.18 atm
Thus, the approximate partial pressure of oxygen at 1500 m is 0.18 atm.
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Answer:
165 g of NaCl are formed in the reaction
Explanation:
2Na + Cl₂ → NaCl
In order to determine the limiting reactant, we convert the mass of each reactant to moles
35 g / 23g/mol = 1.52 moles Na
100 g / 70.9 g/mol = 1.41 moles Cl₂
1 mol of chlorine reacts with 2 moles of Na, so If I have an x value of moles of Cl₂ I would need the double to react.
For 1.41 moles of Cl₂, I need 2.82 moles of Na; therefore my limiting reagent is the Na. Ratio is 2:2. So if I have 2.82 moles of Na I will produce 2.82 moles of NaCl
We convert the moles to mass: 2.82 mol . 58.45 g/1 mol =164.8 g
Answer:
It falls in Liquid and Solid.
Explanation:
Answer: gas particles that are in constant motion and exhibit perfectly elastic collisions
Explanation: