Answer:
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Explanation:
Answer:
Partial pressure SO₂ → 0.440 atm
Explanation:
We apply the mole fraction concept to solve this:
Moles of gas / Total moles = Partial pressure of the gas / Total pressure
Total moles = 0.3 moles of CO₂ + 0.2706 moles of SO₂ + 0.35 moles H₂O
Total moles = 0.9206 moles
Mole fraction SO₂ = 0.2706 moles / 0.9206 moles → 0.29
Now, we can know the partial pressure:
0.29 = Partial pressure SO₂ / Total pressure
0.29 = Partial pressure SO₂ / 1.5 atm
0.29 . 1.5atm = Partial pressure SO₂ → 0.440 atm
Answer:
2365.0 g
Explanation:
First we <u>convert 1.2 x 10²⁵ particles into moles</u>, using <em>Avogadro's number</em>:
- 1.2 x 10²⁵ particles ÷ 6.023x10²³ particles/mol = 19.9 mol
Then we <u>convert 19.9 moles of NiCO₃ into grams</u>, using the <em>molar mass of NiCO₃</em>:
- NiCO₃ Molar Mass = 118.702 g/mol
- 19.9 mol * 118.702 g/mol = 2365.0 g
What are your examples to work off?
