Answer:
23 kPa = Partial pressure O₂
Explanation:
In a mixture of gases, the sum of partial pressure of each gas that contains the mixture = Total pressure
Total pressure = Partial pressure N₂ + Partial pressure CO₂ + Partial pressure O₂
95 kPa = 48 kPa + 24 kPa + Partial pressure O₂
95 kPa - 48 kPa - 24 kPa = Partial pressure O₂
23 kPa = Partial pressure O₂
Answer:
I believe the correct answer is a mixture. Most rocks are just different compounds or elements somewhat fused through heat and pressure. The substances are not chemically bonded together which means that they all retain their chemical identity and therefore can be separated by breaking them up. A good example of this is granite where you can see the different compounds that got fused together and can falls apart when you grind it. I hope this helps. Let me know if anything is unclear.
Explanation:
HOPE THIS HELPS :)
Answer:
300 gr.
Explanation:
if 204gr/100gr=solubility, then according to the condition solubility=612/x.
It means, 204/100=612/x, where x=612*100/204=300 gr.
I think the answer will be homogeneous mixture
<span>Missing question: The first-order rate
constant for the decomposition of N2O5, 2N2O5(g)→4NO2(g) + O2(g) at 70°</span><span>C is 6.82×10−3 s−1. Suppose we start with 2.70×10−2 mol of
N2O5(g) in a volume of 1.8 L .
</span>c₀(N₂O₅) = 0,027 mol ÷ 1,8 L.<span>
c</span>₀(N₂O₅) =
0,015 mol/L.<span>
c(N</span>₂O₅) = 0,019 mol/ 1,8 L = 0,01055 mol/L.<span>
k = 6,82·10</span>⁻³ s⁻¹.<span>
ln c(N</span>₂O₅) =
ln c₀(N₂O₅) -
k·t.<span>
t = (ln c</span>₀(N₂O₅) - ln c(N₂O₅)) ÷ k.<span>
t = 0,35 ÷ 0,00682 s</span>⁻¹.<span>
t = 51 s = 0,86 min.</span>
