9 ÷ 45 = 0,2 g/ml
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A mixture of 3.05-atm N₂(g) and 5.29-atm He(g) exerts a total pressure of 8.34 atm.
<h3>What does Dalton's law of partial pressure state?</h3>
Dalton's law states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases.
A mixture of N₂(g) and He(g) exerts a total pressure of 8.34 atm, while the partial pressure of N₂ is 3.05 atm.
We will use Dalton's law to calculate the partial pressure of He.
P = pHe + pN₂
pHe = P - pHe = 8.34 atm - 3.05 atm = 5.29 atm
where,
- P is the total pressure.
- pHe is the partial pressure of He.
- pN₂ is the partial pressure of N₂.
A mixture of 3.05-atm N₂(g) and 5.29-atm He(g) exerts a total pressure of 8.34 atm.
Learn more about Dalton's law here: brainly.com/question/14119417
The answer is 0.0171468704904. We assume you are converting between moles Mg(OH)2 and gram. This compound is also known as Magnesium Hydroxide. 1 mole<span> is equal to </span>1 moles<span> Mg(OH)2, or 58.31968 grams.</span>
Answ burh i dont even know
Explanation: i dont even know this
Answer:
When for example, heating up an ice cube the particles of the ice start to vibrate fast enough to get separated into liquid caused from high temperature. So the answer is Higher.