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Stella [2.4K]
3 years ago
7

What would happen to a diver who does no exhale while surfacing from a 30 m dive?

Chemistry
1 answer:
sertanlavr [38]3 years ago
6 0
Their lungs would try to expand to about 4 timed the normal volume which would force air into the various body tissues. this can cause a lung expansion injury and it could case air embolism. Air embolism is when air bubbles get trapped in blood vessels. This can lead to a blockage which will could be fatal.
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Use the periodic table in the tools bar to answer these questions. How many moles of AgNO3 are present in 1.50 L of a 0.050 M so
IgorC [24]
M= moles de soluto / litros de solucion 
moles de soluto = M. litros de solucion 

Moles de soluto = 0.050 M x 1.50 L = 0.075 moles de AgNo3
4 0
3 years ago
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What is this element?<br> 1s22s22p63s2<br> Magnesium<br> Aluminum<br> Potassium<br> Neon
valkas [14]

Answer:

It should be silicon... I even googled it to see if I was correct and that’s what it says so can someone figure out why silicon is not an answer

Explanation:

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2 years ago
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The half-life of tritium, or hydrogen-3, is 12.32 years. After about 37 years, how much of a sample of tritium will remain uncha
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1/16 ( ignore this the stupid website just makes us use 20 characters UGH! )
7 0
3 years ago
HELP ASAP PLEASE!!!! 30 POINTS
valentina_108 [34]

Answer:

it's option c

Explanation:

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2.0L of hydrogen gas is mixed with 3.0L of nitrogen gas at STP in a rigid 5.0L vessel. A reaction occurs, producing ammonia gas
IrinaK [193]

Answer:

Moles NH₃: 0.0593

0.104 moles of N₂ remain

Final pressure: 0.163atm

Explanation:

The reaction of nitrogen with hydrogen to produce ammonia is:

N₂ + 3 H₂ → 2 NH₃

Using PV = nRT, moles of N₂ and H₂ are:

N₂: 1atmₓ3.0L / 0.082atmL/molKₓ273K = 0.134 moles of N₂

H₂: 1atmₓ2.0L / 0.082atmL/molKₓ273K = 0.089 moles of H₂

The complete reaction of N₂ requires:

0.134 moles of N₂ × (3 moles H₂ / 1 mole N₂) = <em>0.402 moles H₂</em>

That means limiting reactant is H₂. And moles of NH₃ produced are:

0.089 moles of H₂ × (2 moles NH₃ / 3 mole H₂) = <em>0.0593 moles NH₃</em>

Moles of N₂ remain are:

0.134 moles of N₂ - (0.089 moles of H₂ × (1 moles N₂ / 3 mole H₂)) = <em>0.104 moles of N₂</em>

And final pressure is:

P = nRT / V

P = (0.104mol + 0.0593mol)×0.082atmL/molK×273K / 5.0L

<em>P = 0.163atm</em>

7 0
3 years ago
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