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Alex73 [517]
3 years ago
10

Why do astronauts have to wear pressurized suits in space? Need to know for homework!

Chemistry
1 answer:
Leno4ka [110]3 years ago
6 0
Astronauts<span> must </span>wear<span> spacesuits whenever they leave a spacecraft and are exposed to the environment of </span>space<span>. In </span>space, there is no air to breath and no air pressure.Space<span> is extremely cold and filled with dangerous radiation. Without protection, an</span>astronaut<span> would quickly die in </span>space<span>.</span>
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katen-ka-za [31]
First, find out how many years are in a decade. There 10 years per decade. So in 5 decades, that makes 50 years. Then multiply 50×12 because there are 12 months in a year. So there are 600 months in 5 decades.
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3 years ago
The compound fes is an example of a(n) element ionic compound covalent compound atom
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3 years ago
A buffer solution contains 0.240 M ammonium chloride and 0.499 M ammonia. If 0.0565 moles of perchloric acid are added to 250 mL
snow_lady [41]

Answer:

The pH of the resulting solution is 9.02.

Explanation:

The initial pH of the buffer solution can be found using the Henderson-Hasselbalch equation:

pOH = pKb + log(\frac{[NH_{4}Cl]}{[NH_{3}]})  

pOH = -log(1.78\cdot 10^{-5}) + log(\frac{0.240}{0.499}) = 4.43        

pH = 14 - pOH = 14 - 4.43 = 9.57

Now, the perchloric acid added will react with ammonia:

n_{NH_{3}} = 0.499moles/L*0.250 L - 0.0565 moles = 0.0683 moles

Also, the moles of ammonium chloride will increase in the same quantity according to the following reaction:

NH₃ + H₃O⁺ ⇄ NH₄⁺ + H₂O    

n_{NH_{4}Cl} = 0.240 moles/L*0.250L + 0.0565 moles = 0.1165 moles

Finally, we can calculate the pH of the resulting solution:

pOH = pKb + log(\frac{[NH_{4}Cl]}{[NH_{3}]})  

pOH = -log(1.78\cdot 10^{-5}) + log(\frac{0.1165 moles/0.250 L}{0.0683 moles/0.250 L}) = 4.98  

pH = 14 - 4.98 = 9.02

Therefore, the pH of the resulting solution is 9.02.

I hope it helps you!

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