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Anni [7]
3 years ago
10

45.6 grams of CH4 is placed into a 275 mL container at 55.00C. What is the pressure inside the container in atm?

Chemistry
1 answer:
xxTIMURxx [149]3 years ago
4 0

<em>Given-</em>

<em>Mass of CH4 - 45.6 grams</em>

<em>Molar mass of CH4 - 16.04 g/mol</em>

<em>volume - 275mL</em>

<em>Temperature- 55°C</em>

<em>Solution,</em>

<em>moles of methane (CH4) n =</em><em> </em><em>45.6/16.04 </em>

<em>= 2.84 moles</em>

<em>Using Formula,</em>

<em>Pv = nRT</em>

<em>P*275 = 2.84*8.314*55</em>

<em>P</em><em> = 1298.64/275</em>

<em>P </em><em>= 4.72 Atm.</em>

<em>Answer - The pressure inside the container in atm is 4.72.</em>

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Explanation:

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Therefore, 7.81×10¯³ mole of O2 occupy 175mL.

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From the balanced equation above,

2 moles of H2O2 decomposed to produce 1 mole of O2.

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Xmol of H2O2 = 2 x 7.81×10¯³

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3 years ago
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Explanation :

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