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nadezda [96]
2 years ago
10

How many grams of gas must be released from a 32.0 L sample of CO2(g) at STP to reduce the volume to 16.6 L at STP?

Chemistry
1 answer:
Hoochie [10]2 years ago
6 0

Answer:

30.3 g

Explanation:

At STP, 1 mol of any gas will occupy 22.4 L.

With the information above in mind, we <u>calculate how many moles are there in 32.0 L</u>:

  • 32.0 L ÷ 22.4 L/mol = 1.43 mol

Then we <u>calculate how many moles would there be in 16.6 L</u>:

  • 16.6 L ÷ 22.4 L/mol = 0.741 mol

The <u>difference in moles is</u>:

  • 1.43 mol - 0.741 mol = 0.689 mol

Finally we <u>convert 0.689 moles of CO₂ into grams</u>, using its <em>molar mass</em>:

  • 0.689 mol * 44 g/mol = 30.3 g
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2AgNO3 + CaCl2 → 2AgCl + Ca(NO3)2
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We have to find the amount of AgCl formed from 100 g of Silver nitrate by writing the expression.

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mihalych1998 [28]

Hey there!

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