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nikklg [1K]
3 years ago
15

If a sample of gas is at 672 °C and 3.9 atm, what is the new temperature at 12.2 atm?

Chemistry
1 answer:
Snowcat [4.5K]3 years ago
7 0
In order to calculate the final temperature of the gas, we may apply Charles's law, which states that the pressure and temperature of a fixed amount of gas at constant volume are directly proportional. Mathematically:
P/T = constant
(absolute temperature is used, so T = 672 + 273 = 945 K)
Thus,
3.9 / 945 = 12.2 / T
T = 2,956 K or 2,683 °C
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Answer

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Answer:

The molar mass of copper (II) nitrate is 187.5 g/mol.

Explanation:

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Suppose a student started with 142.0 mg of trans-cinnamic acid, 412 mg of pyridinium tribromide, and 2.30 mL of glacial acetic a
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Answer: Theoretical Yield = 0.2952 g

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Explanation:

Calculation of limiting reactant:

n-trans-cinnamic acid moles = (142mg/1000) / 148.16 = 9.584*10⁻⁴ mol

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The molar ratio according to the equation mentioned is equals to 1:1

The brominated product moles is also = 9.584*10⁻⁴ mol

Theoretical yield = (9.584*10⁻⁴ mol) * (Mr of brominated product)

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Percentage Yield is : Actual Yield / Theoretical Yield = 0.2223/0.2952

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3 years ago
This was in my chemistry class- <br> What's the color combination code?
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3 years ago
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Explanation:

Hope that made sense!

8 0
3 years ago
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