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AysviL [449]
3 years ago
9

A gas has a volume of 240mL at 700mmHg pressure. What pressure is needed to reduce the volume to 80mL?

Chemistry
1 answer:
Dovator [93]3 years ago
5 0

Answer:

<h3>The answer is 2100 mmHg</h3>

Explanation:

The new pressure can be found by using the formula for Boyle's law which is

P_1V_1 = P_2V_2

Since we are finding the new pressure

P_2 =  \frac{P_1V_1}{V_2}  \\

From the question we have

P_2 =  \frac{240 \times 700}{80}  =  \frac{168000}{80}  =  \frac{16800}{8}  \\

We have the final answer as

<h3>2100 mmHg</h3>

Hope this helps you

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13.41g of Fe(NO3)2 is dissolved in 83.0mL of water. Calculate the molarity of the solution.
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Answer:

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Hydrogen gas, iodine vapor, hydrogen iodine are mixed in a flask and heated to 696°C. H2(g) + I2(g) ⇋ 2 HI(g) Kc = 52 at 696°C I
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Explanation:

The chemical reaction follows the equation:

                  H_2(g)+I_2(g)\rightleftharpoons 2HI(g)

At t = 0          0.044M     0.044M              0.177M  

At t=t_{eq}    (0.044-x)M    (0.044-x)M      (0.177+x)M

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We are given:

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The metabolic oxidation of glucose, C6H12O6, in our bodies produces CO2, which is expelled from our lungs as a gas.
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Answer:

\large \boxed{\text{21.6 L}}

Explanation:

We must do the conversions

mass of C₆H₁₂O₆ ⟶ moles of C₆H₁₂O₆ ⟶ moles of CO₂ ⟶ volume of CO₂

We will need a chemical equation with masses and molar masses, so, let's gather all the information in one place.

Mᵣ:        180.16

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m/g:      24.5

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\text{Moles of C$_{6}$H$_{12}$O}_{6} = \text{24.5 g C$_{6}$H$_{12}$O}_{6}\times \dfrac{\text{1 mol C$_{6}$H$_{12}$O}_{6}}{\text{180.16 g C$_{6}$H$_{12}$O}_{6}}\\\\= \text{0.1360 mol C$_{6}$H$_{12}$O}_{6}

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We can use the Ideal Gas Law.

pV = nRT

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T = (37 + 273.15) K= 310.15 K

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Answer:

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