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saw5 [17]
3 years ago
9

sample of carbon monoxide gas occupies 3.20 L at 125 °C. At what temperature will the gas occupy a volume of 1.54 L if the press

ure remains constant?
Chemistry
2 answers:
Anna [14]3 years ago
3 0

Answer:

-81.5 degrees C or 191.5 K

Explanation:

We want to use Charles' gas law: V/T = V/T

Our initial volume is 3.20 L, and our initial temperature is 125 degrees C, or 125 + 273 = 398 degrees Kelvin.

Our new Volume is 1.54 L, but we don't know what the temperature is. So, we use the equation:

3.20 L / 398 K = 1.54 L / T ⇒ Solving for T, we get: T = 191.5 K

If we want this in degrees Celsius, we subtract 273: 191.5 - 273 = -81.5 degrees C

Sophie [7]3 years ago
3 0

Answer:

- 81.5°C

Explanation:

Data obtained from the question include:

V1 (initial volume) = 3.20 L

T1 (initial temperature) = 125 °C = 125 + 273 = 398K

V2 (final volume) = 1.54 L

T2 (final temperature) =.?

At constant pressure indicates that the gas is obeying Charles' law. Using the Charles' law equation V1/T1 = V2/T2 , the final temperature of the gas can be obtained as illustrated below:

V1/T1 = V2/T2

3.2/398 = 1.54/T2

Cross multiply to express in linear form

3.2 x T2 = 398 x 1.54

Divide both side by 3.2

T2 = (398 x 1.54)/ 3.2

T2 = 191.5K

Now let us convert 191.5K to celsius temperature. This is illustrated below

°C = K - 273

°C = 191.5 - 273

°C = - 81.5°C

Therefore the gas will occupy 1.54L at a temperature of - 81.5°C

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You have a 1.153 g sample of an unknown solid acid, HA, dissolved in enough water to make 20.00 mL of solution. HA reacts with K
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Answer:

HA +  KOH  →  KA  +  H₂O

Explanation:

The unknown solid acid in water can release its proton as this:

HA  +  H₂O  →  H₃O⁺  +  A⁻

As we have the anion A⁻, when it bonded to the cation K⁺, salt can be generated, so the reaction of HA and KOH must be a neutralization one, where you form water and a salt

HA +  KOH  →  KA  +  H₂O

It is a neutralization reaction because H⁺ from the acid and OH⁻ from the base can be neutralized as water

7 0
3 years ago
What are the hydronium and hydroxide ion concentrations in a solution whose ph is 6.52?
erica [24]

A solution with a pH of 6.52 has a hydronium ion concentration of 3.02x10-7 mol/L and a hydroxide ion concentration of 3.31x10-8 mol/L.

The hydronium ion concentration of a solution can be calculated from pH by using 10^{-pH}. For a pH of 6.52, hydronium ion concentration is 3.02x10-7 mol/L.

The concentration of hydroxide ions can be determined by identifying the value of pOH. The sum of pOH and pH is equal to 14, which is based on the negative logarithm of the ion-product constant of water. At a pH of 6.52, pOH is equal to 7.48.

The relationship between pOH and hydroxide ion concentration is the same as the relationship between pH and hydronium ion concentration. With this, the hydroxide ion concentration at pOH of 7.48 is 10^{-7.48} or 3.31x10-8 mol/L.

For more information regarding pH and pOH,  please refer to the link brainly.com/question/13557815.

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3 0
1 year ago
Write the molecular formula for the compound that exhibits a molecular ion at M+ = 112.0499. Assume that C, H, N, and O might be
navik [9.2K]

Answer:

C₆H₁₀NO

Explanation:

In order to arrive at a molecular formula we have to make some assumptions and they are

Assuming there is one ( 1 ) N and one ( 1 ) O that is present in the said molecule

Total mass =   29.998

next step: subtract the total mass from 112.0499 = 82.501

next : assume the presence of 6 carbon atoms in said molecule

Total mass =  6 * 12 = 72

Mass of Hydrogens = 82.501 - 72 = 10.501

∴ number of hydrogens = 10.501 / 1.0078  ≈ 10

Hence Total mass = 29.998 + 82.501  ≈ 112.0499

Finally Molecular formula = C₆H₁₀NO

3 0
3 years ago
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