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Simora [160]
3 years ago
7

A 30.0 L container was filled by pumping into it 10.0 L of CO2 gas at 60.0 torr of pressure and 20.0 L of O2 gas at 50.0 torr of

pressure. All volumes and pressures were measured at the same temperature. What is the final pressure of CO2 in this mixture?
Chemistry
1 answer:
NeX [460]3 years ago
7 0

The final volume of the Oxygen O2 would simply be equivalent to the overall volume of the final mixture. This is because gases would occupy every space of its container. So in this case, the volume of CO2 and O2 would be the same and it would be 30 L. What would be different is the partial pressures of each.

Answer:

 30 L

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What is the pH of a 900 mL solution containing 3.40 grams of hydrocyanic acid
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Answer:

pH = 5.05

Explanation:

pH is derived from the concentration of hydronium ions in a solution. Hydrocyanic acid is HCN.

First, we shall figure out the moles of HCN:

\frac{3.4g}{27.03g/mol}  = 0.125786

If HCN was a strong acid:

HCN has a 1:1 ratio of H+ ions, the moles of H+ is also the same.

To find the molarity, we now divide by Liters. This gets us:

\frac{0.125786 moles}{0.9L} = 0.139762 M

Finally, we plug it into the definition of pH:

pH = -log[H^{+} ]

pH = -log(0.139762)

pH = 0.855

However, since HCN is a weak acid, it only partially dissociates. The K_a of HCN is 6.2 * 10^{-10}.

K_a = \frac{[H^+][A^-]}{[HA]}

We can use an ice table to determine that when x = H+,

K_a = \frac{x^2}{0.125786-x}

[H^+] = 8.83*10^{-6}

pH = -log[H^{+} ]

pH = -log(8.83 * 10^{-6} )

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Answer: 76.017 moles

Explanation:

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Learn more:

Nuclear decay brainly.com/question/4207569

#learnwithBrainly

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3 years ago
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