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Vesnalui [34]
3 years ago
6

Determine the rate of a reaction that follows the rate law:

Chemistry
1 answer:
Natali5045456 [20]3 years ago
8 0
A. 0.12 (mol/L)/s

rate = 1 x 10-2 • 2^2 • 3
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Calculate the partial pressure of oxygen given the total barometric pressure of 515 mmHg. Round to the nearest hundredth.
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The partial pressure of oxygen given the total barometric pressure is : 108.15 mmHg

<u>Given data : </u>

Total barometric pressure = 515 mmHg

Assuming oxygen percentage = 21%

Barometric pressure dry at 37°C

<h3 /><h3>Determine the partial pressure of oxygen </h3>

Applying  the relation below

Partial pressure = oxygen percentage * Barometric pressure

                          = 21% * 515 mmHg

                          = 108.15 mmHg

Hence we can conclude that the partial pressure of oxygen is 108.15 mmHg.

Learn more about Partial pressure : brainly.com/question/1835226

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