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Andrei [34K]
3 years ago
13

A sample of nitrogen gas was collected via water displacement. Since the nitrogen was collected via water displacement, the samp

le is saturated with water vapor. If the total pressure of the mixture at 2121 °C is 1.721.72 atm, what is the partial pressure of nitrogen? The vapor pressure of water at 2121 °C is 18.718.7 mm Hg
Chemistry
1 answer:
vova2212 [387]3 years ago
8 0

Answer:

Explanation:

Total pressure = partial pressure of nitrogen + partial pressure of water vapour

partial pressure of water vapour = 18.7 mm of Hg

760 mm of Hg = 1 atm

18.7 mm of Hg = 18.7 / 760 atm

= .0246 atm

Total pressure = partial pressure of nitrogen + partial pressure of water vapour

Putting in the values in atm

1.72 atm = partial pressure of nitrogen + .0246 atm

partial pressure of nitrogen = 1.72 atm - .0246 atm

= 1.6954 atm

= 1.70 atm

partial pressure of nitrogen = 1.70 atm .

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True

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Given the following balanced equation, determine the rate of reaction with respect to [O2]. If the rate of formation of O2 is 7.
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Explanation:

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2O_3(g)\rightleftharpoons 3O_2(g)

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4 years ago
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oksano4ka [1.4K]

Answer:

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2. 125mg/min is the drip of the patient

Explanation:

1. In a body, an amount of Valium > 1.52mg / kg of body weight would be lethal.

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90.72kg × (1.52mg / kg) =

137.9mg ≡

<h3>0.138g of valium would be lethel in the woman</h3>

2. The IV contains 1.5g = 1500mg/mL.

If the patient is receiving 5.0mL/h, its rate in mg/h is:

5.0<u>mL</u>/h × (1500mg/<u>mL</u>) = 7500mg/h

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