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cestrela7 [59]
3 years ago
5

A sample of nitrogen gas is collected over water at a temperature of 23.0 C. What is the pressure of the nitrogen gas if atmosph

eric pressure is 785 mm Hg
Chemistry
1 answer:
Whitepunk [10]3 years ago
4 0
We first consider the gases that will be present in that sample.
First, there will be nitrogen, as stated. Second, there will also be water in the form of water vapor. For this, we need the vapor pressure of water at 23.0 °C, which is about 21.0 mmHg. Now, the sum of the vapor pressures of the gases will be equivalent to the total pressure. So the pressure of nitrogen gas is:
785 - 21
= 764 mmHg
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<h3>What is Density ?</h3>

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<h3>What is Intensive Property ? </h3>

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Disclaimer: The given question is incomplete on the portal. Here is the complete question.

Question: The density (d) of a substance is an intensive property that is defined as the ratio of its mass (m) to its volume (v)

density = \frac{\text{Mass}}{\text{Volume}}  or d = \frac{m}{V}

Considering that mass and volume are both extensive properties, explain why their ratio, density is intensive.

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2 years ago
Calculate the molality of a solution prepared by dissolving 175 g of KNO3 in 750 g of water. (round to nearest hundreth)
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