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nexus9112 [7]
3 years ago
7

Examples of nitrogens unreactivity

Chemistry
1 answer:
REY [17]3 years ago
8 0
WATCH OUT BUDDY:<span>reactivity....Spelling mistake.

ANSWER:
</span>For example<span>, "air" sometimes comes bubbling out of the ground near oil wells. Today ... For </span>example, nitric oxide combines with oxygen and water in the atmosphere to make nitric acid. When it ....Nitrogen's<span> role in the Oklahoma City bombing.</span>
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What is the vapor pressure of the solution if 35.0 g of water is dissolved in 100.0 g of ethyl alcohol at 25 ∘C? The vapor press
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<u>Answer:</u> The vapor pressure of the solution is 43.55 mmHg

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}      .....(1)

  • <u>For water:</u>

Given mass of water = 35.0 g

Molar mass of water = 18 g/mol

Putting values in equation 1, we get:

\text{Moles of water}=\frac{35.0g}{18g/mol}=1.944mol

  • <u>For ethyl alcohol:</u>

Given mass of ethyl alcohol = 100.0 g

Molar mass of ethyl alcohol = 46 g/mol

Putting values in equation 1, we get:

\text{Moles of ethyl alcohol}=\frac{100.0g}{46g/mol}=2.174mol

Total moles of solution = [1.944 = 2.174] moles = 4.118 moles

  • Mole fraction of a substance is given by:

\chi_A=\frac{n_A}{n_A+n_B}

<u>For water:</u>

\chi_{\text{water}}=\frac{n_{\text{water}}}{n_{\text{water}}+n_{\text{ethyl alcohol}}}

\chi_{water}=\frac{1.944}{4.118}=0.472

<u>For ethyl alcohol:</u>

\chi_{\text{ethyl alcohol}}=\frac{n_{\text{ethyl alcohol}}}{n_{\text{water}}+n_{\text{ethyl alcohol}}}

\chi_{\text{ethyl alcohol}}=\frac{2.174}{4.118}=0.528

Dalton's law of partial pressure states that the total pressure of the system is equal to the sum of partial pressure of each component present in it.

To calculate the vapor pressure of the solution, we use the law given by Dalton, which is:

P_T=\sum_{i=1}^n (p_i\times \chi_i)

Or,

P_T=[(p_{\text{water}}\times \chi_{\text{water}})+(p_{\text{ethyl alcohol}}\times \chi_{\text{ethyl alcohol}}

We are given:

Vapor pressure of water = 23.8 mmHg

Vapor pressure of ethyl alcohol = 61.2 mmHg

Putting values in above equation, we get:

p_T=[(23.8\times 0.472)+(61.2\times 0.528)]\\\\p_T=43.55mmHg

Hence, the vapor pressure of the solution is 43.55 mmHg

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