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spin [16.1K]
3 years ago
6

What is the partial pressure of water vapor in an air sample when the total pressure is 1.00 atm, the partial pressure of nitrog

en is 0.79 atm, the partial pressure of oxygen is 0.19 atm, and the partial pressure of all other gases in air is 0.0044 atm?
Chemistry
1 answer:
Inga [223]3 years ago
7 0

Answer:

0.0156 atm

Explanation:

Let the partial pressure of water vapor be P_w.

Given:

Total pressure of air sample is, P_T=1.00\ atm

Partial pressure of nitrogen is, P_n=0.79\ atm

Partial pressure of oxygen is, P_o=0.19\ atm

Partial pressure of all other gases is, P_{other}=0.0044\ atm

From Dalton's law of partial pressure, we know that, the total pressure of a mixture of gases is equal to sum of partial pressure of each individual gas.

So, total pressure of air sample is equal to the sum of partial pressure of nitrogen, oxygen, other gases and water vapor.

Therefore, framing in equation form, we have:

P_n+P_o+P_{other}+P_w=P_T

Plug in the given values and solve for P_w. This gives,

0.79+0.19+0.0044+P_w=1.00\\\\0.9844+P_w=1.00\\\\P_w=1.00-0.9844\\\\P_w=0.0156\ atm

Therefore, the partial pressure of water vapor in an air sample is 0.0156 atm.

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netineya [11]

The unbalanced equation is one in which the moles of atoms are not equal on both sides of the reaction.

<h3>What is a balanced chemical equation?</h3>

A balanced chemical equation is one in wgich the moles of atoms in the reactants side is equal to the moles of atoms on the product side.

The given equations of reaction is not clearly stated.

Therefore, the unbalanced equation is one in which the moles of atoms are not equal on both sides of the reaction.

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Hydrogen boils at 20k. what is the boiling point of hydrogen on the celsius scale
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Celsius scale is related to kelvin scale by the following equation,

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So as here temperature is given in kelvin, so it can be converted into celsius as follows:

So 20 K = 20K-273 °C  

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Answer: See description

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3 years ago
Problem PageQuestion Aqueous sulfuric acid will react with solid sodium hydroxide to produce aqueous sodium sulfate and liquid w
quester [9]

Answer:

0.72g

Explanation:

Step 1:

We'll begin by writing a balanced equation for the reaction. This is illustrated below:

H2SO4 + 2NaOH —> Na2SO4 + 2H2O

Step 2:

Determination of the mass of sulphuric acid (H2SO4) and the mass of sodium hydroxide (NaOH) that reacted from the balanced equation. This is illustrated below:

Molar Mass of H2SO4 = (2x1) + 32 +(16x4) = 2 + 32 + 64 = 98g/mol

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Mass of NaOH from the balanced equation = 2 x 40 = 80g

Step 3

Determination of the limiting reactant. To do this, we need to know which of the reactant is excess.

Now let us consider using all of the mass of NaOH given to see if there will be left over for H2SO4. This is illustrated below:

From the balanced equation above,

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Therefore, Xg of H2SO4 will require 1.6g of NaOH i.e

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Now comparing the mass of H2SO4 that reacted ( i.e 1.96g) and the mass of H2SO4 given ( i.e 2.94g), we can see clearly that there are left over ( i.e 2.94 - 1.96 = 0.98g) of H2SO4. Therefore, H2SO4 is the excess reactant and NaOH is the limiting reactant.

Step 4:

Determination of the mass of water produced from the reaction. This is illustrated below:

The balanced equation for the reaction is given below:

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Therefore, the maximum mass of water (H2O) produced by the chemical reaction of aqueous sulfuric acid with solid sodium hydroxide is 0.72g

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