Answer:
342
g/mol
Explanation:
Just get out that Periodic Table of the Elements, find the atomic masses for each atom, and add them up!
Credit to "SCooke" (User)
G We've all blown up balloons. When you blow into a balloon, you are putting in more moles of gas. Let's say that on the second exhalation (blow) you blow in the exact same number of moles as you did with the first exhalation. So, you doubled the number of moles in the balloon. If the temperature and pressure remained constant, what is true about the volume of the gas in the balloon
Answer:
- <em>The conditions under which a real gas is most likely to behave ideally is at low pressure and hight temperatures.</em>
Explanation:
According to molecular kinetic theory, 1) gas particles (molecules or atoms) occupy a negligible fraction of the total volume of the gas, and 2) the force of attraction between gas molecules is zero.
Those two assumptions constitute the basis for the behavior of a gas and an ideal gas.
The lower the pressure and the higher the temperature the closer those assumptions are valid for real gases.
At low pressure, the particles of the gas will be more separated from each other and so the tiny volume they occupy will be a smaller fraction of the total volume.
At higher temperatures, the particles will have more kinetic energy, which means that they will have larger average speed, and so the forces between the molecules will count less.
So, you conclude that <em>under low pressure and high temperatures a real gas is most likely to behave ideally.</em>
201 grams.
<h3>Explanation</h3>
What's the formula of Silver Sulfide?
Consider the two kinds of ions in silver sulfide:
- Silver ions , and
- Sulfide ions .
The charge on the two types of ions should balance. The charge on each sulfide ion is twice as much as that on a silver ion. There needs to be <em>two</em> silver ions for each sulfide ion.
Hence the formula: .
How many <em>moles </em>of formula units in 174 grams of Ag₂S.
Relative atomic mass from a modern periodic table:
- Silver Ag: 107.868;
- Sulfur S: 32.06;
- Chlorine Cl: 35.45.
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How many <em>moles</em> of AgCl formula units will be formed from 174 grams of Ag₂S?
The question doesn't mention the other product in this reaction. Finding that product isn't a must as long as all Ag from Ag₂S end up in AgCl.
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We are trying to answer the question: how many moles of AgCl does <em>each</em> mole formula unit of Ag₂S produce. Thus, assign a coefficient of <em>one</em> to Ag₂S.
There are two silver atoms in each formula unit Ag₂S. Both would end up in AgCl. However, there's only one silver atom in each formula unit of AgCl. Two Ag atoms would make two formula units of AgCl. In other words, each mole formula units of Ag₂S would produce <em>two</em> moles formula units of AgCl.
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There are 0.702 moles of Ag₂S formula units in 174 grams of the compound. That would lead to of AgCl.
What's the mass of 1.40 mol of AgCl?
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