Explanation:
Yes, a chemical reaction can happen with only one substance.
A typical example of such reaction is the radioactive decay.
Radioactive decay is the loss of elementary particles from an unstable nucleus, ultimately changing the unstable element into another more stable element. .
When radioactive elements are let alone, they decompose to form stable harmless elements.
An example of radioactive decay is attached in the image below;
Answer:
For a good consert mix aggregate needed to the clean hard strong partical free of absorb chemicals or coating clay and other fine materials
Answer:
<u><em></em></u>
- <u><em>Concentrated</em></u>
Explanation:
Concentration measures the amount of solute in a solution. There are many expressions of concentration. Some of then are percentage (mass/mass, volume/mass, volume/volume), molarity, molality, mole fraction, among others.
When a solution has a high concentration it is said that it is <em>concentrated; </em>when a solution has a low concentration is is said that is is diluted.
Concentrated solutions expressed in percentage typically have about 80 - 90% (or more) of solute.
Diluted solutions expressed in percentage, tipylcally have about 10% - 20% or less.
But they are not fixed limits. You might say that a 85% solution is concentrated. Acids at 75 % sure are concentrated.
Hence, a 93.3% solution is concentrated, definitely.
Hello.
The answer would be <span>A. Three feet of concrete.
Have a nice day.</span>
You would need to utilize Mole ratios found in the adjusted condition;
for each mole of hydrogen utilized, 2 moles of HCl are delivered.
Thusly:
10 mol H2 x 2 mol HCl/1 mol H2 = 20 mol HCL.
For the second question:
you would need to change over 2.0x10^23 particles of Oxygen to moles of oxygen, utilizing Avogadro's number:
2.0x10^23 particles oxygen x 1 mol oxygen/6.022x10^23 atoms oxygen = 0.33 mol Oxygen
utilizing mole proportions once more:
0.66 mol H2O = 2 mol H2O/1 mol Oxygen x 0.33 mol Oxygen
45.0 mol H2O = 2 mol H2O/1 mol Oxygen x 22.5 mol Oxygen
fundamentally to answer stoichiometry, you should take a gander at the adjusted condition to make sense of the mole proportions between components/mixes, and utilizing mole proportions you can change over from moles of one component/compound to moles of another component/compound
