One mole of carbon atoms has a mass of exactly 12 g. Because magnesium atoms each have twice the mass of carbon atoms (24Mg compared with 12C), one mole of magnesium has a mass of 24 g. In fact, one mole of any element has a mass in grams that is equal to its relative atomic mass. One mole of iron has a mass of 56 g
Answer:
2g
Explanation:
The balanced equation for the reaction is given below:
2Na + 2H2O —> 2NaOH + H2
Next, we'll determine the mass of the water (H2O) that reacted and the mass of H2 produced from the balanced equation.
This is illustrated below:
Molar Mass of H2O = (2x1) + 16 = 18g/mol
Mass of H2O from the balanced equation = 2 x 18 = 36g
Molar Mass of H2 = 2x1 = 2g/mol
Therefore, from the balanced equation above, 36g of H2O reacted to produce 2g of H2.
From the illustration above, we can see that 36g of water will produce 2g of H2.
Answer:
2HgS + 3O2 → 2HgO + 2SO2
The coefficients are: 2, 3, 2, 2
Explanation:
HgS + O2 → HgO + SO2
The equation can be balance as follow:
Put 3 in front of O2 as shown below:
HgS + 3O2 → HgO + SO2
Now we can see that there are 6 atoms of O on the left side of the equation and a total of 3 atoms on the right side. It can be balance by putting 2 in front of HgO and SO2 as shown below:
HgS + 3O2 → 2HgO + 2SO2
Now we have 2 atoms of both Hg and S on the right side and 1atom each on the left. It can be balance by putting 2 in front of HgS as shown below:
2HgS + 3O2 → 2HgO + 2SO2
Now the equation is balanced.
The coefficients are: 2, 3, 2, 2
The law of conservation of mass(matter) states that matter(mass) can neither be created nor destroyed during a chemical reaction but changes from one form to another. An unbalanced equation suggests that matter has been created or destroyed. While a balanced equation proofs that matter can never be created but changes to different form. This is the more reason we have count the atoms of an element on both side of the equation to see if they are balanced irrespective of the new form they assume in the product
Answer:
Water and applesauce are examples of a Homogeneous Mixture
Chicken Noodle Soup and Soil with Water would be examples of a Heterogeneous Mixture.
Explanation:
Homogeneous Mixtures are mixtures that are the same throughout, i.e. it's just one substance. A good example of this is a glass of water, this is because it is all one solution <u><em>without any other visible</em></u><u> </u><u><em>different parts</em></u><em> </em>that will settle if left alone for a while. The same applies to the applesauce, it is one type of a mixture with nothing else added to it.
Hetergeneous Mixtures on the other hand <u><em>are different substances </em></u>added together. The noodles, soup and chicken, three different substances in one mixture. The soil and water mixture also applies, two substances which separate if left alone.
See http://chemistry.elmhurst.edu/vchembook/106Amixture.html#:~:text=A%20homogeneous%20mixture%20has%20the,gas%2C%20liquid%2C%20and%20solid. For more information.
Answer:
<em>Solution:</em>
Explanation:
V1 = 3.00m3
T1 = 150kPa
V2 = 1.20m3
T2 = x
As ,
<u> V1 </u> = <u>V2</u>
T1 T2
<u> 3.00</u> = <u>1.20</u>
150 X
3.00 x X = 150 x 1.20
3.00X = 180
X = <u>180</u>
3.00
<em>X = 60 kPa</em>