For the answer to the question above, <span>1.18 x 3 = 3.55.</span>
<span>First, you need to find the ratio of F to F in each compound. It is the law of multiple proportions stating that the masses of one element which combine with a fixed mass of the second element are in a ratio of whole numbers. In this case, F would be the "one element" and S would be the "fixed mass", the ratio of F6 to Fx = 3:1 </span>
<span>therefore x would be 2 since there is less F in SFx and the ratio is 3:1. divide 6 by 3 and you get 2.</span>
Answer:
0.071L
Explanation:
From the question given, we obtained the following data:
Molarity of HCl = 2.25 M
Mass of HCl = 5.80g
Molar Mass of HCl = 36.45g/mol
Number of mole of HCl =?
Number of mole = Mass /Molar Mass
Number of mole of HCl = 5.8/36.45 = 0.159mole
Now, we can obtain the volume required as follows:
Molarity = mole /Volume
Volume = mole /Molarity
Volume = 0.159mole/ 2.25
Volume = 0.071L
Answer:
1. a)
2. a)
3. b)
4. d)
Explanation:
The disposal method is how we throw away the wastes. In a chemical lab, the correct disposal method guarantees the security of the environment and the humans and animals that may be in contact with the materials.
So:
1. Excess chemical: Because it can be toxic, it may be disposed of in the appropriate waste container, which will depend on the characteristics of the material;
2. Reaction mixture: As the excess chemical, it can be toxic, so it must be disposed of at an appropriate waste container;
3. Used filter paper: Generally, the solids in the filter paper is not toxic, so it can be thrown away in the trash can;
4. Cracked or chipped beaker: Because the beaker is made of glass, it can cut when broken, so it must go to a broken glass box, that will protect the people that will deal with it.
Answer:
D. Partial pressure
Explanation:
Partial pressure is the individual pressure exerted by each gas present in a gaseous mixture. As he is measuring the pressure of each gas in the atmosphere separately, so PARTIAL PRESSURE is the exact term for his measurement.
