Answer:
The answer is sodium which is the element is the most reactive.
To convert the given value we need conversion factors to relate molecules to liters. At STP, we know that 1 mol is equal to 22.4 L and by using Avogadro's number we can relate molecules to 1 mol. Calculation is as follows:
5.0x10^24 molecules ( 1
mol / <span>6.022 x 10^23 molecules<span> ) ( 22.4 L / 1 mol) = 186.0 L </span></span>
Answer:
The law of multiple proportions is the third postulate of Dalton's atomic theory. It states that the masses of one element which combine with a fixed mass of the second element are in a ratio of whole numbers.
Therefore, the masses of oxygen in the two compounds that combine with a fixed mass of carbon should be in a whole number ratio. In 100 grams of the first compound (100 is chosen to make calculations easier), there are 57.1 grams oxygen and 42.9 grams carbon. The mass of oxygen (O) per gram of carbon (C) is:
57.1 g O / 42.9 g C = 1.33 g O per g C
In the 100 grams of the second compound, there are 72.7 grams of oxygen (O) and 27.3 grams of carbon (C). The mass of oxygen per gram of carbon is:
72.7 g O / 27.3 g C = 2.66 g O per g C
Dividing the mass O per g C of the second (larger value) compound:
2.66 / 1.33 = 2
This means that the masses of oxygen that combine with carbon are in a 2:1 ratio. The whole-number ratio is consistent with the law of multiple proportions.
Explanation:
<span>coefficient is 2
2Al (s) + 3 ZnCl2s (aq) --> 3 Zn (s) + 2 AlCl3 (aq) </span>
<u>Answer:</u> The amount of acetylene gas needed in the reaction is 2.00 moles
<u>Explanation:</u>
We are given:
Moles of water = 2.00 moles
The chemical equation for the reaction of acetylene with oxygen gas follows:
By Stoichiometry of the reaction:
2 moles of water is produced by 2 moles of acetylene gas
So, 2.00 moles of water will be produced by = 
of acetylene gas
Hence, the amount of acetylene gas needed in the reaction is 2.00 moles
