Answer:
A. endothermic.
A. Yes, absorbed.
Explanation:
Let's consider the following thermochemical equation.
2 HgO(s) ⇒ 2 Hg(l) + O₂(g) ΔH = 182 kJ
The enthalpy of the reaction is positive (ΔH > 0), which means that the reaction is endothermic.
182 kJ are absorbed when 2 moles of HgO react (molar mass 216.59 g/mol). The heat absorbed when 72.8 g of HgO react is:
<u>Answer:</u> The ratio of carbon in both the compounds is 1 : 2
<u>Explanation:</u>
Law of multiple proportions states that when two elements combine to form two or more compounds in more than one proportion. The mass of one element that combine with a given mass of the other element are present in the ratios of small whole number. For Example:
Total mass of sample = 100 g
Mass of carbon = 27.2 g
Mass of oxygen = (100 - 27.7) = 72.8 g
To formulate the formula of the compound, we need to follow some steps:
Moles of Carbon =
Moles of Oxygen =
For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 2.26 moles.
For Carbon =
For Oxygen =
The ratio of C : O = 1 : 2
Hence, the formula for sample 1 is
Total mass of sample = 100 g
Mass of carbon = 42.9 g
Mass of oxygen = (100 - 42.9) = 57.1 g
To formulate the formula of the compound, we need to follow some steps:
Moles of Carbon =
Moles of Oxygen =
For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 3.57 moles.
For Carbon =
For Oxygen =
<u>Step 3:</u> Taking the mole ratio as their subscripts.
The ratio of C : O = 1 : 1
Hence, the formula for sample 1 is
In the given samples, we need to fix the ratio of oxygen atoms.
So, in sample one, the atom ratio of oxygen and carbon is 2 : 1.
Thus, for 1 atom of oxygen, the atoms of carbon required will be =
Now, taking the ratio of carbon atoms in both the samples, we get:
Hence, the ratio of carbon in both the compounds is 1 : 2