1.43.4 kcal of heat is required to decompose 2 mole of mecury(II) oxide according to the equation 2HgO(s)➡2Hg(l) + O⬇2(g) . What quantity of energy is required to decompose 10.8g of HgO ? (Hg=200.59, O=16)
Is that question 1 which says 43.4 kcal or some other notation. If I have interpreted this correctly, then
1 mol HgO is (216.6) so 2 mols = 2*216.6. You have 10.8 g; therefore,
43.4 Kcal x [10.8/(2*216.6)] = ?
2.17kcal
To find the quantity of energy required to decompose 10.8g of HgO, we need to follow these steps:
Step 1: Calculate the molar mass of HgO
The molar mass of HgO can be calculated by summing the atomic masses of its constituent elements:
Hg = 200.59 g/mol
O = 16.00 g/mol
Molar mass of HgO = 200.59 + 16.00 = 216.59 g/mol
Step 2: Convert the mass of HgO to moles
The number of moles of HgO can be calculated using the formula:
moles = mass / molar mass
moles = 10.8 g / 216.59 g/mol ≈ 0.0499 mol
Step 3: Use the mole ratio to find the quantity of energy required
From the balanced equation, we can see that 2 moles of HgO require 1.43.4 kcal of heat energy for decomposition. Therefore, we can set up a mole ratio to find the energy required for 0.0499 mol of HgO:
1.43.4 kcal / 2 mol = x kcal / 0.0499 mol
Cross multiply and solve for x:
x = (1.43.4 kcal * 0.0499 mol) / 2 mol ≈ 1.42 kcal
Therefore, the quantity of energy required to decompose 10.8g of HgO is approximately 1.42 kcal.
To find the quantity of energy required to decompose 10.8 grams of HgO, you need to convert the given mass to moles using the molar mass of HgO.
1. Calculate the molar mass of HgO:
Molar mass of Hg = 200.59 g/mol
Molar mass of O = 16 g/mol
Molar mass of HgO = (2 * molar mass of Hg) + molar mass of O
Molar mass of HgO = (2 * 200.59 g/mol) + 16 g/mol
Molar mass of HgO = 401.18 g/mol + 16 g/mol
Molar mass of HgO = 417.18 g/mol
2. Convert the given mass of HgO to moles:
Number of moles = mass (in grams) / molar mass
Number of moles = 10.8 g / 417.18 g/mol
3. Calculate the quantity of energy required using the stoichiometry of the reaction:
The stoichiometry of the reaction states that 2 moles of HgO decompose to produce 2 moles of Hg and 1 mole of O2. Therefore, the heat energy required for 2 moles of HgO is 1.43.4 kcal.
To find the quantity of energy required for the calculated number of moles of HgO, set up a proportion:
(1.43.4 kcal) / (2 moles of HgO) = (X kcal) / (calculated moles of HgO)
Cross multiply and solve for X to find the quantity of energy required to decompose 10.8 g of HgO.