First, we calculate the number of moles of each reactant using the formula:
Moles = mass / molecular weight
CaO:
Moles = 7.15/56 = 0.128
Water:
Moles = 152/18 = 8.44
The reaction equation shows that the reactants must be present in an equal number of moles, so CaO will be the limiting reactant and 0.128 mole of calcium hydroxide will form.
The energy released is given by:
Heat of reaction * number of moles
= -64.8 * 0.128
= -8.29 kJ
8.29 kJ of energy will be released
Answer: Im not sure if you are doing this in your class.
Explanation:
So... for the element of MAGNESIUM, you already know that the atomic number tells you the number of electrons. That means there are 12 electrons in a magnesium atom. Looking at the picture, you can see there are two electrons in shell one, eight in shell two, and two more in shell three
Answer:
7.34684 × 10^23 atoms
Explanation:
Well, one mole is basically
6.022 × 10^23 atoms. So 1.22 moles would be
6.022 × 10^23 ⋅ 1.22 atoms.
6.022 × 10^23 ⋅ 1.22 = 7.34684 × 10^23 atoms
<h3>
Answer:</h3>
126.14 g
<h3>
Explanation:</h3>
- Complete combustion of hydrocarbons yields water and carbon dioxide.
- Methane is a hydrocarbon in the homologous series known as alkanes.
- Methane undergoes combustion in air to produce water and carbon dioxide according to the equation below.
CH₄ (g) + 2O₂ (g) → CO₂(g) + 2H₂O(g)
<u>We are given;</u>
We are required to determine the mass of H₂O produced
<h3>Step 1: Moles of H₂O produced</h3>
- From the equation 1 mole of methane undergoes combustion to produce 2 mole of H₂O.
Therefore, Moles of methane = Moles of H₂O × 2
Hence, Moles of H₂O = 7.0 moles
<h3>Step 2: Mass of H₂O produced </h3>
We know that; mass = Moles × Molar mass
Molar mass of water = 18.02 g/mol
Therefore;
Mass of water = 7.0 moles × 18.02 g/mol
= 126.14 g
Thus, the mass of water produced is 126.14 g
