A process to produce aluminum from aluminum oxide has an 85.0% yield. How much aluminum will be produced from a reaction 700.0 kg of aluminum oxide to produce Al? (assume that the reaction is Al2O3 + H2=Al+H2O

Explanation:

First you need to calculate the theoretical yield using the balanced chemical equation and the amount of aluminium available to react. Next, you use the percent yield to calculate the true yield.

1. Balanced chemical equation:

2. Mole ratios

3. Number of moles of aluminium oxide

4. Number of moles of aluminium

The mole ratio is ; thus 6,865.4 mol of aluminium oxide produce 2 × 6,865.4 mol of aluminum = 13,730.8 mol of aluminium.

5. Calculate the mass of 13,730.8 mol of aluminium

6. Calculate the actual yield

7. Convert to kg and three significant figures

we can conclude that the melting point of table salt is above room temperature (it's actually 801 deg c). the melting point of mercury must be below room temperature (- 39 deg c).

"among the transition metal elements, manganese and zinc have a slight lowering of electronegativities. the reason behind this is that the nuclear charges of these elements are slightly weaker than the other transition metal elements due to the way their valence electrons are filled up. both manganese and zinc have their valence electrons filled up to the 4th shell with 1 pair of electrons (4s2) completely occupying it. although the electrons in the 3rd shell (3d) are yet to be paired since the outer most shell is filled up, the ability of the nucleus to attract electrons is lessened. hence,   the electronegativity (or the ability to attract electrons) is lessened."