The iron filings<span> can be separated with a magnet. The </span>wood chips<span> can be separated by adding water to the water and picking the floating </span>wood chips<span>from the top. The </span>sand<span> can be separated by pouring the water/</span>sand/salt<span>mixture through a coffee filter or a paper towel</span>
If it an alkyne and gives 3-ethylhexane on hydrogenation then the reaction will be
There will be three isomers of alkyne with given molecular formula
The reactions are shown in the attached figure
<span>Eventually the increase in water may cause the blood cells to burst (cytolysis.) In a hypertonic solution, the concentration of dissolved solutes is greater than that of the cell. ... If the salt solution outside is 20% salt, then the water concentration is 80%.
The red blood cells will shrink in size due to osmotic-like pressure differences until it reaches a "favorable" size.</span>
What you are looking for is something from the left side of the periodic table (the metals), combined with something from the right side of the periodic table.
SiCl4 is something from the middle with something on the right. Not the answer.
HCl is a possible answer, but it is not the best one, because Hydrogen can be on both sides. It is not quite as willing to give up its electrons as the answer.
CCl4 has the same problem as A.
The answer is C
Ca is in column 2 just about as far left as you can get.
Cl is in column 17 which is just about as far right as you can get.
Answer:
The correct answer is: 6.6 g MgO
Explanation:
First we have to write and balance the chemical reaction as follows:
2Mg(s) + O₂(g) → 2MgO(s)
That means that 2 moles of Mg(s) react with 1 mol of O₂(g) to give 2 moles of MgO(s). If Mg is totally consumed and a mass of O₂ remains unaltered after reaction, t<em>he limiting reactant is Mg</em>. We use the limiting reactant to calculate the mass of product.
According to the balanced chemical equation, 2 moles of Mg(s) produce 2 moles of MgO(s).
2 moles Mg = 2 mol x molar mas Mg= 2 mol x 24.3 g/mol = 48.6 g Mg
2 moles MgO= 2 mol x (molar mass Mg + molar mass O) = 2 mol x (24.3 g/mol + 16 g/mol) = 80.6 g MgO
The stoichiometric ratio is 80.6 g MgO/48.6 g Mg. So, we multiply this ratio by the mass of consumed Mg (4.0 g) in order to obtain the produced mass of MgO:
4.0 g Mg x 80.6 g MgO/48.6 g Mg = 6.63 g MgO
6.6 grams of magnesium oxide are formed.