Na3PO4 • 12 H2O (s) ----> Na3PO4 (s) + 12 H2O (g)
A reaction doesn't occur.
When a reaction has products that have a lower temperature than the reactants did, the reaction is endothermic.
4-methylcyclohexene, 3-methylcyclohexene and 1-methylcyclohexene which is the major product because it is trisubstituted as opposed to the first two which are only disubstituted
Glucose monomers
They would be equal .Because of the conservation of matter no mass can be destroyed or created
Usually these reaction are done with a substantial excess of NaOH. You would getH3PO4 + 3NaOH --> Na3PO4(aq) + 3HOH.
No. Dehydration causes it.
This reaction would yield a fatty acid glyceryl monoester, more commonly called a monoglyceride or monoacylglycerol.
I assume double displacement reaction. Balanced equation. 3AgNO3 + Na3PO4 -> Ag3PO4 + 3NaNO3 2.00 moles sodium phosphate ( 3 moles AgNO3/1 mole Na3PO4) = 6.00 moles silver nitrate needed =========================
A reaction doesn't occur.
The reactants are on the left side of the equation, and the products are on the right side of the equation. The reactants are used up in a chemical reaction, and the products are the substances made by the reaction.
You would add water through a hydrolysis reaction to reverse the condensation reaction (dehydration synthesis) that you started with to form the starch into a polysaccharide. All in all, you would just add WATER.
A reaction which goes to completion without the product of any by products, in effect a reaction which has a 100% yield. Although that would be impossible
When a reaction has products that have a lower temperature than the reactants did, the reaction is endothermic.
A chemical reaction whose reactants have less potential energy than the products would be called an endothermic reaction.
4-methylcyclohexene, 3-methylcyclohexene and 1-methylcyclohexene which is the major product because it is trisubstituted as opposed to the first two which are only disubstituted
It measures the amount of reactants actually produced in a reaction compared to the amount that would theoretically be produced if 100% of the reactants were converted to products according to the stoichiometry of the reaction. It is found by: actual moles of products ÷ predicted moles of products * 100%