Answer:
We can solve this by the method of which i solved your one question earlier
so again here molar mass of C12H25NaSO4 is 288.372 and number of moles for 11900 gm of C12H25NaSO4 will be = 11900/288.372
which is almost = 41.26 moles
so to get one mole of C12H25NaSO4 we need one mole of C12H26O
so for 41.26 moles of C12H25NaSO4 it will require 41 26 moles of C12H26O
so the mass of C12H26O = 41.26× its molar mass
C12H26O = 41.26×186.34
= 7688.38 gm!!
so the conclusion is If you need 11900 g of C12H25NaSO4 (Sodium Lauryl Sulfate) you need C12H26O 7688.38 gm !!
Again i d k wether it's right or wrong but i tried my best hope it helped you!!
Metal atoms have outer electrons which are not tied to any one atom. These electrons can move freely within the structure of a metal when an electric current is applied. There are no such free electrons in covalent or ionic solids, so electrons can't flow through them - they are non-conductors.
In a shorter term - no
<span>Transmutation
is the process of changing the substance, tangible or not, from one form to the
other. It means the transformation of one element in the periodic table into
another by one or a series of nuclear decays or reactions. One type of transmutation
is nuclear transmutation. Nuclear transmutation is the conversion of one
chemical element or isotope into another though nuclear reactions or nuclear
decay. Second type of transmutation is artificial transmutation. Artificial transmutation
occur in machinery that uses nough energy to cause changes in the nuclear
structure of the elements.</span>
B <span>Divide the chemical equation into two half-reaction equations, identifying which half-reaction is oxidation and which is reduction
</span>
Answer:
Oxidation state] is defined as the charge an atom might be imagined to have when electrons are counted according to an agreed-upon set of rules:
The oxidation state of a free element (uncombined element) is zero for a simple (monoatomic) ion, the oxidation state is equal to the net charge on the ion.
Hydrogen has an oxidation state of 1 and oxygen has an oxidation state of −2 when they are present in most compounds. (Exceptions to this are that hydrogen has an oxidation state of −1 in hydrides of active metals, e.g. LiH, and oxygen has an oxidation state of −1 in peroxides, e.g. H2O2 the algebraic sum of oxidation states of all atoms in a neutral molecule must be zero, while in ions the algebraic sum of the oxidation states of the constituent atoms must be equal to the charge on the ion.
The same is written in my textbook. But how am I supposed to find the ox. number of an atom, which is in compound like K2UO4?
