Balance the equations

2 answers:

4 0

Answer:

Instructions on balancing chemical equations:
Enter an equation of a chemical reaction and click 'Balance'. The answer will appear below
Always use the upper case for the first character in the element name and the lower case for the second character. Examples: Fe, Au, Co, Br, C, O, N, F. Compare: Co - cobalt and CO - carbon monoxide
To enter an electron into a chemical equation use {-} or e
To enter an ion specify charge after the compound in curly brackets: {+3} or {3+} or {3}.
Example: Fe{3+} + I{-} = Fe{2+} + I2
Substitute immutable groups in chemical compounds to avoid ambiguity.
For instance equation C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced,
but PhC2H5 + O2 = PhOH + CO2 + H2O will
Compound states [like (s) (aq) or (g)] are not required.
If you do not know what products are enter reagents only and click 'Balance'. In many cases a complete equation will be suggested.
Reaction stoichiometry could be computed for a balanced equation. Enter either the number of moles or weight for one of the compounds to compute the rest.
Limiting reagent can be computed for a balanced equation by entering the number of moles or weight for all reagents.

Dafna1 [17]3 years ago

3 0

Fe + Cl2 = FeCl3

KMnO4 + HCl = KCl + MnCl2 + H2O + Cl2

PhCH3 + KMnO4 + H2SO4 = PhCOOH + K2SO4 + MnSO4 + H2O

calcium hydroxide + carbon dioxide = calcium carbonate + water

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antiseptic1488 [7]

Answer:

1. NaCl .

Explanation:

Hello there!

In this case, it is necessary to keep in mind that just ionic compounds are able to conduct electricity and therefore, the more ionic the compound is, the more electricity it conducts. In such a way, we may be able to predict how ionic these compounds are, considering that the electronegativity increases from bottom to top and from left to right.

1. NaCl: this is the most ionic compound since it is at the leftmost group and bonded with chlorine, so this is the most conductive one.

2. Mg(CIO3)2: Mg is bonded to O, not to Cl, which makes the compound ionic but not as ionic as NaCl.

3. NiCl: Ni is more electronegative than Na and Mg, so even when this is ionic, it is not as ionic as NaCl.

4. CaCl2: This is similar to NaCl but since Ca is in group 2A, it is more electronegative than Na, which makes CaCl2 conductive but not as much as NaCl.

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