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Kruka [31]
4 years ago
7

Please please please please please help me

Chemistry
1 answer:
Papessa [141]4 years ago
6 0

Answer: Iodine

Explanation:

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the earth is green because the green part is the plants and tree.

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Which group 1 metal and group 2 non metal would react together most?​
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A balanced chemical equation is a direct presentation of the ___________.
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The chemical equation needs to be balanced so that it follows the law of conservation of mass. A balanced chemical equation occurs when the number of the different atoms of elements in the reactants side is equal to that of the products side.

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How do you balance equations?

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3 years ago
1: Write balanced complete ionic equation for
monitta

Answer 1 : The balanced complete ionic equation will be,

NaOH(aq)+HNO_3(aq)\rightarrow H_2O(l)+NaNO_3(aq)

Na^+(aq)+OH^-(aq)+H^+(aq)+NO_3^-(aq)\rightarrow H_2O(l)+Na^+(aq)+NO_3^-(aq)

By removing the spectator ion in this equation, we get the balanced ionic equation.

OH^-(aq)+H^+(aq)\rightarrow H_2O(l)

Answer 2 : The balanced net ionic equation will be,

2Na_3PO_4(aq)+3NiCl_2(aq)\rightarrow Ni_3(PO_4)_2(s)+6NaCl(aq)

6Na^+(aq)+2PO_4^{3-}(aq)+3Ni^+(aq)+6Cl^-(aq)\rightarrow Ni_3(PO_4)_2(s)+6Na^+(aq)+6Cl^-(aq)

By removing the spectator ion in this equation, we get the balanced ionic equation.

2PO_4^{3-}(aq)+3Ni^+(aq)\rightarrow Ni_3(PO_4)_2(s)

Answer 3 : The balanced net ionic equation will be,

2Na_3PO_4(aq)+3NiCl_2(aq)\rightarrow Ni_3(PO_4)_2(s)+6NaCl(aq)

6Na^+(aq)+2PO_4^{3-}(aq)+3Ni^+(aq)+6Cl^-(aq)\rightarrow Ni_3(PO_4)_2(s)+6Na^+(aq)+6Cl^-(aq)

By removing the spectator ion in this equation, we get the balanced ionic equation.

2PO_4^{3-}(aq)+3Ni^+(aq)\rightarrow Ni_3(PO_4)_2(s)

Balanced equations : Balanced equations are the equations in which the number of individual elements present on the reactant side must be equal to the number of individual elements present on the product side.

Spectator ions : It is defined as the ions which do not participate in the chemical reaction. These ions exists in the same form on both the sides of the reaction.

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