Question

Convert the following into balanced equations. ( Use the lowest possible coefficents)?(a) When gallium metal is heated in oxygen gas, it melts and forms solid gallium(III) oxide. (b) Liquid hexane burns in oxygen gas to form carbon dioxide gas and water vapor. (c) When solutions of calcium chloride and sodium phosphate are mixed, solid calcium phosphate forms and sodium chloride remains in solution.

Answer 1

The balanced chemical equations for the reactions provided are 4Ga(s) + O2(g) → 2Ga2O3(s), 2C6H14(l) + 19O2(g) → 12CO2(g) + 14H2O(g), and 3CaCl2(aq) + 2Na3PO4(aq) → Ca3(PO4)2(s) + 6NaCl(aq).

Step-by-step explanation:

To convert the given descriptions into balanced chemical equations, we use the lowest possible coefficients:

1. When gallium metal is heated in oxygen gas, it melts and forms solid gallium(III) oxide:
   4Ga(s) + O2(g) → 2Ga2O3(s)
2. Liquid hexane burns in oxygen gas to form carbon dioxide gas and water vapor:
   2C6H14(l) + 19O2(g) → 12CO2(g) + 14H2O(g)
3. When solutions of calcium chloride and sodium phosphate are mixed, solid calcium phosphate forms and sodium chloride remains in solution:
   3CaCl2(aq) + 2Na3PO4(aq) → Ca3(PO4)2(s) + 6NaCl(aq)

Here, we've included only the relevant parts of the question and omitted typos as instructed.

Answer 2

Step-by-step explanation:

(a) Balanced reaction of gallium with oxygen is as follows:

`4Ga(s)+3O_2(g) \rightarrow 2Ga_2O_3 (s)`

(b)
`C_6H_(14)(l)+O_2(g)\rightarrow CO_2(g)+H_2O(l)`

Multiply the carbon dioxide by 6 to balance carbon as follows:

`C_6H_(14)(l)+O_2(g)\rightarrow 6CO_2(g)+H_2O(l)`

After that multiply H2O by 7 to balance hydrogen as follows:

`C_6H_(14)(l)+O_2(g)\rightarrow CO_2(g)+7H_2O(l)`

Finally balance oxygen by multiplying O2 by 19/2. Therefore, balanced reaction is as follows:

`C_6H_(14)(l)+(19)/(2) O_2(g)\rightarrow 6CO_2(g)+7H_2O(l)`

(c)
`Na_3PO_4(s)+CaCl_2 \rightarrow Ca_3(PO_4)_2+NaCl`

first balance calcium, by multiply
`CaCl_2` by 3 as follows:

`Na_3PO_4(s)+3CaCl_2 \rightarrow Ca_3(PO_4)_2+NaCl`

After that balance phosphorous by multiplying
`Na_3PO_4` by 2 as follows:

`2Na_3PO_4(s)+3CaCl_2 \rightarrow Ca_3(PO_4)_2+NaCl`

Finally balance Na by multiplying NaCl by 6. Therefore, balance reaction is as follows:

`2Na_3PO_4(s)+3CaCl_2 \rightarrow Ca_3(PO_4)_2+6NaCl`