Determine how many grams of water are produced when burning 1.71 g of hexane, C6H14(l), as a component of gasoline in automobile engines. Assume excess oxygen is present.

2.51 g of H2O.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below below:

2C6H14 + 19O2 —> 12CO2 + 14H2O

Next, we shall determine the mass of hexane (C6H14) that reacted and the mass of water (H2O) produce from the balanced equation. This is illustrated below:

Molar mass of C6H14 = (12×6) + (14×1)

= 72 + 14

= 86 g/mol

Mass of C6H14 from the balanced equation = 2 × 86 = 172 g

Molar mass of H2O = (2×1) + 16

= 2 + 16

= 18 g/mol

Mass of H2O from the balanced equation = 14 × 18 = 252 g

From the balanced equation above,

172 g of C6H14 reacted to produce 252 g of H2O.

Finally, we shall determine the mass of water produced by burning 1.71 g of hexane, C6H14. This is illustrated below:

From the balanced equation above,

172 g of C6H14 reacted to produce 252 g of H2O.

Therefore, 1.71 g of C6H14 will react to produce = (1.71 × 252) / 172 = 2.51 g of H2O.

Therefore, 2.51 g of H2O were obtained from the reaction.

each  column  of the  table  is called a group. elements in a group share similar properties. groups are  read  from  top  to  bottom. metal. metalloid. nonmetal. solid. liquid. gas. fe. hg. o.  2. 3. 4. 5. 6. 7. 8. 9.  2. beryllium. 9.012. 4.  sodium. 22.990.  11. 3.  magnesium. 24.305.  12.  potassium. 39.098.  19. 4.  calcium. 40.078.  20. i guess  i  

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.