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3 years ago

1. Balance the following equations:a. -C8H18(1) + ___02(g) +CO2(g) +H2O(1)

Chemistry

1 answer:

LenaWriter [7]3 years ago

4 0

Answer:

1. 2C8H18 + 25O2 —> 16CO2 + 18H2O

2. The coefficient of O2 is 25

Explanation:

C8H18 + O2 —> CO2 + H2O

The above equation can be balance as follow:

There are 8 atoms of C on the left side and 1 atom on the right side. It can be balance by putting 8 in front of CO2 as shown below:

C8H18 + O2 —> 8CO2 + H2O

There are 18 atoms of H on the left side and 2 atoms on the right. It can be balance by putting 9 in front of H2O as shown below:

C8H18 + O2 —> 8CO2 + 9H2O

Now, there are a total of of 25 atoms of O on the right side and 2 atoms on the left side. It can be balance by putting 25/2 in front of O2 as shown below:

C8H18 + 25/2O2 —> 8CO2 + 9H2O

Multiply through by 2 to clear the fraction as shown below :

2C8H18 + 25O2 —> 16CO2 + 18H2O

Now the equation is balanced.

2. 2C8H18 + 25O2 —> 16CO2 + 18H2O

From the balanced equation above, the coefficient of O2 is 25

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What is the empirical formula for a compound that is 83.7% carbon and 16.3% hydrogen?

zubka84 [21]

Hello!

We use the amount in grams (mass ratio) based on the composition of the elements, see: (in 100 g solution)

C: 83.7% = 83,7 g
H: 16.3% = 16.3 g

Let us use the above mentioned data (in g) and values will be converted to amount of substance (number of moles) by dividing by molecular mass (g / mol) each of the values, lets see:

$C: \dfrac{83.7\:\diagup\!\!\!\!\!g}{12\:\diagup\!\!\!\!\!g/mol} \approx 6.975\:mol$

$H: \dfrac{16.3\:\diagup\!\!\!\!\!g}{1\:\diagup\!\!\!\!\!g/mol} = 16.3\:mol$

We note that the values found above are not integers, so let's divide these values by the smallest of them, so that the proportion is not changed, let's see:

$C: \dfrac{6.975}{6.975} = 1$

$H: \dfrac{16.3}{6.975} \approx 2.3$

Note: So the ratio in the smallest whole numbers of carbon to hydrogen is 3:7, t<span>hus, the minimum or empirical formula found for the compound will be:
</span>
$\boxed{\boxed{C_3H_7}}\end{array}}\qquad\checkmark$

I hope this helps. =)

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3 years ago

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Vaselesa [24]

Answer:

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Explanation:

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3 years ago

If you have a 1500 g aluminum pot, how much heat energy is needed to raise its temperature by 100°C?

Nataly [62]

The heat energy required to raise the temperature of 1500 g of aluminium pot by 100°C is 135 kJ.

The heat energy required to raise the temperature of 1500 g of copper pot by 100 °C is 57.75 kJ.

Explanation:

The heat energy required to raise the temperature of any body can be obtained from the specific heat formula. As this formula states that the heat energy required to raise the temperature of the body is directly proportional to the product of mass of the body, specific heat capacity of the material and temperature change experienced by the material.

So in this problem, the mass of the aluminium is given as m = 1500 g, the specific heat of the aluminium is 0.900 J/g °C. Then as it is stated that the temperature is raised by 100 °C, so the pots are heat to increase by 100 °C from its initial temperature. This means the difference in temperature will be 100°C (ΔT = 100°C).

Then, the heat energy required to raise the temperature will be

$q = m*c*del T = 1500 * 0.900 * 100 = 135000 = 135 kJ$

Thus, the heat energy required to raise the temperature of 1500 g of aluminium pot by 100 °C is 135 kJ.

Similarly, the mass of copper pot is given as 1500 g, the specific heat capacity of copper is 0.385 and the difference in temperature is 100 °C.

Then, the heat energy required to raise its temperature will be

$q = m*c*del T = 1500 * 0.385 * 100 = 57750 = 57.75 kJ$

And the heat energy required to raise the temperature of 1500 g of copper pot by 100°C is 57.75 kJ.

So, the heat energy required to raise the temperature of 1500 g of aluminium pot by 100°C is 135 kJ. And the heat energy required to raise the temperature of 1500 g of copper pot by 100 °C is 57.75 kJ.