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3 years ago

Why does a mole of silicon weigh a different amount than a mole of carbon?

Chemistry

1 answer:

solniwko [45]3 years ago

5 0

Answer:

$\boxed {\boxed {\sf Different \ amount \ of \ protons, neutrons, \ and \ electrons}}$

Explanation:

Remember that a mole is equal to Avogadro's number: 6.022*10²³ atoms. Also, remember that an atom is made up of protons, neutrons, and electrons. Each element has a different amount of each.

If an element has more of these particles in 1 atom, then the atomic mass will be greater, ultimately making the molar mass (mass of 1 mole) greater.

Silicon has 14 protons, electrons, and neutrons, making its atomic mass 28.085 amu and its molar mass 28.085 grams. However, carbon only has 6 of each particle, so its atomic mass is smaller at 12.011 amu and molar mass is 12.011 grams.

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It is thought that Vitamin C might be an effective preventative

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4 years ago

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3 years ago

Read 2 more answers

When menthol, CH3OH, is burned in the presence of oxygen gas, O2, a large amount of heat energy is released. For this reason, it

Drupady [299]

We have the following balanced equation:

$CH_3OH_{(g)}+\frac{3}{2}O_{2\text{ (g)}}\rightarrow CO_{2\text{ (g)}}+2H_2O_{(l)}$

They also give us the heat of reaction equal to -764 kJ, i.e. it is an exothermic reaction.

By observing the reaction, we can deduce that for this heat to be generated, one mole of methanol is needed. Now let's see how many grams that mole of methanol equals. We will use the molecular weight equal to 32.04 g/mol

$\begin{gathered} g\text{ of methanol = 1 mol }\times\text{ 32.04 g/mol} \\ g\text{ of methanol }=\text{ 32.04 g} \end{gathered}$

Now we know the grams of methanol that generate 764 kJ, because the heat of reaction is directly proportional to the mass of the reactants, we can apply a rule of three to know the grams needed to produce a heat of reaction equal to 701 kJ:

$\begin{gathered} \frac{32.04\text{ g of methanol}}{764\text{ kJ}}=\text{ }\frac{x\text{ g of methanol}}{701\text{ kJ}} \\ x\text{ g of methanol = }\frac{32.04\text{ g of methanol }\times\text{ 701 kJ}}{764\text{ kJ}} \\ g\text{ of methanol = 29.4 g} \end{gathered}$

So, 29.4 g of methanol must be found to produce 701 kJ of heat

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1 year ago