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UNO [17]
3 years ago
6

An ore sample with a mass of 92.3 g is found to contain 17.7% by mass iron. What mass of iron is contained in the ore?

Chemistry
1 answer:
JulsSmile [24]3 years ago
4 0

Answer:

19.18g of iron

Explanation:

To find the mass of iron, we simply find the amount of the ore in grammes that corresponds to 17.7% iron.

We can do this mathematically. We simply place the 17.7 over 100 and multiply by the total mass of the iron.

The mass of iron in the ore is thus: 17.7/100 * 92.3 = 19.18g

The ore simply contains a mass of 19.18g of iron

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Explanation:

Hello,

The law of mass action, allows us to know the required amounts, thus, for this chemical reaction it is:

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(c) Since no initial data is specified, we could establish the rate of the reaction as based of the law of mass action:

r=\frac{1}{-3} \frac{d[D]}{dt} =\frac{1}{-1} \frac{d[E]}{dt} =\frac{1}{-2} \frac{d[F]}{dt} =\frac{1}{5} \frac{d[G]}{dt} =\frac{1}{4} \frac{d[H]}{dt}

Thus, any of the available expressions are suitable to quantify the rate of the reaction.

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4 years ago
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the gas left in an used aerosol can is at a pressure of 103 kPa at 25 degrees celsius if this can be thrown into fire what is th
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Hello!

The pressure of the gas when it's temperature reaches 928 °C is 3823,36 kPa

To solve that we need to apply Gay-Lussac's Law. It states that the pressure of a gas when the volume is left constant (like in the case of a sealed container like an aerosol can) is proportional to temperature. This is the relationship derived from this law that we use to solve this problem:

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