It is not advisable to wear clothes made of synthetic fiber while working near fire because?

Chemistry

1 answer:

Svetradugi [14.3K]3 years ago

8 0

Answer:

They catch fire very easily.

Explanation:

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How many moles of MgO can be made from 5 moles of Mg?<br> 2Mg + O2 -> 2MgO

kkurt [141]

Answer:

Explanation:

The expected product is MgO, so the 1-to-1 mole ratio Mg to O in the product is all that is required.

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How many moles of Fe2+ are there in a 2.0g sample that is 80% by mass of FeCl2?

KIM [24]

Answer:

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অনুপস্থিত: 80%

Explanation:

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2 years ago

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(part 1 of 3) Copper reacts with silver nitrate through a single replacement. If 1.29 g of silver are produced from the reaction

ale4655 [162]

Answer:

See explanation.

Explanation:

Hello there!

In this case, according to the described chemical reaction, we first write the corresponding equation to obtain:

$Cu+2AgNO_3\rightarrow 2Ag+Cu(NO_3)_2$

Thus, we proceed as follows:

Part 1 of 3: here, since the molar mass of silver and copper (II) nitrate are 107.87 and 187.55 g/mol respectively, and the mole ratio of the former to the latter is 2:1, we can set up the following stoichiometric expression:

$m_{Cu(NO_3)_2}=1.29gAg*\frac{1molAg}{107.87gAg}*\frac{1molCu(NO_3)_2}{2molAg}*\frac{187.55gCu(NO_3)_2}{1molCu(NO_3)_2} \\\\m_{Cu(NO_3)_2}=1.12gCu(NO_3)_2$

Part 2 of 3: here, the molar mass of copper is 63.55 g/mol and the mole ratio of silver to copper is 2:1, the mass of the former that was used to start the reaction was:

$m_{Cu}=1.29gAg*\frac{1molAg}{107.87gAg}*\frac{1molCu}{2molAg}*\frac{63.55gCu)_2}{1molCu} \\\\m_{Cu}=0.380gCu$