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3 years ago

I don’t know if it’s that one or not

Chemistry

1 answer:

Sphinxa [80]3 years ago

3 0

Answer:

I think is the last one.

Anthracite – Stage Four

Anthracite, the fourth stage in coal formation, is also known as “hard coal” because it is hard and has a high lustre. It appears to have been formed as a result of combined pressure and high temperature. Anthracite burns with a short flame and little smoke.

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What is the mass of 3.2 moles of h2O ?

Arturiano [62]

Answer:

$\boxed{\text{57.7 g} }$

Explanation:

The first step is to calculate the molar mass of H₂O:

$\begin{array}{rcr}\text{2 H} & = & 2.02\\\text{1 O} & = & 16.00\\\text{TOTAL} & = & \mathbf{18.02}\\\end{array}$

So, 1 mol has a mass of 18.02 g.

Next you calculate the mass of 3.2 mol of H₂O

$\begin{array}{rcl}m & = & \text{3.2 mol H$_{2}$O} \times \dfrac{\text{18.02 g H$_{2}$O}}{\text{1 mol H$_{2}$O}}\\ & = &\boxed{\textbf{57.7 g H$_{2}$O}} \\\end{array}$

6 0

3 years ago

Please help with this , thanks you very much

netineya [11]

Explanation:

reaction A is exothermic reaction as a substance is produced from two substances

and

reaction B is endothermic as two substances are formed from one complex structure

7 0

3 years ago

Look at the image shown

klemol [59]

Answer:

b) Linear molecule with two domains

Explanation:

The image represents a linear molecule with two domains.

The compound shown here is carbon dioxide in which a central carbon atom is surrounded by two oxygen atoms.

This bond geometry is of the type AX₂
In this linear molecule the bond angle is a perfect 180°
The lone pairs are perfectly balanced out and will not cause distortion of the central carbon.

5 0

3 years ago

How to do my homework? i’ll give 20 points to anyone who will do it!

tensa zangetsu [6.8K]

what is it ??? ill edit this

3 0

3 years ago

Read 2 more answers

Consider the combustion reaction for octane (C8H18), which is a primary component of gasoline.

lesya692 [45]

Answer:

$n_{CO_2}=1.93 gCO_2$

Explanation:

Hello,

In this case, considering the given chemical reaction, we can use the molar mass of octane (114.23 g/mol) and the 2:16 molar ratio with carbon dioxide to compute the emitted moles of CO2 to the atmosphere via the following stoichiometric procedure:

$n_{CO2}=27.6gC_8H_{18}*\frac{1molC_8H_{18}}{114.23gC_8H_{18}} *\frac{16molCO_2}{2molC_8H_{18}} \\\\n_{CO_2}=1.93 gCO_2$

Which also corresponds to the following mass:

$m_{CO_2}=1.93molCO_2*\frac{44gCO_2}{1molCO_2} \\\\m_{CO_2}=85.0gCO_2$

Best regards.

6 0

3 years ago