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3 years ago

Which choice can be a solid, liquid, or a gas?

1 answer:

3 0

I believe that your option C would be the correct answer. We know that water can turn to a solid materail because during cold temperatures, water turns to ice.

We know that water can turn to gas, as water can evaporate.

And also, we know that water is obviosly a liquid.

Therefore, Option C would be your answer.

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The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process.... In the first step, manganes

frez [133]

Answer : The mass of $MnCO_3$ required are, 35 kg

Explanation :

First we have to calculate the mass of $MnO_2$ .

The first step balanced chemical reaction is:

$2MnCO_3+O_2\rightarrow 2MnO_2+2CO_2$

Molar mass of $MnCO_3$ = 115 g/mole

Molar mass of $MnO_2$ = 87 g/mole

Let the mass of $MnCO_3$ be, 'x' grams.

From the balanced reaction, we conclude that

As, $(2\times 115)g$ of $MnCO_3$ react to give $(2\times 87)g$ of $MnO_2$

So, $xg$ of $MnCO_3$ react to give $\frac{(2\times 87)g}{(2\times 115)g}\times x=0.757xg$ of $MnO_2$

And as we are given that the yield produced from the first step is, 65 % that means,

$60\% \text{ of }0.757xg=\frac{60}{100}\times 0.757x=0.4542xg$

The mass of $MnO_2$ obtained = 0.4542x g

Now we have to calculate the mass of $Mn$ .

The second step balanced chemical reaction is:

$3MnO_2+4Al\rightarrow 3Mn+2Al_2O_3$

Molar mass of $MnO_2$ = 87 g/mole

Molar mass of $Mn$ = 55 g/mole

From the balanced reaction, we conclude that

As, $(3\times 87)g$ of $MnO_2$ react to give $(3\times 55)g$ of $Mn$

So, $0.4542xg$ of $MnO_2$ react to give $\frac{(3\times 55)g}{(3\times 87)g}\times 0.4542x=0.287xg$ of $Mn$

And as we are given that the yield produced from the second step is, 80 % that means,

$80\% \text{ of }0.287xg=\frac{80}{100}\times 0.287x=0.2296xg$

The mass of $Mn$ obtained = 0.2296x g

The given mass of Mn = 8.0 kg = 8000 g (1 kg = 1000 g)

So, 0.2296x = 8000

x = 34843.20 g = 34.84 kg = 35 kg

Therefore, the mass of $MnCO_3$ required are, 35 kg

4 0

3 years ago

Read 2 more answers

How do you balance AlC3+H2O➡️Al(OH)3+CH4?

Alex17521 [72]

Info: Al(oh)3 might be an improperly capitalized: Al(OH)3
Error: Some elements or groups in the reagents are not present in the products: O
Error: equation Al4C3+H2O=Al(oh)3+CH4 is an impossible reaction
Please correct your reaction or click on one of the suggestions below:
Al4C3 + H2O = Al(OH)3 + CH4

5 0

4 years ago

Explain why we must balance all chemical equations

enyata [817]

Answer:

The chemical equation needs to be balanced so that it follows the law of conservation of mass.

Explanation:

3 0

3 years ago

Read 2 more answers

What is the atomic number, mass number, element symbol, group number, and period number for oxygen?

yawa3891 [41]

Answer:

Atomic no. = 8

Mass no. = 16

Period no. = 2

Group no. = 6

4 0

3 years ago

10 POINTS.

enot [183]

There are a total of 40 valence electrons in the PCl5 Lewis structure. Remember when you draw the Lewis structure for PCl5 that Phosphorous (P) is in Period 3 on the Periodic table. This means that it can hold more than 8 valence electrons.

I hope this helps and please don't report

7 0

3 years ago