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stepan [7]
2 years ago
11

How many moles of carbon dioxide can be formed by the decomposition of 5.0 moles of aluminium carbonate

Chemistry
1 answer:
Ksenya-84 [330]2 years ago
3 0

Answer:

30 moles of CO₂

Explanation:

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What is the major product of this reaction? which reaction sequence would provide the highest yield of 1 -bromo-2-mcihylcyclohex
Aleonysh [2.5K]
Of which reaction may I ask? And do you mean 1-bromo-2-methylcyclohexane??
3 0
3 years ago
Carbon dioxide in the atmosphere dissolves in raindrops to produce carbonic acid (H2CO3), causing the pH of clean, unpolluted ra
anastassius [24]

Answer:

The range of [H⁺] is from 2.51 x 10⁻⁶ M to 6.31 x 10⁻⁶ M,

Explanation:

To answer this problem we need to keep in mind the <u>definition of pH</u>:

  • pH = -log [H⁺]

So now we <u>calculate [H⁺] using a pH value of 5.2 and of 5.6</u>:

  • 5.2 = -log [H⁺]

-5.2 = log [H⁺]

10^{-5.2} = [H⁺]

6.31 x 10⁻⁶ M = [H⁺]

  • 5.6 = -log [H⁺]

-5.6 = log [H⁺]

10^{-5.6} = [H⁺]

2.51 x 10⁻⁶ M = [H⁺]

6 0
3 years ago
How many grams of lead(II) sulfate (303 g/mol) are needed to react with sodium chromate (162 g/mol) in order to produce 0.162 kg
Afina-wow [57]

Answer : The mass of PbSO_4 needed are, 1.515 grams.

Explanation :

First we have to calculate the mole of PbCrO_4.

\text{Moles of }PbCrO_4=\frac{\text{Mass of }PbCrO_4}{\text{Molar mass of }PbCrO_4}=\frac{0.162g}{323g/mole}=0.005mole

Now we have to calculate the moles of PbSO_4.

The balanced chemical reaction will be,

PbSO_4+Na_2CrO_4\rightarrow PbCrO_4+Na_2SO_4[tex]From the balanced chemical reaction, we conclude thatAs, 1 mole of [tex]PbCrO_4 produced from 1 mole of PbSO_4

So, 0.005 mole of PbCrO_4 produced from 0.005 mole of PbSO_4

Now we have to calculate the mass of PbSO_4

\text{Mass of }PbSO_4=\text{Moles of }PbSO_4\times \text{Molar mass of }PbSO_4

\text{Mass of }PbSO_4=0.005mole\times 303g/mole=1.515g

Therefore, the mass of PbSO_4 needed are, 1.515 grams.

6 0
3 years ago
How many grams of iron oxide, Fe2O3 will be produced if 165 g of O2 gas is supplied? (follow the same steps as mol to mol, only
forsale [732]

Answer:

m_{Fe_2O_3}=549gFe_2O_3

Explanation:

Hello there!

In this case, according to the given chemical reaction for this problem about stoichiometry:

4Fe+3O_2\rightarrow 2Fe_2O_3

Whereas there is a 3:2 mole ratio of oxygen (molar mass = 32.0 g/mol) to iron (III) oxide (molar mass = 159.69 g/mol) and therefore, the correct stoichiometric setup is:

m_{Fe_2O_3}=165gO_2*\frac{1molO_2}{32.00gO_2}*\frac{2molFe_2O_3}{3molO_2} *\frac{159.69gFe_2O_3}{1molFe_2O_3}  \\\\m_{Fe_2O_3}=549gFe_2O_3

Regards!

8 0
3 years ago
Can someone plz help me with this one problem plzzzzz I’m being timed!!!
poizon [28]

Answer:

answer : the penguins do

4 0
3 years ago
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