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tensa zangetsu [6.8K]
3 years ago
15

for the reactants represented by the equation 2H2 + O2 > 2H2O, how many grams of water are produced from 376.97 mol of hydrog

en?
Chemistry
2 answers:
Hunter-Best [27]3 years ago
8 0

Answer:

6792.1 g

Explanation:

Dimensional analysis:

376.92 mol H2 * (2 mol h2o / 2 mol h2) * (18.02g h2o / 1 mol h2o)

6792.1 g

kirza4 [7]3 years ago
6 0

Answer:

Amount of water produced from 376.97 mole hydrogen is 6785.46 g

Explanation:

Given number of moles of hydrogen = 376.97 mole

The balanced reaction is shown below

2\textrm{H}_{2}\left ( g \right )+\textrm{O}_{2}\left ( g \right )\rightarrow 2\textrm{H}_{2}\textrm{O}\left ( l \right )

2 mole of water is produced from 2 mole of hydrogen gas according to the balanced reaction.

Number of moles of water produced by 376.97 mole hydrogen = 376.97 mole

Molar mass of water = 1 8 g/mol

\textrm{Amount of water produced} = \left ( 376.97 \textrm{ mole}\times 18\textrm{ g/mol} \right ) = 6785.46 \textrm{ g}

Amount of water produced = 6785.46 g

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Answer:

The two statements are all True for group 7 and 8 elements.

Explanation:

The Group 7 elements are known as the halogens. They are reactive non-metals and are always found in compounds with other elements. Chlorine, bromine and iodine are all halogens.

Chlorine, bromine and iodine are the three common Group 7 elements. Group 7 elements form salts when they react with metals. The term ‘halogen’ means 'salt former'.

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The density of a 3.37M MgCl2 (FW = 95.21) is 1.25 g/mL. Calulate the molality, mass/mass percent, and mass/volume percent. So fa
Dafna1 [17]

Answer : The molality, mass/mass percent, and mass/volume percent are, 0.0381 mole/Kg, 25.67 % and 32.086 % respectively.

Solution : Given,

Density of solution = 1.25 g/ml

Molar mass of MgCl_2 (solute) = 95.21 g/mole

3.37 M magnesium chloride means that 3.37 gram of magnesium chloride is present in 1 liter of solution.

The volume of solution = 1 L = 1000 ml

Mass of MgCl_2 (solute) = 3.37 g

First we have to calculate the mass of solute.

\text{Mass of }MgCl_2=\text{Moles of }MgCl_2\times \text{Molar mass of }MgCl_2

\text{Mass of }MgCl_2=3.37mole\times 95.21g/mole=320.86g

Now we have to calculate the mass of solution.

\text{Mass of solution}=\text{Density of solution}\times \text{Volume of solution}=1.25g/ml\times 1000ml=1250g

Mass of solvent = Mass of solution - Mass of solute = 1250 - 320.86 = 929.14 g

Now we have to calculate the molality of the solution.

Molality=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Mass of solvent}}=\frac{3.37g\times 1000}{95.21g/mole\times 929.14g}=0.0381mole/Kg

The molality of the solution is, 0.0381 mole/Kg.

Now we have to calculate the mass/mass percent.

\text{Mass by mass percent}=\frac{\text{Mass of solute}}{\text{Mass of solution}}\times 100=\frac{320.86}{1250}\times 100=25.67\%

The mass/mass percent is, 25.67 %

Now we have to calculate the mass/volume percent.

\text{Mass by volume percent}=\frac{\text{Mass of solute}}{\text{Volume of solution}}\times 100=\frac{320.86}{1000}\times 100=32.086\%

The mass/volume percent is, 32.086 %

Therefore, the molality, mass/mass percent, and mass/volume percent are, 0.0381 mole/Kg, 25.67 % and 32.086 % respectively.

8 0
3 years ago
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