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netineya [11]
3 years ago
5

Element

Chemistry
1 answer:
Svetllana [295]3 years ago
7 0

Answer:

Number of moles = 10.6 mol

Explanation:

Given data:

Molar mass of H = 1.008 g/mol

Molar mass of C = 12.01 g/mol

Molar mass of O = 16.00 g/mol

Mass of citric acid = 2.03 kg (2.03×1000 = 2030 g)

Number of moles of citric acid = ?

Solution:

Formula:

Number of moles = mass/molar mass

Now we will calculate the molar mass of citric acid:

C₆H₈O₇ = (12.01× 6) + (1.008×8) + (16.00×7)

C₆H₈O₇ = 72.06 + 8.064+112

C₆H₈O₇ = 192.124g/mol

Number of moles = 2030 g/ 192.124g/mol

Number of moles = 10.6 mol

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Identify limiting and excess reagents when 25g of nitrogen reacts with 25g of hydrogen. How many grams of ammonia gas are formed
Makovka662 [10]

Answer:

Nitrogen is limiting reactant while hydrogen is in excess.

Explanation:

Given data:

Mass of N₂ = 25 g

Mass of H₂ = 25 g

Mass of ammonia formed = ?

Solution:

Chemical equation:

N₂ + 3H₂    →     2NH₃

Number of moles of Nitrogen:

Number of moles = mass/ molar mass

Number of moles = 25 g/ 28 g/mol

Number of moles = 0.89 mol

Number of moles of hydrogen:

Number of moles = mass/ molar mass

Number of moles = 25 g/ 2 g/mol

Number of moles = 12.5 mol        

Now we will compare the moles of both reactant with ammonia.

                   H₂            ;             NH₃

                    3             :              2

                    12.5        :            2/3×12.5 = 8.3

                 

                   N₂            ;             NH₃

                    1              :              2

                    0.89        :            2×0.89 = 1.78

The number of moles of ammonia produced by nitrogen are less thus nitrogen is limiting reactant while hydrogen is in excess.

7 0
3 years ago
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CHEM HELP ASAP!! <br><br> What mass of H2 would be needed to produce 208 kg of methanol?
Eddi Din [679]

So if we use the equation:

CO+2H_{2} → CH_{3}OH

We can then determine the amount of H_{2} needed to produce 208 kg of methanol.

So let's find out how many moles of methanol 208 kg is:

Methanol molar weight = 32.041g/mol

So then we can solve for moles of methanol:

208kg*\frac{1,000g}{1kg} *\frac{1mol}{32.041g} =6,491.68mol

So now that we have the amount of moles produced, we can use the molar ratio (from the balanced equation) of hydrogen and methanol. This ratio is 2:1 hydrogen:methanol.

Therefore, we can set up a proportion to solve for the moles of hydrogen needed:

\frac{2}{1} =\frac{x}{6,491.68}

x=12,983.36mol

So now that we have the number of moles of H_{2} that are produced, we can then use the molar weight of hydrogen to solve for the mass that is needed:

12,983.36mol*\frac{2.016g}{1mol} =26,174.45g_H_{2}

Therefore, the amount of diatomic hydrogen (H_{2}) that is needed to produce 208kg of methanol is 2.62x10^{4}g.

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