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3 years ago

4 NH3 +5 02 +4NO + 6H2O When 70.25 grams of NH3 react, how many moles of H20 are produced?

Chemistry

1 answer:

romanna [79]3 years ago

5 0

Answer:

6.19 mol H₂O

Explanation:

4 NH₃ + 5O₂ → 4NO + 6H₂O

First, we convert 70.25 grams of NH₃ into moles, using its molar mass:

70.25 g ÷ 17 g/mol = 4.13 mol NH₃

Then we convert 4.13 moles of NH₃ into moles of H₂O, using the stoichiometric coefficients of the balanced reaction:

4.13 mol NH₃ * $\frac{6molH_2O}{4molNH_3}$ = 6.19 mol H₂O

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How many seconds are in an exactly 40-hour work week?

Elza [17]

7 days = 1 week 60 seconds = 1 minute.
40 hr 60 min 60 sec = 144,000 s.
The answer is 144,000 seconds hopes this helps :)

4 0

3 years ago

Read 2 more answers

5. Azulene is a beautiful blue hydrocarbon. If 0.106 g of the compound is burned in oxygen, 0.364 g of CO2 and 0.0596 g of H2O a

max2010maxim [7]

Answer: The empirical and molecular formula for the given organic compound is CH and $C_{10}H_{10}$ and it is not an alkane.

Explanation:

The chemical equation for the combustion of hydrocarbon having carbon and hydrogen follows:

$C_xH_y+O_2\rightarrow CO_2+H_2O$

where, 'x' and 'y' are the subscripts of Carbon, hydrogen and oxygen respectively.

We are given:

Mass of $CO_2=0.364g$

Mass of $H_2O=0.0596g$

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 0.364 g of carbon dioxide, $\frac{12}{44}\times 0.364=0.0993g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18 g of water, 2 g of hydrogen is contained.

So, in 0.0596 g of water, $\frac{2}{18}\times 0.0596=0.0067g$ of hydrogen will be contained.

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{0.0993g}{12g/mole}=0.00828moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.0067g}{1g/mole}=0.0067moles$ ]

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.0067 moles.

For Carbon = $\frac{0.00828}{0.0067}=1.23\approx 1$

For Hydrogen = $\frac{0.0067}{0.0067}=1$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H = 1 : 1

The empirical formula for the given compound is CH

For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is:

$n=\frac{\text{Molecular mass}}{\text{Empirical mass}}$

We are given:

Mass of molecular formula = 128.2 g/mol

Mass of empirical formula = 13 g/mol

Putting values in above equation, we get:

$n=\frac{128.2g/mol}{13g/mol}=9.86\approx 10$

Multiplying this valency by the subscript of every element of empirical formula, we get:

$C_{(1\times 10)}H_{(1\times 10)}=C_{10}H_{10}$

The general formula of an alkane is $C_nH_{(2n+2)}$ , where n = any natural number

Here, n = 10 and it does not satisfy being an alkane

Hence, the empirical and molecular formula for the given organic compound is CH and $C_{10}H_{10}$ and it is not an alkane.

7 0

3 years ago

34 atoms of carbon (C) react with 22 molecules of hydrogen gas (H2). How many molecules of methane (CH4) will be formed, and wha

kolbaska11 [484]

Answer:

11 molecules of CH4.

23 atoms of C is the leftover.

Explanation:

Hello!

In this case, for the formation of methane:

$C+2H_2\rightarrow CH_4$

We can see there is an excess of carbon based on their stoichiometry, because the needed amount of hydrogen gas molecules would be:

$molecules _{H_2}=34atomC*\frac{2molec\ H_2}{1atomC} =68molec\ H_2$

Thus, the formed molecules of methane are computed below:

$molec\ CH_4=22molec\ H_2 *\frac{1molec\ CH_4}{2molmolec\ H_2} \\\\molec\ CH_4=11molec\ CH_4$

In such a way, the leftover of carbon atoms are:

$atoms \ C^{left over}=34-22molec\ H_2*\frac{1atoms C}{2molec\ H_2} \\\\atoms \ C^{left over}=23 atoms C$

Best regards!

4 0

3 years ago

7.no . with steps please anyone no spam

gulaghasi [49]

Given mass=1.3g
Atomic mass=65u

Molar mass=65g/mol

Now

$\boxed{\sf No\:of\:moles=\dfrac{Given\:Mass}{Molar\:Mass}}$

$\\ \rm\longmapsto No\:of\;Moles=\dfrac{1.3}{65}=0.02mol$

6 0

3 years ago

Hydrocarbons do not dissolve in concentrated sulfuric acid, but methyl benzoate does. Explain this difference and write an equat

finlep [7]

Answer:

See explanation

Explanation:

For a substance to dissolve in another, there must be some sort of interaction between the substances.

Recall that like dissolves like. That is, polar substances dissolve polar substances and non polar substances dissolve nonpolar substances.

Hydrocarbons are nonpolar hence they do not dissolve in polar sulphuric acid. Methyl benzoate is polar hence it dissolve in polar sulphuric acid.

The equation showing the ions is depicted in the image attached to this answer.

7 0

3 years ago