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r-ruslan [8.4K]

3 years ago

15

Ammonia and oxygen react to form nitrogen monoxide and water, like this:

1 answer:

olchik [2.2K]3 years ago

6 0

4NH3+5O2 <=>4NO + 6H2O

Using the definition of Kp, we have
Kp=(Pno^4*Ph2o^6)/(Pnh3^4*Po2^5)
where Pno=partial pressure of NO, etc.

The numerical value for a given temperature can be evaluated when the actual partial pressures are known.

You might be interested in

How much heat is required to melt 26.0 g of ice at its melting point?

MAXImum [283]

Answer:

Heat required to melt 26.0 g of ice at its melting point is 8.66 kJ.

Explanation:

Number of moles of water in 26 g of water: 26× $\frac{1}{18.02}$ moles

=1.44 moles

The enthalpy change for melting ice is called the entlaphy of fusion. Its value is 6.02 kj/mol.

we have relation as:

q = n × ΔH

where:

q = heat

n = moles

Δ H = enthalpy

So calculating we get,

q= 1.44*6.02 kJ

q= 8.66 kJ

We require 8.66 kJ of energy to melt 26g of ice.

8 0

3 years ago

The structure of an atom is

kirill115 [55]

Answer:

Atoms consist of three basic particles: protons, electrons, and neutrons. The nucleus (center) of the atom contains the protons (positively charged) and the neutrons (no charge). The outermost regions of the atom are called electron shells and contain the electrons (negatively charged).

5 0

3 years ago

Which of the following is the correct scientific notation for 0.000056?

svet-max [94.6K]

Hi,

$0.000056 = 5.6 \times {10}^{ - 5}$

Hope this helps.
r3t40

7 0

3 years ago

I need to solve for x in this equation<br><br> ln(760/630)=32/8.314(1/x-1/329.5)

Anuta_ua [19.1K]

X=0.031903 I think if you don’t know how to do this photo math would be a good thing for you

4 0

3 years ago

Various members of a class of compounds, alkenes, react with hydrogen to produce a corresponding alkane. Termed hydrogenation, t

Vitek1552 [10]

<u>Answer:</u> The mass of decane produced is $1.743\times 10^2g$

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ ......(1)

Mass of hydrogen gas = 2.45 g

Molar mass of hydrogen gas = 2 g/mol

Putting values in equation 1:, we get:

$\text{Moles of }H_2=\frac{2.45g}{2g/mol}=1.225mol$

The chemical equation for the hydrogenation of decene follows:

$C_{10}H_{20}(l)+H_2(g)\rightarrow C_{10}H_{22}(s)$

As, decene is present in excess. So, it is considered as an excess reagent.

Thus, hydrogen gas is a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

1 mole of hydrogen gas produces 1 mole of decane.

So, 1.225 moles of hydrogen gas will produce = $\frac{1}{1}\times 1.225=1.225mol$ of decane

Now, calculating the mass of decane by using equation 1, we get:

Moles of decane = 1.225 mol

Molar mass of decane = 142.30 g/mol

Putting values in equation 1, we get:

$1.225mol=\frac{\text{Mass of decane}}{142.30g/mol}\\\\\text{Mass of carbon dioxide}=(1.225mol\times 142.30g/mol)=174.3g=1.743\times 10^2g$

Hence, the mass of decane produced is $1.743\times 10^2g$

5 0

3 years ago