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3 years ago

How many atoms are in one molecule of dinitrogen pentoxide

Chemistry

1 answer:

Reptile [31]3 years ago

4 0

Explanation:

As the name suggests, a single molecule of Dinitrogen Pentoxide will have 2 (di) nitrogen atoms and 5 (Pent) oxygen atoms.

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One liter of air contains about 0.21 L of oxygen. When filled, the human lungs hold about 6.0 L of air. How much oxygen is in th

Pie

Simple 6L of air times the .21L of O2 = 1.26

3 0

3 years ago

If a mixture of gases contained 78% nitrogen at a pressure of 984 torr and 22% carbon dioxide at 345 torr, what is the total pre

AysviL [449]

Answer:

P(total) = 1329 torr

Explanation:

Given data:

Pressure of nitrogen = 984 torr

Pressure of carbon dioxide = 345 torr

Total pressure of system = ?

Solution:

The given problem will be solve through the Dalton law of partial pressure of gases.

According to the this law,

The total pressure exerted by the mixture of gases is equal to the sum of partial pressure of individual gas.

Mathematical expression,

P(total) = P₁ + P₂ +.......+ Pₙ

Here we will put the values in formula,

P₁ = partial pressure of nitrogen

P₂ = partial pressure of carbon dioxide

P(total) = 984 torr + 345 torr

P(total) = 1329 torr

8 0

3 years ago

Which statement best describes the equation given: C2H6+CL2-> C2H5CL+HCl

agasfer [191]

Answer:

substitution involving a saturated hydrocarbon

Explanation:

3 0

3 years ago

What is true valence electrons?

dangina [55]

Answer:

Energy level where all chemical reactions occur. The remaining electrons are 'core' electrons that do not react.

Explanation:

6 0

3 years ago

Acetic acid (CH3COOH) is formed from its elements by the following reaction equation:

Alecsey [184]

Answer:

111 L

Explanation:

Calculation of moles of hydrogen gas:-

Mass of $H_2$ = 18.6 g

Molar mass of $H_2$ = 2.01588 g/mol

$Moles=\frac{Mass}{Molar\ mass}=\frac{18.6}{2.01588}\ mol=9.23\ mol$

According to the given reaction:-

$2C+2H_2+O_2\rightarrow CH_3COOH$

2 moles of hydrogen gas on reaction produces one mole of acetic acid gas.

So,

1 mole of hydrogen gas on reaction produces $\frac{1}{2}$ mole of acetic acid gas.

Also,

9.23 mole of hydrogen gas on reaction produces $\frac{1}{2}\times 9.23$ mole of acetic acid gas.

Moles of acetic acid gas = 4.615 moles

Given that:

Temperature = 35 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15

So,

T = (35 + 273.15) K = 308.15 K

n = 4.615 moles

P = 1.05 atm

V = ?

Using ideal gas equation as:

$PV=nRT$

where,

P is the pressure

V is the volume

n is the number of moles

T is the temperature

R is Gas constant having value = 0.0821 L atm/ K mol

Applying the equation as:

1.05 atm × V = 4.615 moles ×0.0821 L atm/ K mol × 308.15 K

3 0

4 years ago