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2 years ago

What is diatomic gas?

Chemistry

2 answers:

Anika [276]2 years ago

7 0

Molecules composed of only two atoms of the same or different chemical elements

Ann [662]2 years ago

3 0

Gases in which the molecules that make it up naturally consist of two atoms of the same type.

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A 17.11 gram sample of an organic compound containing only C, H, and O is analyzed by combustion analysis and 21.71 g CO2 and 5.

Andru [333]

Answer: The empirical formula and the molecular formula of the organic compound is $CHO$ and $C_4H_4O_4$ respectively.

Explanation:

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

$C_xH_yO_z+O_2\rightarrow CO_2+H_2O$

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

We are given:

Mass of $CO_2$ = 21.71 g

Mass of $H_2O$ = 5.926 g

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

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

So, in 21.71 g of carbon dioxide, = $\frac{12}{44}\times 21.71=5.921g$ of carbon will be contained.

For calculating the mass of hydrogen:

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

So, in 5.926 g of water, = $\frac{2}{18}\times 5.926=0.658g$ of hydrogen will be contained.

Mass of oxygen in the compound = (17.11) - (5.921+0.658) = 10.53 g

Mass of C = 5.921 g

Mass of H = 0.658 g

Mass of O = 10.53 g

Step 1 : convert given masses into moles.

Moles of C = $\frac{\text{ given mass of C}}{\text{ molar mass of C}}= \frac{5.921g}{12g/mole}=0.493moles$

Moles of H= $\frac{\text{ given mass of H}}{\text{ molar mass of H}}= \frac{0.658g}{1g/mole}=0.658moles$

Mass of O= $\frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{10.53g}{16g/mole}=0.658moles$

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For C = $\frac{0.493}{0.493}=1$

For H = $\frac{0.658}{0.493}=1$

For O= $\frac{0.658}{0.493}=1$

The ratio of C : H: O = 1: 1: 1

Hence the empirical formula is $CHO$ .

empirical mass of CHO = 12(1) + 1(1) + 1 (16) = 29

Molecular mass = 104.1 g/mol

$n=\frac{\text {Molecular mass}}{\text {Equivalent mass}}=\frac{104.1}{29}=4$

Thus molecular formula = $n\times {\text {Empirical formula}}=4\times CHO=C_4H_4O_4$

6 0

3 years ago

1. Given the following equation:

CaHeK987 [17]

Answer:

a. C₄H₁₀/O₂ = 2:13 (example)

b. O₂/CO₂ = 13:8

c. O₂/H₂O = 13:10

d. C₄H₁₀/CO₂ = 2:8

e. C₄H₁₀/H₂O = 2:10

Explanation:

2C₄H₁₀ + 13O₂ ⟶ 8CO₂ + 10H₂O

The molar ratios are the same as the coefficients in front of the formulas.

3 0

3 years ago

What does <br> the atomic mass tell you?

saveliy_v [14]

Answer:

how many protons and neutrons in its atoms

Explanation:

3 0

3 years ago

Read 2 more answers

What is the density of carbon dioxide gas if 2g occupies a volume of 10ml?

Thepotemich [5.8K]

Answer:

Molar mass=2×Vapour density

Given, Vapour Density=11.2

Molar mass=11.2×2=22.4g/mol

No.of moles of gas=

22.4

≅0.45moles

At STP, 1 mole occupies 22.4L volume.

0.45 moles occupy 22.4×0.45=10 L volume.

∴ Volume occupied is 10 litres.

Explanation:

4 0

2 years ago

In , the bonds cause the carbon chain to bend or "kink", which gives the molecules an irregular shape. as a result, acids cannot

Anuta_ua [19.1K]

Answer:ur mom

Explanation:

8 0

3 years ago