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1 year ago

15

What types of mixtures are these? a cup of tea and sugar peanuts and almonds mixed together in a bowl a bucket full of sand and

gravel food coloring dissolved in water

1 answer:

Allushta [10]1 year ago

3 0

Answer:

The answer to your question is below

Explanation:

There are two kinds of mixtures

- Homogeneous is a mixture of two or more elements or compounds and its components can not be distinguished visually.

- Heterogeneous is a mixture of two or more elements or compounds and its components can be distinguished visually.

a cup of tea and sugar homogeneous

peanuts and almonds mixed together in a bowl heterogeneous

a bucket full of sand and gravel heterogeneous

food coloring dissolved in water homogeneous

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A chemist has 2.0 mol of methanol (CH3OH). The molar mass of methanol is 32.0 g/mol. What is the mass, in grams, of the sample?

rodikova [14]

Answer:

$\boxed {\boxed {\sf D. \ 64 \ grams }}$

Explanation:

Given the moles, we are asked to find the mass of a sample.

We know that the molar mass of methanol is 32.0 grams per mole. We can use this number as a fraction or ratio.

$\frac{32 \ g \ CH_3OH}{1 \ mol \ CH_3OH}$

Multiply by the given number of moles, which is 2.0

$2.0 \ mol \ CH_3OH *\frac{32 \ g \ CH_3OH}{1 \ mol \ CH_3OH}$

The moles of methanol will cancel each other out.

$2.0 \ *\frac{32 \ g \ CH_3OH}{1 }$

The denominator of 1 can be ignored.

$2.0 * 32 \ g\ CH_3OH$

Multiply.

$64 \ g \ CH_3OH$

There are 64 grams of methanol in the sample.

3 0

2 years ago

Use average bond energies to calculate ΔHrxn for the following hydrogenation reaction: H2C=CH2(g)+H2(g)→H3C−CH3(g)

marissa [1.9K]

Answer:

The $\Delta H_{rxn}$ of the given reaction is -129.6 kJ

Explanation:

The given chemical reaction is as follows.

$H_{2}C=CH_{2}(g)+H_{2}(g)\rightarrow H_{3}C-CH_{3}(g)$

Enthalpy of each reactant and products are as follows.

$\Delta H_{C=C}\,=615.0\,kJ\,mol^{-1}$

$\Delta H _{H-H}\,=435.1\,kJ\,mol^{-1}$

$\Delta H _{C-C}\,=347.3\,kJ\,mol^{-1}$

$\Delta H _{C-H}\,=416.2\,kJ\,mol^{-1}$

In the given chemical reaction involved two C-H bonds in the reactant side and one C-C bond in the product side therefore, the enthalpy of formation will be the negative.

$\Delta H_{rxn}=-\Delta H_{C-C}-2\Delta H_{C-H}+\Delta H_{C=C}+\Delta H_{H-H}$

$=-347.4-2\times416.2+615.0+435.1$

$=-129.6 \,kJ$

Therefore, The $\Delta H_{rxn}$ of the given reaction is -129.6 kJ

4 0

1 year ago

Which of the following molecules can form hydrogen bonds?

frosja888 [35]

Hydrogen bonding is a type of intermolecular forces of attraction in which hydrogen atom is bonded to one of the most electronegative atoms. This gives a partial positive charge to hydrogen atom and a partial negative charge to the electronegative atom involved in the bonding. The electronegative atoms that can form hydrogen bonding are fluorine (F), nitrogen (N), and oxygen (O).

Therefore the correct option is,

A) NH3

3 0

1 year ago

A 0.133 mol sample of gas in a 525 ml container has a pressure of 312 torr. The temperature of the gas is ________ °c.

Serggg [28]

Answer:

$-253.2 ^{\circ}C$

Explanation:

First of all, we need to convert the pressure of the gas from torr to Pa. We know that:

1 torr = 133.3 Pa

So, the pressure in Pascals is

$p=(312 torr)(133.3 Pa/torr)=4.16\cdot 10^4 Pa$

Then we also have:

n = 0.133 number of moles of the gas

$V=525 mL=0.525 L=5.25\cdot 10^{-4} m^3$ volume of the gas

The ideal gas equation states that

$pV=nRT$

where R is the gas constant and T the absolute temperature. Solving the equation for T, we find

$T=\frac{pV}{nR}=\frac{(4.16\cdot 10^4 Pa)(5.25\cdot 10^{-4} m^3)}{(0.133 mol)(8.314 J/mol K)}=19.8 K$

In Celsius, it becomes

$T=19.8 K-273=-253.2 ^{\circ}C$

3 0

1 year ago

For the reaction 2Fe+3Cl2=2FeCl3

Butoxors [25]

The question is incomplete but the full question may be found in other sources.

This is the complete question:

For the reaction 2Fe + 3Cl₂ → 2FeCl₃ which option is more accurate?

a. FeCl₃, reducing agent; Fe, oxidizing agent.

b. Cl₂, oxidising agent; Fe reducing agent.

c. Fe, reducing agent; FeCl₃, oxidizing agent.

d. FeCl₃, oxidizing agent, Cl₂, reducing agent.

Answer:

<em><u>Option b. Cl₂, oxidising agent; Fe reducing agent.</u></em>

Explanation:

It is easy to recognize by simple inspection that the given reaction is a redox one (oxidation - reduction) because the substances in the reactant side are pure elements (whose oxidation state is always zero) and the substance in the product side is a compound formed by the two reactant elements (which means that now they have a different oxidation state).

In a redox reaction, <u>the element that increases its oxidation number</u> loses electrons and reduces other element, so this <u>is the reducing agent</u>. On the other hand, <u>the element whose oxidation number is decreased</u> has gained electrons, a so it <u>is the oxidizing agent</u> (it oxidizes other element).

I will show the oxidation states of each species in the chemical reaction, using superscripts:

Fe⁰ + 3Cl₂⁰ → 2 Fe⁺³Cl₃⁻¹

Thus:

2 atoms of Fe increased their oxidation number from 0 to +3; meaning that they lost 6 electrons (3 electrons each), so Fe is the reducing agent (it reduced the Cl atoms).

6 atoms of Cl decreased their oxidation number from 0 to -1; meaning that they gained 6 electrons in total (1 elecron each), so Cl is the oxidizing agent (it oxidized the Fe atoms).

6 0

2 years ago