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4 years ago

Which sample of matter is classified as a solution? 1. H2O(s) 2. H2O(l) 3. CO2(g) 4. CO2(aq)

Chemistry

2 answers:

Goshia [24]4 years ago

8 0

4. CO2(aq)

Because of the symbol aq, meaning aqueous, which means in solution.

lys-0071 [83]4 years ago

4 0

Answer : Option 4) $CO_{2}_{(aq)}$

Explanation : $CO_{2}_{(aq)}$ is the only sample of matter which can be classified as a solution. As the solution can be defined as a liquid mixture which contains a minor component (the solute) that is uniformly distributed within the major component (the solvent).

In this case, the solute is $CO_{2}$ which is dissolved in water which acts as an solvent. Also, it has a subscript which is aq. which means aqueous, is often given to the solution in which the solvent is water.

Therefore, $CO_{2}_{(aq)}$ is the correct answer.

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What is a planet smaller than earth

Elenna [48]

Answer:

Mercury, Venus, and Mars are all smaller than Earth, and technically Pluto a well.

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Explanation:

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3 years ago

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3. Methane (CH4) behaves as an ideal gas under standard temperature and pressure conditions. What volume is occupied by 1 kg of

AlekseyPX

Answer:

1711.11L

Explanation:

Given parameters:

Mass of methane = 1kg = 1000

Temperature of gas = 35°C

Pressure of the gas = 0.9atm

Converting to the temperature to kelvin, we have:

35+ 273 = 308k

Solution

From the given parameters, we can solve this problem using the ideal gas equation which is combination of the gas laws. It is expressed below:

PV = nRT .......................(i)

Where P is the pressure of the gas

V is the volume of the gas

n is the number of moles

R is the gas constant

T is the temperature

Now, from the above parameters, we have two unknowns which are n and V.

To find the number of moles n, we use the expression below:

number of moles = $\frac{mass}{molar mass}$

molar mass of methane = 12 + (4x1) = 16g/mol

Number of moels of methane = $\frac{1000}{16}$ = 62.5mole

Now that we know the number of moles, we can make the unknown Volume the subject of the formula:

V = $\frac{nRT}{P}$

V = $\frac{62.5 x 0.082 x 308}{0.9}$ = 1711.11L

7 0

3 years ago

Mercury(II) oxide (HgO) decomposes to form mercury (Hg) and oxygen (O2). The balanced chemical equation is shown below. 2HgO Rig

BigorU [14]

Taking into account the reaction stoichiometry, the correct answer is the third option: 15.63 moles of HgO are needed to produce 250 g of O₂.

In first place, the balanced reaction is:

2 HgO → 2 Hg + O₂

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

HgO: 2 moles
Hg: 2 moles
O₂: 1 moles

The molar mass of the compounds is:

HgO: 216.59 g/mole
Hg: 200.59 g/mole
O₂: 32 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

HgO: 2 moles× 216.59 g/mole= 433.18 grams
Hg: 2 moles× 200.59 g/mole= 401.18 grams
O₂: 1 mole× 32 g/mole= 32 grams

Then the following rule of three can be applied: if by reaction stoichiometry 32 grams of O₂ are produced by 2 moles of HgO, 250 grams of O₂ are produced from how many moles of HgO?

$moles of HgO=\frac{250 grams of O_{2} x2 moles of HgO}{32grams of O_{2}}$

moles of HgO= 15.625 moles≅ 15.63 moles

Finally, the correct answer is the third option: 15.63 moles of HgO are needed to produce 250 g of O₂.

Learn more about reaction stoichiometry:

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Answer:

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