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3 years ago

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Chemistry

1 answer:

Korvikt [17]3 years ago

5 0

1) $CO (g) + 2H_{2}(g) ---> CH_{3}OH (g)$

Moles of methanol = $208 kg CH_{3}OH * \frac{1000 g}{1 kg} * \frac{1 mol CH_{3}OH}{32.04 g CH_{3}OH} = 6492 mol CH_{3}OH$

Mass of $H_{2}$ that would produce 208 kg methanol =

$6492 mol CH_{3}OH * \frac{2 mol H_{2}}{1 mol CH_{3}OH} * \frac{2.02 g H_{2}}{1 mol H_{2}} * \frac{1 kg}{1000 g}= 26.2 kg H_{2}$

2) Mass of sodium = $1.3 * 10^{21} atoms Na * \frac{1 mol Na}{6.022* 10^{23}atoms Na} * \frac{22.99 g Na}{1 mol Na} = 0.0496 g Na$

3) Mass of mercury = $1.2 mL * 13.6 \frac{g}{mL} = 16.32 g$

Number of atoms of mercury = $16.32 g Hg * \frac{1 mol Hg}{200.59 g Hg} * \frac{6.022* 10^{23} atoms Hg}{1 mol Hg} = 4.9 * 10^{22} atoms Hg$

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Need help asap with this chemistry if someone could help me

Burka [1]

Answer:

Structure One:

N: -2
C: 0
O: +1

Structure Two:

N: 0
C: 0
O: -1

Structure Three:

N: -1
C: 0
O: 0.

Structure Number Two would likely be the most stable structure.

All five C atoms: 0
All six H atoms to C: 0
N atom: +1.

The N atom is the one that is "likely" to be attracted to an anion. See explanation.

Explanation:

When calculating the formal charge for an atom, the assumption is that electrons in a chemical bond are shared equally between the two bonding atoms. The formula for the formal charge of an atom can be written as:

$\text{Formal Charge} \\ = \text{Number of Valence Electrons in Element} \\ \phantom{=}-\text{Number of Chemical Bonds} \\\phantom{=} - \text{Number of nonbonding Lone Pair Electrons}$ .

For example, for the N atom in structure one of the first question,

N is in IUPAC group 15. There are 15 - 10 = 5 valence electrons on N.
This N atom is connected to only 1 chemical bond.
There are three pairs, or 6 electrons that aren't in a chemical bond.

The formal charge of this N atom will be $5 - 1 - 6 = -2$ .

Apply this rule to the other atoms. Note that a double bond counts as two bonds while a triple bond counts as three.

Structure One:

N: -2
C: 0
O: +1

Structure Two:

N: 0
C: 0
O: -1

Structure Three:

N: -1
C: 0
O: 0.

In general, the formal charge on all atoms in a molecule or an ion shall be as close to zero as possible. That rules out Structure number one.

Additionally, if there is a negative charge on one of the atoms, that atom shall preferably be the most electronegative one in the entire molecule. O is more electronegative than N. Structure two will likely be favored over structure three.

Similarly,

All five C atoms: 0
All six H atoms to C: 0
N atom: +1.

Assuming that electrons in a chemical bond are shared equally (which is likely not the case,) the nitrogen atom in this molecule will carry a positive charge. By that assumption, it would attract an anion.

Note that in reality this assumption seldom holds. In this ion, the N-H bond is highly polarized such that the partial positive charge is mostly located on the H atom bonded to the N atom. This example shows how the formal charge assumption might give misleading information. However, for the sake of this particular problem, the N atom is the one that is "likely" to be attracted to an anion.

5 0

3 years ago

a 2.7 L of N2 is collected at 121kpa and 288 K . if the pressure increases to 202 kpa and the temperature rises to 303 K , what

jok3333 [9.3K]

Answer:

The gas will occupy a volume of 1.702 liters.

Explanation:

Let suppose that the gas behaves ideally. The equation of state for ideal gas is:

$P\cdot V = n\cdot R_{u}\cdot T$ (1)

Where:

$P$ - Pressure, measured in kilopascals.

$V$ - Volume, measured in liters.

$n$ - Molar quantity, measured in moles.

$T$ - Temperature, measured in Kelvin.

$R_{u}$ - Ideal gas constant, measured in kilopascal-liters per mole-Kelvin.

We can simplify the equation by constructing the following relationship:

$\frac{P_{1}\cdot V_{1}}{T_{1}} = \frac{P_{2}\cdot V_{2}}{T_{2}}$ (2)

Where:

$P_{1}$ , $P_{2}$ - Initial and final pressure, measured in kilopascals.

$V_{1}$ , $V_{2}$ - Initial and final volume, measured in liters.

$T_{1}$ , $T_{2}$ - Initial and final temperature, measured in Kelvin.

If we know that $P_{1} = 121\,kPa$ , $P_{2} = 202\,kPa$ , $V_{1} = 2.7\,L$ , $T_{1} = 288\,K$ and $T_{2} = 303\,K$ , the final volume of the gas is:

$V_{2} = \left(\frac{T_{2}}{T_{1}} \right)\cdot \left(\frac{P_{1}}{P_{2}} \right)\cdot V_{1}$

$V_{2} = 1.702\,L$

The gas will occupy a volume of 1.702 liters.

6 0

3 years ago

Antoine put some metal into a container with air. He closed the container. He measured the weight of the closed container with t

Mandarinka [93]

Answer:

the same

Explanation:

due to the law of conservation of mass, the mass will not change

7 0

3 years ago

What determines the order of placement of the elements on the modern Periodic Table?

Pachacha [2.7K]

The order of placement of the elemnts on the modern Periodic Table is determinated by:
1)atomic number (Z=number of protons).

3 0

3 years ago

Read 2 more answers

When chlorobenzene reacts with Mg in ether followed by CO2 and neutralization with dilute HCl, __________ will be formed.

allsm [11]

Answer:

c. benzoic acid

Explanation:

The given reaction is an example of a Grignard reaction:

When chlorobenzene (C₆H₅Cl) reacts with Mg in ether, an intermediate is formed (C₆H₅MgCl).

Said intermediate then reacts with CO₂ producing a benzoic acid salt (C₆H₅CO₂X), this salt is then neutralized with dilute HCl producing benzoic acid (C₆H₅CO₂H).

4 0

3 years ago