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3 years ago

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Chemistry

1 answer:

GalinKa [24]3 years ago

6 0

Answer:

436.8 mmHg.

Explanation:

From the question given above, the following data were obtained:

Total pressure (Pₜ) = 0.93 atm

Pressure of N₂ (Pₙ₂) = 270 mmHg

Pressure of O₂ (Pₒ₂) =?

Next, we shall convert the total pressure to mmHg . This can be obtained as follow:

1 atm = 760 mmHg

Therefore,

0.93 atm = 0.93 × 760 mmHg / 1 atm

0.93 atm = 706.8 mmHg

Finally, we shall determine the pressure of the O₂. This can be obtained as follow:

Total pressure (Pₜ) = 706.8 mmHg

Pressure of N₂ (Pₙ₂) = 270 mmHg

Pressure of O₂ (Pₒ₂) =?

Pₜ = Pₙ₂ + Pₒ₂

706.8 = 270 + Pₒ₂

Collect like terms

706.8 – 270 = Pₒ₂

436.8 = Pₒ₂

Pₒ₂ = 436.8 mmHg

Thus, the pressure of O₂ is 436.8 mmHg

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List the following aqueous solutions in order of increasing boiling point: 0.12 m C6H12O6, 0.05 m LiBr, and 0.05 m Zn(NO3)2. Exp

GalinKa [24]

Answer: The order of increasing boiling points follows:

$\text{LiBr }$

Explanation:

The expression of elevation in boiling point is given as:

$\Delta T_b=i\times k_b\times m$

where,

$\Delta T_b$ = Elevation in boiling point

i = Van't Hoff factor

$T_b$ = change in boiling point

$k_b$ = boiling point constant

m = molality

For the given options:

Option 1: 0.12 m $C_6H_{12}O_6$

Value of i = 1 (for non-electrolytes)

So, molal concentration will be = $(0.12)\times 1=0.12m$

Option 2: 0.02 m LiBr

Value of i = 2

So, molal concentration will be = $(0.02)\times 2=0.04m$

Option 3: 0.05 m $Zn(NO_3)_2$

Value of i = 3

So, molal concentration will be = $(0.05)\times 3=0.15m$

As, the molal concentration of $Zn(NO_3)_2$ is the highest, so its boiling point will be the highest.

Hence, the order of increasing boiling points follows:

$\text{LiBr }$

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3 years ago

How many electrons are in na+1

andrew11 [14]

Answer:

Explanation:

Sodium has 11 electrons when it is neutral. This sodium isn't neutral, it has a +1 charge. The +1 charge means it has lost 1 electron.

11 - 1 = 10

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3 years ago

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How many liters are there in 144g of H₂O (g)? What is the mass of 200L at STP of H₂O₂ (g)?

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Answer:

1. 179.2 L

2. 303.62 g

Explanation:

1. Determination of volume of H₂O (g).

We'll begin by calculating the number of mole in 144 g of H₂O. This is illustrated below:

Mass of H₂O = 144 g

Molar mass of H₂O = (2×1) + 16 = 2 + 16 = 18 g/mol

Mole of H₂O =?

Mole = mass /Molar mass

Mole of H₂O = 144/18

Mole of H₂O = 8 moles

Finally, we shall determine volume of H₂O (g) as follow:

1 mole of any gas occupy 22.4L at stp.

Therefore, 8 moles of H₂O (g) will occupy =

8 × 22.4 = 179.2 L

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2. Determination of the mass of H₂O₂ (g).

We'll begin by calculating the number of mole of H₂O₂ (g) that occupied 200 L at STP. this can be obtained as follow:

1 mole of any gas occupy 22.4 L at stp.

Therefore, Xmol of H₂O₂ (g) will occupy 200 L at STP i.e

Xmol of H₂O₂ (g) = 200/22.4

Xmol of H₂O₂ (g) = 8.93 moles

Thus, 8.93 moles of H₂O₂ (g) occupied 200 L at STP.

Finally, we shall determine the mass of H₂O₂ (g) as follow:

Mole of H₂O₂ (g) = 8.93 moles

Molar mass of H₂O₂ = (2×1) + (2×16) = 2 + 32 = 34 g/mol

Mass of H₂O₂ =?

Mole = mass /Molar mass

8.93 = mass of H₂O₂ /34

Cross multiply

Mass of H₂O₂ = 8.93 × 34

Mass of H₂O₂ = 303.62 g

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Answer:

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Explanation:

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4 years ago

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