Can someone answer 1<br> For me please?

2. You have 200g or a solution that contains 30g of hydrochloric acid (HCI),

alex41 [277]

Answer:

the percentage of your solution that made up of HCI acid is 15%

Explanation:

The computation of the percentage of your solution that made up of HCI acid is given below:

Given that

There is 200g or a solution that have 0 g of hydrochloric acid (HCI)

Based on the above information

The percentage is

= 30g ÷ 200g

= 15%

Hence, the percentage of your solution that made up of HCI acid is 15%

7 0

3 years ago

A solution is prepared by mixing 0.0300 mol CH2Cl2 and 0.0500 mol CH2Br2 at 25 degrees C. Assuming the solution is ideal, calcul

Vinil7 [7]

Answer:

CH2Cl2 mole fraction = 0.833

CH2Br2 mole fraction = 0.167

Explanation:

Step 1: Data given

Number of moles CH2Cl2 = 0.0300 moles

Number of moles CH2Br2 = 0.0500 moles

Temperature = 25 °C

Vapor pressure of pure CH2Cl2 = 133 torr

Vapor pressure of pure CH2Br2 = 11.4 torr

Step 2: Calculate mol fraction in solution

Mol fraction CH2Cl2 = 0.0300 moles / (0.0300 + 0.0700)

Mol fraction CH2Cl2 = 0.300

Mol fraction CH2Br2 = 0.0700 moles / (0.0300 + 0.0700)

Mol fraction CH2Br2 = 0.700

Step 3: Calculate partial pressure

Partial pressure CH2Cl2 = 133 torr * 0.300 = 39.9 torr

Partial pressure CH2Br = 11.4 torr * 0.700 =7.98 torr

Step 4: Calculate the total pressure

total pressure = 39.9 + 7.98 = 47.88 torr

Step 5: Calculate mol fraction

partial pressure / total pressure = mole fraction

CH2Cl2 mole fraction = 39.9 / 47.88 = 0.833

CH2Br2 mole fraction = 7.98 / 47.88 = 0.167

3 0

3 years ago

Help fast! <br> Determine the density of a liquid if it’s mass is 50.5 grams.

Leto [7]

Answer:

do we have the volume ?

Explanation:

6 0

3 years ago

A sample of 325 mg of neon occupies 2 dm^3 at 20.0 c. use the perfect gas law to determine the pressure of the gas.

Musya8 [376]

Answer:

0.1935atm is the pressure of the gas.

Explanation:

In the problem you have the mass of Neon (You can obtain moles using molar mass), you have volume, and temperature. You can use general ideal gas law to solve pressure:

PV = nRT

P = nRT / V

<em>Where P is pressure in atm, n are moles, R is gas constant (0.082atmL/molK), T is absolute temperature (20.0°C + 273.15 = 293.15K), and V is volume in L = Volume in dm³</em>

<em />

<em>Moles gas:</em>

Molar mass Ne = 20.1797g/mol

0.325g * (1mol / 20.1797g) = 0.0161 moles

Replacing:

P = nRT / V

P = 0.0161 moles * 0.082atmL/molK * 293.15K / 2L

P = 0.1935atm is the pressure of the gas

7 0

3 years ago

Consider the reaction:

Fofino [41]

The mass in grams of NH₃ produced from the reaction is 3.4 g

<h3>Balanced equation</h3>

We'll begin by writing the balanced equation for the reaction. This illustrated below:

N₂ + 3H₂ -> 2NH₃

From the balanced equation above,

1 dm³ of N₂ reacted to produced 2 dm³ NH₃

<h3>How to determine the volume of NH₃ produced</h3>

From the balanced equation above,

1 dm³ of N₂ reacted to produced 2 dm³ NH₃

Therefore,

2.24 dm³ of N₂ will react to produce = 2.24 × 2 = 4.48 dm³ of NH₃

<h3>How to determine the mass of NH₃ produced</h3>

We'll begin by obtained the mole of 4.48 dm³ of NH₃. Details below:

22.4 dm³ = 1 mole NH₃

Therefore,

4.48 dm³ = 4.48 / 22.4

4.48 dm³ = 0.2 mole of NH₃

Finally, we shall determine the mass of NH₃ as follow:

Molar mass of NH₃ = 17 g/mol
Mole of NH₃ = 0.2 mole
Mass of NH₃ =?

Mass = mole × molar mass

Mass of NH₃ = 0.2 × 17

Mass of NH₃ = 3.4 g

Learn more about stoichiometry:

brainly.com/question/13196642

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4 0

1 year ago

Can someone answer 1 For me please?