All categories

2 years ago

20 POINTS!!

Chemistry

1 answer:

Alenkinab [10]2 years ago

8 0

Answer:

1. molarity is = 0.1174

2. molarity is = 9.3

3. molarity is =0.009392

Explanation:

Q#1.

mass of sucrose is 14.07g

molar mass of sucrose is 342 3g/mol

so, 14.07x1/342.3 = 0.0411

now the volume is of water is 0.35

so, 0.0411/0.35 = 0.1174

Q#2.

concentration is 4.5

so, 4.5x1/1000= 0.0045

then, 0.0411/0.0045 = 9.13

Q#3.

M1M1=M2M2

molarity of the same sucrose is 0.1174

so, diluted in 40mL

and the volumetric flask is 500mL

so, 0.1174x40/500= 0.009392

You might be interested in

30. The density of an unknown gas at 27°C and 2 atm pressure is equal with density of N2 gas at

Zanzabum

Answer:

Molar mass of the unknown gas is 64.6 g/mol

Explanation:

Let's think this excersise with the Ideal Gases Law.

We start from the N₂. At STP conditions we know that 1 mol of anything occupies 22.4L.

We apply: P . V = n . R . T

5 atm . V = 1 mol . 0.082 . 325K

V = (1 mol . 0.082 . 325K) / 5 atm = 5.33 L

It is reasonable to say that, if we have more pressure, we may have less volume.

As this is the volume for 1 mol of N₂, our mass is 28 g. Then, the density of the nitrogen and the unknown gas is 28 g/5.33L = 5.25 g/L

Our unknown gas has, this density at 27°C and 2 atm.

If we star from this, again: 1 mol of any gas occupy 22.4L at STP, we can calculate the volume for 1 mol at those conditions:

P₁ . V₁ / T₁ = P₂ . V₂ / T₂

1 atm . 22,4L / 273K = 2 atm . V₂ / 300K

Remember that the value for T° is Absolute (T°C + 273)

[ (1 atm . 22.4L / 273K) . 300K] / 2 atm = V₂ → 12.3L

This is the volume for 1 mol of the unknown gas at 2 atm and 27°C

We use density to determine the mass: 12.3 L . 5.25 g/L = 64.6 g

That's the molar mass: 64.6 g/mol

6 0

2 years ago

1b<br>Describe the terms below:<br>2. adiabatic process

Ugo [173]

Answer:

defined as a process in which mo heat transfer take place

Explanation:

is a process which occurs without transferring heat /mass between the system and it's surrounding.

8 0

2 years ago

At 100°C, Kp = 60.6 for the reaction2NOBr(g) ⇄ 2NO(g) + Br₂(g) In a given experiment, 0.10 atm of each component is placed in a

Mariana [72]

The system is not at equilibrium.

The reaction will proceed to the right to attain the equilibrium.

Let's consider the following reaction.

2 NOBr(g) ⇌ 2 NO(g) + Br₂(g)

The pressure equilibrium constant (Kp) is 60.6. To determine if the system is at equilibrium when the pressure of each component is 1.75 atm, we have to calculate the reaction quotient (Q) and compare it with Kp.

Q = [NO]².[Br₂] / [NOBr]²

Q = (1.75)².(1.75) / (1.75)²

Q = 1.75

Since Q ≠ Kp, the system is not at equilibrium.

Since Q < Kp, the reaction will proceed to the right to attain the equilibrium.

To know more about equilibrium.

brainly.com/question/517289

#SPJ4

6 0

11 months ago

What volume of a 0.160 MM solution of KOHKOH must be added to 550.0 mLmL of the acidic solution to completely neutralize all of

puteri [66]

The given question is incomplete. The complete question is :

What volume of 0.160 M solution of KOH must be added to 550.0 mL of the acidic solution to completely neutralize all of the 0.150 M hydrochloric acid?

Answer: Volume in liters to three significant figures is 0.516 L

Explanation:

To calculate the volume of acid, we use the equation given by neutralization reaction:

$n_1M_1V_1=n_2M_2V_2$

where,

$n_1,M_1\text{ and }V_1$ are the n-factor, molarity and volume of acid which is $HCl$

$n_2,M_2\text{ and }V_2$ are the n-factor, molarity and volume of base which is KOH

We are given:

$n_1=1\\M_1=0.50M\\V_1=550.0mL\\n_2=1\\M_2=0.160M\\V_2=?$

Putting values in above equation, we get:

$1\times 0.150\times 550.0=1\times 0.160\times V_2\\\\V_2=516mL=0.516L$ (1L=1000ml)

Thus volume in liters to three significant figures is 0.516 L

6 0

3 years ago

6. when multiplying and dividing measured quantities, the number of significant figures in the result should be equal to the num

8090 [49]

The correct option is D.

Significant figure refers to the number of digits that are used to report a measured quantity. The amount of a significant number in a measurement always equal to the number of digits that are known with some degree of confidence and the last number, which is usually an estimate. When carrying out calculations with significant figures measurements, one must be careful to report the number of significant figure to reflect the least precise measurement.

4 0

3 years ago

Read 2 more answers