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Tatiana [17]
3 years ago
8

A chemist must dilute of aqueous potassium dichromate solution until the concentration falls to . He'll do this by adding distil

led water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Be sure your answer has the correct number of significant digits.
Chemistry
1 answer:
Phantasy [73]3 years ago
5 0

The question is incomplete; the complete question is;

A chemist must dilute 99.4 mL of 152 mM aqueous potassium dichromate (K_2Cr_2O_7) solution until the concentration falls to 55.0 mM He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in liters. Be sure your answer has the correct number of significant digits.

Answer:

0.275 L

Explanation:

From C1V1 = C2V2

Where;

C1= initial concentration of the solution 152 × 10^-3 M

V1= initial volume of the solution = 99.4 × 10^-3 L

C2 = concentration after dilution = 55 × 10^-3 M

V2 = volume after dilution = the unknown

V2 = C1 V1/C2

V2 = 152 × 10^-3 × 99.4 × 10^-3 / 55 × 10^-3

V2 = 0.275 L

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Is gas occupies 733 cm at 10.9 at what temp will it occupy 950 cm
alexgriva [62]

Temperature of gas at volume of 950 cm³ is 368.14K or 94.99⁰c.

  • Volume is the amount of space a three-dimensional object takes up, expressed in cubic units.
  • units of volume are mL, liter, cm³ or m³.

Given,

in this question, volume occupied by gas at 10.9⁰c is 733cm³.

we have to find out temperature at which gas occupies volume of 950 cm³.

First, convert temperature from celcius to Kelvin

10.9⁰c = 10.9 + 273.15 = 284.05 K

By equation or Boyle's Law

P1 x V1 / T1 = P2 x V2 / T2

Pressure is constant here

therefore, V1 / T1 = V2 / T2

here, V1 = 733 cm³

T1 = 284.05 K

V2 = 950 cm³

we have to find out T2

So, 733 / 284.05 = 950 / T2

T2 = 284.05 × 950 / 733 = 368.14 K

= 94. 99⁰c

Therefore the temperature of gas at volume of 950 cm³ is 368.14K or 94.99⁰c.

Learn more about Boyle's Law here:

https://brainly.in/question/2900894

#SPJ9

5 0
2 years ago
Need help with 1 2 and 3
Pepsi [2]
1 would be the 3 one
Hope it’s correct
4 0
3 years ago
The empirical formula of styrene is CH; the molar mass of styrene is 104.14 g/mol. How many H atoms are present in a 7.80 g samp
Makovka662 [10]

Answer:

In 7.80 g of styrene, we have 3.60×10²³ atoms of H

Explanation:

Empirical formula of styrene is CH

Molecular formula of styrene is C₈H₈

So, 1 mol of styrene has 8 moles of C and 8 moles of H and 1 mol weighs 104.14 grams. Let's make a rule of three:

104.14 g (1 mol of C₈H₈) have 8 moles of H

Then 7.80 g would have ( 7.80  .8) / 104.14 = 0.599 moles

As we know, 1 mol of anything has NA particles (Avogadro's Number,  6.02×10²³), so 0.599 moles will have (mol . NA) particles

0.599 mol . 6.02×10²³ atoms / 1 mol = 3.60×10²³ atoms

3 0
3 years ago
1 2.2.3 Quiz: Shapes of Molecules
ivann1987 [24]

Answer:

iu

Explanation:

kjk

8 0
3 years ago
A 3.0 L cointainer contains 4 mol He, 2 mol Ne,and 1 mol Ar. What is the mole fraction of neon gas? What is the partial pressure
CaHeK987 [17]

Answer:

Partial pressure of Ne = 1.43 atm

Explanation:

Step 1: Data given

Volume = 3.0 L

Number of moles He = 4 moles

Number of moles Ne = 2 moles

Number of moles Ar = 1 mol

Total pressure = 5 atm

Step 2: Calculate total moles

Total moles = 4 moles + 2 moles + 1 mol

Total moles = 7 moles

Step 3: Calculate the mol ratio

Mol ratio = moles / total mol

Mol ratio He = 4 moles / 7 moles = 0.571

Mol ratio Ne = 2 moles / 7 moles = 0.286

Mol ratio Ar = 1 mol / 7 moles = 0.143 moles

Ste p4: Calculate partial pressure

PArtial pressure = mol ratio * total pressure

Partial pressure of Ne = mol ratio Ne * total pressure

Partial pressure of Ne = 0.286 * 5 atm

Partial pressure of Ne = 1.43 atm

8 0
3 years ago
Read 2 more answers
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