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4 years ago

Assuming the following materials will not mix,show how the materials would "Stack up" in a graduated cylinder.

Chemistry

1 answer:

mihalych1998 [28]4 years ago

4 0

<u>Answer:</u>

Density is mass per unit volume.

Its formula is

Density = Mass / Volume

Its units can be kg/L or kg/( $dm^3$ ) or g/mL or g/( $cm^3$ )

Density of various substances are given. The more denser substance goes to the bottom of the graduated cylinder.

Air on the top then comes Wood followed by Corn oil followed by Ice and then Water followed by Glycerin then Rubber then Corn syrup and at last Steel at the bottom which will more denser than all the substances mentioned above.

The staking up of the substances is in the order mentioned below in the tabular column

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How many chloride ions are in 2.6 moles of CaCl2?

Rama09 [41]

Answer:

31.31× 10²³ number of Cl⁻ are present in 2.6 moles of CaCl₂ .

Explanation:

Given data:

Number of moles of CaCl₂ = 2.6 mol

Number of Cl₂ ions = ?

Solution:

CaCl₂ → Ca²⁺ + 2Cl⁻

The given problem will solve by using Avogadro number.

It is the number of atoms , ions and molecules in one gram atom of element, one gram molecules of compound and one gram ions of a substance.

The number 6.022 × 10²³ is called Avogadro number.

In one mole of CaCl₂ there are two moles of chloride ions present.

In 2.6 mol:

2.6×2 = 5.2 moles

1 mole Cl⁻ = 6.022 × 10²³ number of Cl⁻ ions

5.2 mol × 6.022 × 10²³ number of Cl⁻ / 1mol

31.31× 10²³ number of Cl⁻

8 0

3 years ago

Fill in the blanks with the word bank. !!URGENT NEED TODAY!!

stiv31 [10]

blank 1: lost

blank 2: gained

blank 3: same

blank 4: side

blank 5: equation

blank 6: coefficients

blank 7: formulas

blank 8: change

6 0

3 years ago

Combustion of hydrocarbons such as undecane (C_11H_24) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Eart

bekas [8.4K]

Answer:

Volume of carbon dioxide is 428.23 L.

Explanation:

Below is the chemical reaction or chemical equation for the combustion of hydrocarbons such as undecane into carbon dioxide.

$C_{11}H_{24}(l) + 17O_{2}(g) \to 11CO_{2} (g) + 12H_2O(g)$

Here, undecane is in liquid form that reacts with gaseous oxygen (combustion) and produces carbon dioxide and water as a product in the gaseous form.

The molar mass of undecane = $156.31 g/mol.$

$\text{Number of moles} = \frac{260g}{156.31g/mol} = 1.66 \ mol.$

From the equation, it can be seen that 1 mole of undecane produces 11 moles of carbon dioxide. Therefore, 1.66 mol will produce 18.26 mol of carbon dioxide.

Now find the volume of 18.26 mol of carbon dioxide when the temperature is 13 degrees Celsius and pressure is 1 atm.

$V = \frac{nRT}{P} \\$

$V = \frac{18.26 \times 0.082 \times 286 \ K}{1atm} \\$

$V = 428.23 \ L$

6 0

3 years ago

A student was asked to prepare 500.0 mL of 6.0 M NaOH. The student measured 120.0 g of NaOH and placed it in a 1000 mL beaker. T

Morgarella [4.7K]

Answer:

The concentration of the solution will be much lower than 6M

Explanation:

To prepare a solution of a solid, the appropriate mass is taken and accurately weighed in a weighing balance and then made up to mark with distilled water.

From

n= CV

n = number of moles m/M( m= mass of solid, M= molar mass of compound)

C= concentration of substance

V= volume of solution

m=120g

M= 40gmol-1

V=500ml

120/40= C×500/1000

C= 120/40× 1000/500

C=6M

This solution will not be exactly 6M if the student follows the procedure outlined in the question. The actual concentration will be much less than 6M.

This is because, solutions are prepared in a standard volumetric flask. Using a 1000ml beaker, the student must have added more water than the required 500ml thereby making the actual concentration of the solution less than the expected 6M.

7 0

3 years ago

15 Celsius to kelvin

navik [9.2K]

Answer:

308K

Explanation:

293+15=308

7 0

3 years ago

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