All categories

1 year ago

How is density different from weight and mass?

2 answers:

6 0

Density is basically how compact an object is

Weight is how heavy an object is/ how much force it exerts

Mass is how much matter is in an object

I hope this helps! If you need the formulas on how to get them you can always comment and ask :)

defon1 year ago

5 0

Hello there!

How is density different from weight and mass you say? It's simple!

1. Unlike weight, density is composed of mass and volume.

2. By dividing the mass over the volume, you can determine an object's density, while weight is the product of mass and gravity.

Hope this helps :) if so, can I get Brainliest?

You might be interested in

A solution containing 8.3 g of a nonvolatile, nondissociating substance dissolved in 1.00 mol of chloroform, CHCl3, has a vapor

Margaret [11]

Answer:

a. Xm = 0.0229

b. 0.0234 moles

c. 354.1 g/mol

Explanation:

ΔP = P° . Xm

ΔP = P° - P', where P° is vapor pressure of pure solvent and P', vapor pressure of solution-

This is the formula for lowering vapor pressure.

If we apply the data given: 523 Torr - 511 Torr = 523 . Xm

Xm = ( 523 Torr - 511 Torr) / 523 Torr → 0.0229

Xm = Mole fraction of solute → Moles of solute / Total moles (sv + solute)

We can make this equation to determine moles of solute

0.0229 = Moles of solute / Moles of solute + 1

0.0229 (Moles of solute + 1) = Moles of solute

0.0229 = Moles of solute - 0.0229 moles of solute

0.0229 = 0.9771 moles of solute → 0.0229 / 0.9971 = 0.0234 moles

Molecular mass of solute → g/mol → 8.3 g / 0.0234 mol = 354.1 g/mol

7 0

3 years ago

Convert the following to moles.

Luda [366]

Use dimensional analysis.
$\frac{60.0 grams NaOH}{1} * \frac{1 mole NaOH}{40.0 amu NaOH} =1.5 moles$

$\frac{2.73 grams NH4Cl}{1} * \frac{1 mole NH4Cl}{53.49 amu NH4Cl} = .051 moles$

Now you try converting moles to grams. All you have to do is start with MOLES (Unlike the previous examples) over 1 then multiply that ratio by the ratio of molar mass over 1 mole. Hope this helps!

6 0

2 years ago

The kinetic-molecular theory of gases says A. the particles of a gas move independently of each other. B. the particles in a gas

Korolek [52]

Answer:

D. all of the above.

Explanation:

The kinetic-molecular theory of gases suggests that; the particles of a gas move independently of each other, the particles in a gas move rapidly, the particles in a gas are far apart.

Hope it helps.

5 0

3 years ago

B. if 6.73 g of na2co3 is dissolved in enough water to make 250. ml of solution, what is the molar concentration of sodium carbo

BARSIC [14]

Answer:- $[Na_2CO_3]=0.254M$ , $[Na^+]=0.508 M$ , $[CO_3^2^-]=0.254M$

Solution:- We are asked to calculate the molarity of sodium carbonate solution as well as the sodium and carbonate ions.

Molarity is moles of solute per liter of solution. We have been given with 6.73 grams of sodium carbonate and the volume of solution is 250.mL. Grams are converted to moles and mL are converted to L and finally the moles are divided by liters to get the molarity of sodium carbonate.

Molar mass of sodium carbonate is 105.99 gram per mol. The calculations for the molarity of sodium carbonate are shown below:

$\frac{6.73gNa_2CO_3}{250.mL}(\frac{1mol}{105.99g})(\frac{1000mL}{1L})$

= $0.254MNa_2CO_3$

So, molarity of sodium carbonate solution is 0.254 M.

sodium carbonate dissociate to give the ions as:

$Na_2CO_3(aq)\rightarrow 2Na^+(aq)+CO_3^2^-$

There is 1:2 mol ratio between sodium carbonate and sodium ion. So, the molarity of sodium ion will be two times of sodium carbonate molarity.

$[Na^+]=2(0.254M)$ = 0.508 M

There is 1:1 mol ratio between sodium carbonate and carbonate ion. So, the molarity of carbonate ion will be equal to the molarity of sodium carbonate.

$[CO_3^2^-]=0.254M$

5 0

3 years ago

How many moles of aluminum are needed to react completely with 1.2 mol of feo

Amanda [17]

Answer:

0.8 mol.

Explanation:

The balanced equation for the reaction between Al and FeO is represented as:

2Al + 3FeO → 3Fe + Al₂O₃,

It is clear that 2 mol of Al react with 3 mol of FeO to produce 3 mol of Fe and 1 mol of Al₂O₃.

Using cross multiplication:

2 mol of Al needs → 3 mol of FeO, from stichiometry.

??? mol of Al needs → 1.2 mol of FeO.

∴ The no. of moles of Al are needed to react completely with 1.2 mol of FeO = (2 mol)(1.2 mol)/(3 mol) = 0.8 mol.

3 0

3 years ago