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4vir4ik [10]
2 years ago
7

Suppose you take a piece of hard wax from an unlit candle. After you roll the wax between your fingers for a while, it becomes s

oft. What State of matter is the softer wax ? Is it possible for wax to change without changing state
Chemistry
2 answers:
jolli1 [7]2 years ago
6 0

Answer:

the candle is still solid..................in this case, yes!

Explanation:

it is still solid because the molecules are packed together tighter than the molecules in a liquid or gas.

lisabon 2012 [21]2 years ago
4 0

Answer:

soild form

Explanation:

You might be interested in
How many moles of sulfur<br> dioxide are in 2.26 x 10^33 sulfur dioxide molecules?
LUCKY_DIMON [66]

Answer:

moles = no. of molecules / Avogadro's number

         = 2.26 x 10^33 / 6.022 x 10^23

         = 3752906011

Round to significant figures which is 3 = 3.75 x 10^9 mol

Explanation: The formula for finding how many moles of a substance when given the amount of molecules is: moles = number of molecules / Avogadro's number

6 0
3 years ago
What is the mass in grams of ba(io3)2 can be dissolved in 500 ml of water at 25 degrees celcius?
lesya [120]

The mass of Ba(IO3)2 that can be dissolved in 500 ml of water at 25 degrees celcius is 2.82 g

<h3>What mass of Ba(IO3)2 can be dissolved in 500 ml of water at 25 degrees celcius?</h3>

The Ksp of Ba(IO3)2 = 1.57 × 10^-9

Molar mass of Ba(IO3)2 = 487 g/mol?

Dissociation of Ba(IO3)2 produces 3 moles of ions as follows:

Ba(IO_{3})_{2} \leftrightharpoons Ba^{2+} + 2\:IO_{3}^{-}

Ksp = [Ba^{2+}]*[IO_{3}^{-}]^{2}

[Ba(IO_{3})_{2}] =  \sqrt[3]{ksp} =\sqrt[3]{1.57 \times  {10}^{ - 9} } \\  [Ba(IO_{3})_{2}] = 1.16 \times  {10}^{-3} moldm^{-3}

moles of Ba(IO3)2 = 1.16 × 10^-3 × 0.5 = 0.58 × 10^-3 moles

mass of Ba(IO3)2 = 0.58 × 10^-3 moles × 487 = 2.82 g

Therefore, mass Ba(IO3)2 that can be dissolved in 500 ml of water at 25 degrees celcius is 2.82 g.

Learn more about mass and moles at: brainly.com/question/15374113

#SPJ12

7 0
1 year ago
Solid ammonium chloride, NH4Cl, is formed by the reaction of gaseous ammonia, NH3, and hydrogen chloride, HCl. NH3(g)+HCl(g)⟶NH4
Mashutka [201]

9.41 atm is the pressure in atmospheres of the gas remaining in the flask

<h3>What is the pressure in atmospheres?</h3>

The equation NH3(g) + HCl(g) ==> NH4Cl(s) is balanced.

Divide the moles of each reactant by its coefficient in the balanced equation, and the limiting reagent is identified as the one whose value is less. With the issue we now have...

6.44 g NH3 times 1 mol NH3/17 g equals 0.3688 moles of NH3 ( 1 = 0.3688)

HCl: 6.44 g of HCl times one mole of HCl every 36.5 g equals 0.1764 moles ( 1 = 0.1764). CONTROLLING REAGENT

NH4Cl will this reaction produce in grams

0.1764 moles of HCl multiplied by one mole of NH4Cl per mole of HCl results in 9.44 g of NH4Cl (3 sig. figs.)

the gas pressure, measured in atmospheres, that is still in the flask

NH3(g) plus HCl(g) results in NH4Cl (s)

0.3688......0.1764............0..........

Initial

-0.1764....-0.1764........+0.1764...Change

Equilibrium: 0.1924.......0...............+0.1924

There are 0.1924 moles of NH3 and no other gases in the flask. This is at a temperature of 25 °C (+273 = 298 °K) in a volume of 0.5 L. After that, we may determine the pressure by using the ideal gas law (P).

PV = nRT

P = nRT/V = 0.1924 mol, 0.0821 latm/mol, and 298 Kmol / 0.5 L

P = 9.41 atm

9.41 atm is the pressure in atmospheres of the gas remaining in the flask

To learn more about balanced equation refer to:

brainly.com/question/11904811

#SPJ1

7 0
1 year ago
What is the right answer for this. I really need help
statuscvo [17]
<span>así que te está diciendo que</span>
6 0
3 years ago
How many molecules are in 7.34 g of Na2CO3
kenny6666 [7]

Answer:

The answer is 105.98844.

<h3>Explanation: </h3>

We assume you are converting between grams Na2CO3 and mole. You can view more details on each measurement unit: molecular weight of Na2CO3 or mol This compound is also known as Sodium Carbonate.

7 0
3 years ago
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