If the temperature changes in a chemical reaction, what has occurred?

A postulate of the kinetic molecular theory is listed.

valina [46]

Answer:

Postulate: Gas particles are extremely small and are far apart.

The activities can be used to demonstrate the postulate is :

Observing colored gas spreading into an inverted jar placed on top of a jar containing the gas

Explanation:

colored gas spreading into an inverted jar placed on top of a jar containing the gas:

This occur because of two reasons:

1. The Gaseous particles are largely spaced . There is large distance between the gases molecule

2. The gases are in continuous motion . Hence they posses very high kinetic energy . This is the reason they mixes quickly if placed in a jar.

This occur by the process of diffusion.

Diffusion of Gases: The intermixing of particles from the region of high concentration to low concentration.

The coloured gas goes into the space between the gaseous molecule present in the jar.(Gases are far apart)

As soon as the coloured gas is mixed in the jar , It spread quickly by diffusion because , The gaseous particles are extremely small and are far apart.

5 0

4 years ago

Can condensed milk be substituted for evaporated milk?

GaryK [48]

Yes because condensed milk and
evaporated milk are similar to one another. However, there won't be the same sweet flavor but the texture is the same.

7 0

3 years ago

What is the formula and valency of thiosulphate

tatuchka [14]

Formula: NA2S2O3. Valency: 2

6 0

3 years ago

1) How many molecules are there in 985 mL of nitrogen at 0.0° C and 1.00 x 10-6 mm Hg?

RSB [31]

Answer : The number of molecules present in nitrogen gas are, $3.48\times 10^{13}$

Explanation :

First we have to calculate the moles of nitrogen gas by using ideal gas equation.

$PV=nRT$

where,

P = Pressure of $N_2$ gas = $1.00\times 10^{-6}mmHg=1.32\times 10^{-9}atm$ (1 atm = 760 mmHg)

V = Volume of $N_2$ gas = 985 mL = 0.982 L (1 L = 1000 mL)

n = number of moles $N_2$ = ?

R = Gas constant = $0.0821L.atm/mol.K$

T = Temperature of $N_2$ gas = $0.0^oC=273+0.0=273K$

Now put all the given values in above equation, we get:

$(1.32\times 10^{-9}atm)\times 0.982L=n\times (0.0821L.atm/mol.K)\times 273K$

$n=5.78\times 10^{-11}mol$

Now we have to calculate the number of molecules present in nitrogen gas.

As we know that 1 mole of substance contains $6.022\times 10^{23}$ number of molecules.

As, 1 mole of $N_2$ gas contains $6.022\times 10^{23}$ number of molecules

So, $5.78\times 10^{-11}$ mole of $N_2$ gas contains $(5.78\times 10^{-11})\times (6.022\times 10^{23})=3.48\times 10^{13}$ number of molecules

Therefore, the number of molecules present in nitrogen gas are, $3.48\times 10^{13}$

8 0

3 years ago

What is anything that has mass and volume

Pavlova-9 [17]

Anything that has mass and volume (takes up space) is called matter.

3 0

3 years ago

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