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mrs_skeptik [129]

3 years ago

7

The atomic theory was proposed as early as 400 B.C. by Greek philosophers. Their hypothesis was not proven until much later. Wha

t is the main reason the Greek theory did not stand up over time?

1 answer:

Nastasia [14]3 years ago

5 0

The theory was not tested through experiment and review.

You might be interested in

The size of the gas particles compared to the overall volume of the gas is 22.4 L

jeka57 [31]

Well. Yeah. Basically.

1 mole of any gas is 22.4 L.

Not really sure if that answers your question but that's what i know.
Anyway if we are talking about the size then usually gases are filled with empty space.

4 0

4 years ago

[ 6.5 ] In the space below, briefly explain why the average times for the two CO2 molecules you calculated should have been simi

julsineya [31]

Answer:

This question is incomplete

Explanation:

This question is incomplete but there are two parts to this question that can generally be answered without the missing parts.

(1) If a CO₂ molecule starts out surrounded by other CO₂ molecules, does this influence how quickly it will reach the other side of the leaf?

What controls how quickly a CO₂ molecule/molecules enter into the leaf to the other parts of a leaf is the stomata on the leaf. Stomata are tiny openings on a plant leaf that allows for gaseous exchange (the release of oxygen and the absorption of CO₂) in the leaf.

(2) Collisions influence how molecules move, but do molecules only collide with other molecules of the same substance? NO

One of the kinetic theory of gases states that gases collide with one another and against the walls of the container. <u>It should however be noted that, gas molecules of a particular substance can collide with gas molecules of other substances</u>, so far they are within the same container.

5 0

3 years ago

How many moles are in 8.90 X 10^24 atoms of Na?

mixas84 [53]

Answer:

1.48 x 10^47 mol of Na

Explanation:

8.90 x 10^24 atoms of Na (1 mol of Na/6.022 x 10^23 atoms of Na)=

1.48 x 10^47 mol of Na

5 0

3 years ago

Phosgene, COCl2, gained notoriety as a chemical weapon in World War I. Phosgene is produced by the reaction of carbon monoxide w

jek_recluse [69]

The question is incomplete, here is the complete question:

Phosgene, $COCl_2$ , gained notoriety as a chemical weapon in World War I. Phosgene is produced by the reaction of carbon monoxide with chlorine:

$CO(g)+Cl_2(g)\rightleftharpoons COCl_2(g)$

The value of $K_c$ for this reaction is 5.79 at 570 K. What are the equilibrium partial pressures of the three gases if a reaction vessel initially contains a mixture of the reactants in which $p_{CO}=p_{Cl_2}=0.265atm$ and $p_{COCl_2}=0.000atm$ ?

<u>Answer:</u> The equilibrium partial pressure of CO, $Cl_2\text{ and }COCl_2$ is 0.257 atm, 0.257 atm and 0.008 atm respectively.

<u>Explanation:</u>

The relation of $K_c\text{ and }K_p$ is given by:

$K_p=K_c(RT)^{\Delta n_g}$

$K_p$ = Equilibrium constant in terms of partial pressure

$K_c$ = Equilibrium constant in terms of concentration = 5.79

$\Delta n_g$ = Difference between gaseous moles on product side and reactant side = $n_{g,p}-n_{g,r}=1-2=-1$

R = Gas constant = $0.0821\text{ L. atm }mol^{-1}K^{-1}$

T = Temperature = 570 K

Putting values in above equation, we get:

$K_p=5.79\times (0.0821\times 570)^{-1}\\\\K_p=0.124$

We are given:

Initial partial pressure of CO = 0.265 atm

Initial partial pressure of chlorine gas = 0.265 atm

Initial partial pressure of phosgene = 0.00 atm

The given chemical equation follows:

$CO(g)+Cl_2(g)\rightleftharpoons COCl_2(g)$

<u>Initial:</u> 0.265 0.265

<u>At eqllm:</u> 0.265-x 0.265-x x

The expression of $K_p$ for above equation follows:

$K_p=\frac{p_{COCl_2}}{p_{CO}\times p_{Cl_2}}$

Putting values in above equation, we get:

$0.124=\frac{x}{(0.265-x)\times (0.265-x)}\\\\x=0.0082,8.59$

Neglecting the value of x = 8.59 because equilibrium partial pressure cannot be greater than initial pressure

So, the equilibrium partial pressure of CO = $(0.265-x)=(0.265-0.008)=0.257atm$

The equilibrium partial pressure of $Cl_2=(0.265-x)=(0.265-0.008)=0.257atm$

The equilibrium partial pressure of $COCl_2=x=0.008atm$

Hence, the equilibrium partial pressure of CO, $Cl_2\text{ and }COCl_2$ is 0.257 atm, 0.257 atm and 0.008 atm respectively.

6 0

3 years ago

How many milliliters of a 1M nitric acid solution are required to prepare 60mL of 6.7M solution?

Free_Kalibri [48]

Answer:

the number of milliliters of a 1M is 402mL

Explanation:

The computation of the number of milliliters could be determined by using the following formula

As we know that

$V_1\times M_1 = V_2\times M_2$

where,

V_1 and V_2 are the starting and final volumes

And, the M_1 and M_2 are the starting and the final molarities

Now the V_1 is

$V_1 \times 1M = 60mL \times 6.7M$

So, the V_1 is 402mL

Hence, the number of milliliters of a 1M is 402mL

4 0

3 years ago