Everything in the world is made of matter except you?? TrueFalse

The student collects the H2 (g) produced by the reaction and measures the volume

BARSIC [14]

The question is incomplete, the complete question is;

The student collects the H2(g) produced by the reaction and measures its volume over water at 298 K after carefully equalizing the water levels inside and outside the gas-collection tube, as shown in the diagram below. The volume is measured to be 45.6mL . The atmospheric pressure in the lab is measured as 765 torr , and the equilibrium vapor pressure of water at 298 K is 24 torr .(i) The pressure inside the tube due to the H2(g)

Answer:

741 torr

Explanation:

From the question we can see that the atmospheric pressure in the lab is 765 torr.

The vapour pressure of water = 24 torr

From Dalton's law of partial pressure, we know that;

Total pressure = Pressure of the H2 + Partial pressure of water vapour

Therefore;

Pressure of H2 = Total pressure - Partial pressure of water vapour

Pressure of H2 = 765 torr - 24 torr = 741 torr

7 0

3 years ago

Which property of gases allows you to smell popcorn when you walk into a movie theater?

blsea [12.9K]

Gasses contain highly energetic particles which tend to spread out to fill the room/ container they are in. Often when a smell rises, there is a high concentration of gas molecules in the rising smell. Here diffusion occurs where the molecules spread out randomly moving from an area of high concentration of gas molecules to areas of low gas molecules.

5 0

3 years ago

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What are the products of the chemical reaction between solutions of sodium bromide with a solution of silver nitrate?

iren2701 [21]

Answer : The products of the chemical reaction are, $NaNO_3$ and $AgBr$

Explanation :

Balanced chemical reaction : It is defined as the reaction in which the number of atoms of individual elements present on reactant side must be equal to the product side.

When sodium bromide react with silver nitrate then it react to give sodium nitrate and silver bromide as a product.

The balanced chemical reaction will be:

$NaBr+AgNO_3\rightarrow NaNO_3+AgBr$

The given reaction is a double-displacement reaction in which the cation of two reactants molecule exchange their places to give two different products.

The species present on the left side of the right arrow is the reactant and the species present on the right side of the right arrow is the product.

In the balanced chemical reaction,

$NaBr$ and $AgNO_3$ are reactants.

$NaNO_3$ and $AgBr$ are products.

Hence, the products of the chemical reaction are, $NaNO_3$ and $AgBr$

3 0

3 years ago

2Al+ Fe203 Al203 +2Fe

leonid [27]

Answer:

229 g Al₂O₃; 243 g Fe₂O₃

Explanation:

We have the masses of two reactants, so this is a limiting reactant problem.

We know that we will need a balanced equation with masses, moles, and molar masses of the compounds involved.

Step 1. Gather all the information in one place with molar masses above the formulas and masses below them.

M_r: 26.98 159.69 101.96

2Al + Fe₂O₃ ⟶ Al₂O₃ + 2Fe

Mass/g: 121 601

===============

Step 2. Calculate the moles of each reactant

Moles of Al = 121 × 1/26.98

Moles of Al = 4.485 mol Al

Moles of Fe₂O₃ = 601× 1/159.69

Moles of Fe₂O₃ = 3.764 mol Fe₂O₃

===============

Step 3. Identify the limiting reactant

Calculate the moles of Al₂O₃ we can obtain from each reactant.

From Al

The molar ratio is 1 mol Al₂O₃:2 mol Al

Moles of Al₂O₃ = 4.485 × 1/2

Moles of Al₂O₃ = 2.242 mol Al₂O₃

From Fe₂O₃:

The molar ratio is 1 mol Al₂O₃:1 mol Fe₂O₃

Moles of Al₂O₃ = 3.764 × 1/1

Moles of Al₂O₃ = 3.764 mol Al₂O₃

The limiting reactant is Al because it gives the smaller amount of Al₂O₃.

The excess reactant is Fe₂O₃.

===============

Step 4. Calculate the mass of Al₂O₃ formed

Mass of Al₂O₃ = 2.242 × 101.96

Mass of Al₂O₃ = 229 g Al₂O₃

===============

Step 5. Calculate the moles of Fe₂O₃ reacted

The molar ratio is 1 mol Fe₂O₃:2 mol Al:

Moles of Fe₂O₃ = 4.485 × ½

Moles of Fe₂O₃ = 2.242 mol Fe₂O₃

===============

Step 6. Calculate the moles of Fe₂O₃ remaining

Moles remaining = original moles – moles used

Moles remaining = 3.764 – 2.242

Moles remaining = 1.521 mol Fe₂O₃

==============

Step 7. Calculate the mass of Fe₂O₃ remaining

Mass of Fe₂O₃ = 1.521 × 159.69/1

Mass of Fe₂O₃ = 243 g Fe₂O₃

3 0

4 years ago

A scientist observes that a certain fungus glows under ultraviolet light. What

atroni [7]

Answer:

C. Analyze data

Explanation:

5 0

3 years ago

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