A given sample of oxygen occupies 500 mL when the pressure is 800 mmHg. What volume will the gas occupy at 200 mmHg, provided the temperature remains constant?

Answers

Answer 1

Answer:

Answer:

The volume of the gas at 200 mmHg will be 2 L.

Explanation:

As the volume increases, the gas particles (atoms or molecules) take longer to reach the walls of the container and therefore collide with them fewer times per unit of time. This means that the pressure will be lower because it represents the frequency of collisions of the gas against the walls. In this way pressure and volume are related, determining Boyle's law which says:

"The volume occupied by a certain gaseous mass at constant temperature is inversely proportional to pressure"

Boyle's law is expressed mathematically as:

P * V = k

Now it is possible to assume that you have a certain volume of gas V1 that is at a pressure P1 at the beginning of the experiment. If you vary the volume of gas to a new value V2, then the pressure will change to P2, and it will be fulfilled:

P1 * V1 = P2 * V2

In this case:

P1= 800 mmHg
V1= 500 mL
P2= 200 mmHg
V2= ?

Replacing:

800 mmHg* 500 mL= 200 mmHg* V2

Solving:

$V2=(800 mmHg* 500 mL)/(200 mmHg)$

V2= 2,000 mL= 2 L (being 1,000 mL=1 L)

The volume of the gas at 200 mmHg will be 2 L.

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Answers

In the first situation: the mechanism of covection is the main form of heat transfer when warm air from a heater moves around and upward.

In the case of the metal pan the mechanism of heat transfer is conduction.

In the case of sunburn the mechanism is radiation.

In the case of an ice cube melting in a hand, conduction is the most important mechanism.

Answer:

An ice cube melts when a person holds it in his hand.

Explanation:

The reaction of Cr2O3 with silicon metal at high temperatures will make chromium metal.2Cr2O3(s)+3Si(s) -------> 4Cr(l)+3SiO2(s)

The reaction is begun with 161.00 g of Si and 139.00 g of Cr2O3.

How many grams of the excess reactant is left after the reaction is complete?

Answers

Answer: 122.9 g of $Si$ will be left from the given masses of both reactants.

Explanation:

$2Cr_2O_3(s)+3Si(s)\rightarrow 4Cr(l)+3SiO_2(s)$

To calculate the moles :

$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$

$\text{Moles of} Cr_2O_3=(139.00)/(152)=0.91moles$

$\text{Moles of} Si=(161.00)/(28)=5.75moles$

According to stoichiometry :

2 moles of $Cr_2O_3$ require 3 moles of $Si$

Thus 0.91 moles of $Cr_2O_3$ will require= $(3)/(2)* 0.91=1.36moles$ of $Si$

Thus $Cr_2O_3$ is the limiting reagent as it limits the formation of product and $Si$ is the excess reagent.

Thus (5.75-1.36) = 4.39 moles of excess reagent.

Mass of $Si=moles* {\text {Molar mass}}=4.39moles* 28g/mol=122.9g$

Thus 122.9 g of $Si$ will be left from the given masses of both reactants.

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Answers

Use stoichiometry and convert 2.3 grams of sodium to moles. Then convert the moles to atoms using 6.02(10)^23.

Post your answer and I'll post mine :)

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Answers

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Answers

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Answer:

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Explanation:

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