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3 years ago

A salt sample is placed into some water and nearly all of it dissolves without stirring or heating. the resulting solution is

1 answer:

7 0

The resulting solution is unsaturated.

An unsaturated solution is one in which the amount of solute can be increased. We know that the solution is unsaturated because there is no salt at the bottom of the solution and no means were required to increase the salt's solubility such as increasing temperature or stirring. Once the solution becomes saturated, additional salt will only deposit at the bottom unless changes in conditions are made.

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Pro ∆G0=-RT in k Known as

stepan [7]

Answer:

Gibbs free energy equation

Explanation:

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3 years ago

what biome has many nocturnal animals that burrow underground during the day that are active at night

hram777 [196]

Answer:

it could be maybe a raccoon or a possum

Explanation:

4 0

3 years ago

The octet rule states that all atoms would like to have 8 electrons in their last shell with no exceptions! true or false

Montano1993 [528]

True due to the fact that eight electrons are what applies directly to the octet rule

7 0

3 years ago

10g of hyrogen react with excess of oxygen gas according to the equation:

Degger [83]

Answer:

Volume of O₂ = 56 dm³

mass of water vapors (H₂O) = 90 g

Explanation:

Data Given:

mass of Oxygen = 10 g

Volume of Oxygen = ?

mass of the water vapor = ?

Reaction Given:

2H₂+O₂---->2H₂O

Solution:

First we have to look at the reaction for the information required

2H₂ + O₂ -------> 2H₂O

2 mol 1mol 2 mol

now convert moles to grams

molar mass of H₂ = 2(1) = 2 g/mol

molar mass of O₂ = 2(16) = 32 g/mol

molar mass of H₂0 = 2(1) + 16 = 18 g/mol

So the masses will be

2H₂ + O₂ -------> 2H₂O

2 mol (2 g/mol) 1mol (32 g/mol) 2 mol (18 g/mol)

4 g 32 g 36 g

So now we know that

4 g of hydrogen combine with 32 g of Oxygen and give 36 g of water vapors.

By using above information

First we find the volume of Oxygen:

For this first we find mass and then moles of Oxygen

As we know

if 4 g of hydrogen combine with 32 g of Oxygen then how much oxygen will react with 10 g of hydrogen

Apply unity formula

4 g of hydrogen H₂ ≅ 32 g of Oxygen O₂

10 g of hydrogen H₂ ≅ X g of Oxygen O₂

by doing Cross multiplication

g of Oxygen O₂ = 32 g x 10 g / 4 g

g of Oxygen O₂ = 80 g

So,

mass of oxygen = 80 g

now find moles of oxygen

formula used:

no. of moles = mass in grams/ molar mass . . . . . . (1)

Put values in above equation 1

no. of moles = 80 g / 32 g/mol

no. of moles = 2.5

Now to find volume of oxygen

Formula used

Volume of O₂ = no. of moles x molar volume (22.4 dm³/ mol) . . . . . . (2)

Put values in equation 2

Volume of O₂ = 2.5 moles x 22.4 dm³/mol

Volume of O₂ = 56 dm³

______________________

Now to find mass of water vapors

As we now

if 4 g of hydrogen produce 36 g of water vapors then how much water vapor will produce from 10 g of hydrogen

Apply unity formula

4 g of hydrogen H₂ ≅ 36 g of water vapors (H₂O)

10 g of hydrogen H₂ ≅ X g of water vapors (H₂O)

by doing Cross multiplication

g of water vapors (H₂O) = 36 g x 10 g / 4 g

g of water vapors (H₂O) = 90 g

So,

mass of water vapors (H₂O) = 90 g

5 0

3 years ago

A sample of a gas in a rigid cylinder with a movable piston has a volume of a lamp then .2 L at STP. What is the volume of this

Gnoma [55]

Answer: The new volume of the gas is 0.11 L

Explanation:

To calculate the volume when temperature and pressure has changed, we use the equation given by combined gas law.

The equation follows:

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

where,

$P_1,V_1\text{ and }T_1$ are the initial pressure, volume and temperature of the gas

$P_2,V_2\text{ and }T_2$ are the final pressure, volume and temperature of the gas

At STP:

The temperature at this condition is taken as 273 K and the pressure at this condition is taken as 1 atm or 101.3 kPa.

We are given:

$P_1=101.3kPa\\V_1=0.2L\\T_1=273K\\P_2=202.6kPa\\V_2=?\\T_2=300K$

Putting values in above equation, we get:

$\frac{101.3kPa\times 0.2L}{273K}=\frac{202.6kPa\times V_2}{300K}\\\\V_2=\frac{101.3\times 0.2\times 300}{273\times 202.6}=0.11L$

Hence, the new volume of the gas is 0.11 L

3 0

3 years ago