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3 years ago

Which must be the same when comparing 1 mol of oxygen gas, O2, with 1 mol of carbon monoxide gas, CO?

Chemistry

2 answers:

gayaneshka [121]3 years ago

7 0

Answer: C. The Number of Molecules

Explanation:

I just took the test.

Llana [10]3 years ago

5 0

A mole is a rather unusual unit of measurement. It is defined by a specific number of particles, molecules, atoms, or any other unit.
That number happens to be 6.022×10²³.
When we talk about a mole of water, then, we refer to 6.022×10²³ molecules of water.

Comparing 1 mole of 02 with 1 mole of CO:
This means means that both quantities will have the same number of molecules. The answer is C.

It may be tempting to select D, since it relates to the number of atoms rather than mass or volume, and moles are related to this idea. However, keep in mind that one mole of O2 will actually have twice as much oxygen atoms as one mole of CO, since there are two oxygen atoms per O2 molecule and only 1 oxygen atom per CO molecule.

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Please answer, please answer please answer please answer<br>my last 2 chemistry question.

scoundrel [369]

Answer:

1. filtration and evaporation

2. i) water is added to the sand and salt mixture

ii) then the mixture is filtrated and so the sand and the salt water was seperated

iii) the salt water is heated with the help of burner until the water gets evaporated

iv) after the water gets evaporated, the salt is remained in the container

3. observation:

on adding water to the mixture, the salt is completely dissolved in the water
when filtrated the sand is seperated from the salt water
now the salt water when heated with the burner until the evaporation, the water is evaporated
the salt is precipitated and remained in the container

4. cautions:

while using the burner, we should be cautious with fire
the container that is heated should be holded with the help of a cloth to avoid heat

7 0

3 years ago

A sample of propane (C3H8) has a mass of 0. 47 g. The sample is burned in a bomb calorimeter that has a mass of 1. 350 kg and a

Nady [450]

The amount of heat released by the sample has been 22.54 kJ. Thus, option C is correct.

The specific heat has been defined as the amount of heat required to raise the temperature of 1 gram of substance by 1 degree Celsius.

The specific heat has been expressed as:

$q=mc\Delta T$

<h3 /><h3>Computation for the heat absorbed</h3>

The iron and calorimeter are in side the closed system. Thus, the energy released by the sample, has been equivalent to the energy absorbed by the calorimeter.

$q_{released}=q_{absorbed}\\
q_{released}=m_{calorimeter}\;c_{calorimeter}\;\Delta T$

The given mass of calorimeter has been, $m_{calorimeter}=1350\;\rm g$

The specific heat of the calorimeter has been, $c_{calorimeter}=5.82\;\rm J/g^\circ C$

The change in temperature of the calorimeter has been, $\Delta T=2.87^\circ \rm C$

Substituting the values for heat released:

$q_{released}= 1350\;\text g\;\times\;5.82\;\text J/\text g^\circ \text C\;\times\;2.87^\circ \text C\\
q_{released}=22,549.5\;\text J\\
q_{released}}=22.54\;\rm kJ$

The amount of heat released by the sample has been 22.54 kJ. Thus, option C is correct.

Learn more about specific heat, here:

brainly.com/question/2094845

6 0

3 years ago

What is the molar mass of an unknown gas<br> with a density of 4.95 g/L at 1.00 atm and<br> 25.0 °C?

mestny [16]

Answer:

121 g/mol

Explanation:

To find the molar mass, you first need to calculate the number of moles. For this, you need to use the Ideal Gas Law. The equation looks like this:

PV = nRT

In this equation,

-----> P = pressure (atm)

-----> V = volume (L)

-----> n = moles

-----> R = constant (0.0821 L*atm/mol*K)

-----> T = temperature (K)

Because density is comparing the mass per 1 liter, I am assuming that the system has a volume of 1 L. Before you can plug the given values into the equation, you first need to convert Celsius to Kelvin.

P = 1.00 atm R = 0.0821 L*atm/mol*K

V = 1.00 L T = 25.0. °C + 273.15 = 298.15 K

n = ? moles

PV = nRT

(1.00 atm)(1.00L) = n(0.0821 L*atm/mol*K)(298.15 K)

1.00 = n(0.0821 L*atm/mol*K)(298.15 K)

1.00 = (24.478115)n

0.0409 = n

Now, we need to find the molar mass using the number of moles per liter (calculated) and the density.

0.0409 moles ? grams 4.95 grams
---------------------- x ------------------ = ------------------
1 L 1 mole 1 L

? g/mol = 121 g/mol

**note: I am not 100% confident on this answer

3 0

2 years ago

A compound is found to contain 64.80 % carbon, 13.62 % hydrogen, and 21.58 % oxygen by weight. What is the empirical formula for

insens350 [35]

Answer:

Empirical formula is C₄H₁₀O

Explanation:

Values for C, H and O are determined as centesimal composition.

64.80 g of C in 100g of compound

13.62g of H in 100 g of compound

21.58 g of O in 100 g of compound.

We convert the mass to moles:

64.80 g . 1mol/ 12g = 5.4 moles of C

13.62 g . 1 mol /1g = 13.62 moles of H

21.58 g . 1 mol/16g = 1.35 moles of O

We pick the lowest value and we divide:

5.4 moles of C / 1.35 = 4 C

13.62 moles of H / 1.35 = 10 H

1.35 moles of O / 1.35 = 1 O

Empirical formula is C₄H₁₀O, it can be the diethyl ether.

We confirm, the excersise is well done.

Molar mass = 74g/mol

74 g of compound we have (12 . 4)g of C

In 100 g of compound we may have (100 . 48) / 74 = 64.8 g

5 0

3 years ago

HELP THIS IS DUE IN A FEW MINUTES

Arlecino [84]

If matters mix and it doesn’t make a material it’s called physical change. But, if maters are mixed and they do make a material it’s called chemical change.

3 0

3 years ago

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