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Ahat [919]
2 years ago
15

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

mber of molecules the number of oxygen atoms
Chemistry
2 answers:
Phoenix [80]2 years ago
6 0

Answer : The correct option is, the number of molecules.

Explanation :

As we are given that 1 mole of oxygen gas, (O_2) and 1 mole of carbon monoxide gas, (CO).

From the given options, the number of molecules must be same when comparing 1 mole of oxygen gas, (O_2) and 1 mole of carbon monoxide gas, (CO) because there are 2 molecules present in both oxygen gas and carbon monoxide gas.

The mass of 1 mole of oxygen gas, (O_2) is, 32 g and the mass of 1 mole of carbon monoxide gas, (CO) is, 28 g. So, the mass will not be same.

The number of oxygen atoms in 1 mole of oxygen gas, (O_2) is, 2\times 6.022\times 10^{23} and the number of oxygen atoms in 1 mole of carbon monoxide gas, (CO) is, 1\times 6.022\times 10^{23}. So, the number of oxygen atoms will not be same.

The volume of 1 mole of oxygen gas, (O_2) and 1 mole of carbon monoxide gas, (CO) will not be same due to the difference in the masses.

Hence, the correct option is, the number of molecules.

jekas [21]2 years ago
3 0
The number of molecules because 1 mol is equal to 6.02x10^23 molecules, therefore they both have the same amount of molecules because they both have 1 mol
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Determine the specific heat ofmaterial if a 12g sample absorbed 48j as it was heated from 20-40
devlian [24]

Answer:

c =0.2 J/g.°C

Explanation:

Given data:

Specific heat of material = ?

Mass of sample = 12 g

Heat absorbed = 48 J

Initial temperature = 20°C

Final temperature = 40°C

Solution:

Specific heat capacity:

It is the amount of heat required to raise the temperature of one gram of substance by one degree.

Formula:

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

ΔT =  40°C -20°C

ΔT =  20°C

48 J = 12 g×c×20°C

48 J =240 g.°C×c

c = 48 J/240 g.°C

c =0.2 J/g.°C

6 0
2 years ago
What is he empirical formula for the compound that is of 1.85 moles of nitrogen and 4.63 miles of oxygen
BartSMP [9]

The empirical formula is N₂O₅.

The empirical formula is the <em>simplest whole-number ratio of atoms</em> in a compound.  

The ratio of atoms is the same as the ratio of moles, so our job is to calculate the <em>molar ratio of N:O</em>.  

I like to summarize the calculations in a table.  

<u>Element</u> <u>Moles</u>  <u>Ratio¹ </u>  <u> ×2²  </u>  <u>Integers</u>³

     N        1.85    1             2             2

     O        4.63    2.503   5.005     5

¹To get the molar ratio, you divide each number of moles by the smallest number (1.85).

²Multiply these values by a number (2) that makes the numbers in the ratio close to integers.

³Round off the number in the ratio to integers (2 and 5).

The empirical formula is N₂O₅.

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Explanation:

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