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3 years ago

In the space, show a correct numerical setup for calculating the number of moles of CO2 present in 11 grams of CO2

Chemistry

1 answer:

makvit [3.9K]3 years ago

4 0

Ans: Moles of CO2 = 0.25 moles

Given:

Mass of CO2 = 11 g

To determine

Moles of CO2

Explanation:

Moles = mass/molecular mass

Molecular mass of CO2 = 44 g/mol

Moles of CO2 = 11 g/44 g.mol-1 = 0.25 moles

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Observe the image of the results. List the properties you see.

natka813 [3]

Answer:

C. three substances i believe

Explanation:

lmk if im wrong (im sorry if i am!!) But its because the first pic, its a solid substance, 2nd pic is a liquid substance and 3rd pic is condensation or like gas.

8 0

3 years ago

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Calculate the number of grams contained in each of the following number of moles. Report your answer with the appropriate number

Debora [2.8K]

Answers:

a. 131.85 grams

b. 134.69 grams

To calculate the number of grams in the number of moles given for each compound, consider the formula:

Moles = No. of grams / molar mass

Therefore, to find the gram it will become:

No. of grams = moles x molar mass

a. 0.410 mol of NaCl (sodium chloride)

Molar mass of NaCl = (286.14 + 35.45) = 321.59

No. of grams = moles x molar mass

No. of grams = 0.410 x 321.59 = 131.85 grams

b. 4.80 mol of C2H4 (ethylene)

Molar mass of C2H4 = (12.01 x 2) + (1.01 x 4) = 28.06

No. of grams = moles x molar mass

No. of grams = 4.80 x 28.06 = 134.69 grams

3 0

3 years ago

Read 2 more answers

Which of the following pairs of atoms exhibit an ionic bond?

katen-ka-za [31]

Fe & O makes an ionic bond because of this
Metal and Metal = Metallic
Non-Metal and Metal = Ionic
Non-Metal and Non-Metal = Covalent
In this case Oxygen (O) is a Non-Metal and Iron (Fe) is a Metal so you have an Ionic Bond

5 0

4 years ago

Read 2 more answers

At 20°C, a 0.756 M aqueous solution of ammonium chloride has a density of 1.0107 g/mL. What is the mass % of ammonium chloride i

Molodets [167]

Answer:

$\%m/m=4\%$

Explanation:

Hello,

In this case, by knowing that the molarity is measured in molal units which are mole per liter of solution and the by-mass percentage demands us to compute the mass of the solution, we proceed by assuming 1 L of solution:

$m_{solution}=1L*\frac{1000mL}{1L}*\frac{1.0107g}{1mL} =1010.7g$

Then, for 1 L of solution, we have 0.756 moles of solute (ammonium chloride), so we compute the grams for those moles by using its molar mass of 53.491 g/mol as shown below:

$m_{solute}=0.756mol*\frac{53.491g}{1mol}=40.4g$

Finally, we compute the by-mass percentage as shown below:

$\%m/m=\frac{m_{solute}}{m_{solution}} *100\%=\frac{40.4g}{1010.7g}*100 \%\\\\\%m/m=4\%$

Best regards.

6 0

3 years ago

What is the wavelength of spectral line resulted from the electron transition from n=3 to n=2 in a hydrogen atom.

MakcuM [25]

Answer:

$\lambda=6.56x10^{-7}m$

Explanation:

Hello there!

In this case, it possible to use the Rydberg equation in order to calculate the wavelength for this transition from n=3 to n=2 as shown below:

$\frac{1}{\lambda} =R_H(\frac{1}{n_f^2}-\frac{1}{n_i^2} )$

Thus, we plug in the corresponding energy levels and the Rydberg constant to obtain:

$\frac{1}{\lambda} =10973731.6m^{-1}(\frac{1}{2^2}-\frac{1}{3^2} )\\\\\frac{1}{\lambda} =1524129.4m^{-1}\\\\\lambda=\frac{1}{1524129.4m^{-1}} \\\\\lambda=6.56x10^{-7}m$

Best regards!

5 0

3 years ago