Polar stratospheric clouds __________________________

The molar mass of sucrose (C12H22O11) is 342. 3 g/mol. A chemist has a 0. 500-mol sample of sucrose. What is the mass, in grams,

UNO [17]

Mass is the weight of the compound or the molecule in a sample that is given in grams. The mass of sucrose in the sample is 171 gms.

The mass of the compound is the product of the molar mass of the compound and the number of moles of the compound in a sample.

Given,

The molar mass (m.w.t) of sucrose = 342.3 g/mol

Number of moles (n) of sucrose = 0.500 moles

The mass of sucrose is calculated as:

$\begin{aligned} \rm mass &= \rm molar\; mass \times moles \\\\&= 342.3 \times 0.500\\\\&= 171.15 \;\rm gm\end{aligned}$

Therefore. the mass of sucrose in the sample is option A. 171 gms.

Learn more about mass here:

brainly.com/question/4058235

4 0

2 years ago

A chemist wants to extract copper metal from copper chloride solution. The chemist places 1.50 grams of aluminum foil in a solut

Llana [10]

Less than 6.0 grams of copper is formed, and some aluminum is left in the reaction mixture

<h3>Stoichiometric calculations</h3>

From the equation of the reaction:

3CuCl2 + 2Al → 2AlCl3 + 3Cu

Mole ratio of CuCl2 and Al = 3:2

Mole of 1.5 g aluminum foil = 1.5/26.98

= 0.06 moles

Mole of 14 g CuCl2 = 14/134.45

= 0.10 moles

For every 3 moles of CuCl2, 2 mole of Al is needed.

Thus, for 0.10 moles of CuCl2, the mole of Al needed would be:

0.10 x 2/3 = 0.07 moles

CuCl2 is, thus, slightly in excess while Al is the limiting reagent.

Mole ratio of Al and Cu = 2:3

For 0.06 mole Al, the mole of Cu will be: 0.06x3/2 = 0.09 moles

Mass of 0.09 moles Cu = 0.09 x 63.55

= 5.71 g

Thus, less than 6.0 grams Cu is formed while a little CuCl2 would be left in the reaction mixture.

More on stoichiometric calculations can be found here: brainly.com/question/8062886

5 0

2 years ago

What happens when baking soda and vinegar are mixed together.

egoroff_w [7]

Answer: Mixing vinegar and baking soda initiates a chemical reaction that produces carbon dioxide and water.

Explanation:

8 0

2 years ago

What is the volume of NH3 produced in the following reaction when 3.0L of N2 reacts with 4.0L of H2?

trapecia [35]

Hey there !

Given the reaction:

N2 + 3 H2 = 2 NH3

At constant pressure and temperature ,volume is proporcional to moles:

Theoretical moles of N2 and H2 => 1:3

Theoretical volume of N2 and H2 => 1:3

Experimental volume of N2 and H2 => 3.0 L : 4.0 L

0.75 : 1 = 2.25 : 3

Since N2 is in excess reactant , H2 is the limiting reactant

Therefore:

volume of NH3 is 2/3 * Volume of H2

= 2/3 * 4.0 = 2.66 L

Hope that helps!

4 0

4 years ago

Read 2 more answers

What mass of oxygen is needed for the complete combustion of 1.60-10^-3

vekshin1

Answer:

6.4×10¯³ g of O₂.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is given below:

CH₄ + 2O₂ —> CO₂ + 2H₂O

Next, we shall determine the masses of CH₄ and O₂ that reacted from the balanced equation. This can be obtained as follow:

Molar mass of CH₄ = 12 + (4×1)

= 12 + 4

= 16 g/mol

Mass of CH₄ from the balanced equation = 1 × 16 = 16 g

Molar mass of O₂ = 2 × 16 = 32 g/mol

Mass of O₂ from the balanced equation = 2 × 32 = 64 g

SUMMARY:

From the balanced equation above,

16 g of CH₄ reacted with 64 g of O₂.

Finally, we shall determine the mass of O₂ needed to react with 1.6×10¯³ g of CH₄. This can be obtained as illustrated below:

From the balanced equation above,

16 g of CH₄ reacted with 64 g of O₂.

Therefore, 1.6×10¯³ g of CH₄ will react with = (1.6×10¯³ × 64) / 16 = 6.4×10¯³ g of O₂

Thus, 6.4×10¯³ g of O₂ is needed for the reaction.

7 0

3 years ago

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