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lbvjy [14]
3 years ago
7

An aqueous 0.300 M glucose solution is prepared with a total volume of 0.150 L. The molecular weight of

Chemistry
1 answer:
Rudik [331]3 years ago
4 0

Answer:

8.11g

Explanation:

Given parameters:

Molarity of aqueous solution = 0.3M

total volume  = 0.15L

Molecular weight of glucose  = 180.6g/mol

Unknown:

Mass of glucose needed in the solution = ?

Solution:

To solve this problem, we need to understand molarity.

Molarity is the number of moles of solute in a given volume of solution. In this problem, the solute here is the glucose and the solvent is water.

      Molarity  = \frac{number of moles of solute}{volume of solution}

A solution is made up of solute and solvent.

   now, let us solve for the number of moles of the solute which is glucose;

   Number of moles of glucose  = molarity x volume of solution;

                                                      = 0.3 x 0.15

                                                      = 0.045mole

Now to find the mass of glucose;

        mass of glucose  = number of moles x molar mass

             input the parameters;

       

         Mass of glucose  = 0.045  x 180.16 = 8.11g

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2 years ago
N2(g) + 3H2(g) → 2NH3(g) How many grams of N2 are required to produce 240.0g NH3?
just olya [345]

Answer:

\large \boxed{\text{197.4 g}}

Explanation:

We will need a chemical equation with masses and molar masses, so, let's gather all the information in one place.

Mᵣ:     28.01               17.03

            N₂ + 3H₂ ⟶ 2NH₃

m/g:                          240.0

(a) Moles of NH₃

\text{Moles of NH}_{3} = \text{240.0 g NH}_{3}\times \dfrac{\text{1 mol NH}_{3}}{\text{17.03 g NH}_{3}}= \text{14.09 mol NH}_{3}

(b) Moles of N₂

\text{Moles of N$_{2}$} = \text{14.09 mol NH}_{3} \times \dfrac{\text{1 mol N$_{2}$}}{\text{2 mol NH}_{3}} = \text{7.046 mol N$_{2}$}

(c) Mass of N₂

\text{Mass of N$_{2}$} =\text{7.046 mol N$_{2}$} \times \dfrac{\text{28.01 g N$_{2}$}}{\text{1 mol N$_{2}$}} = \textbf{197.4 g N$_{2}$}\\\\\text{The reaction requires $\large \boxed{\textbf{197.4 g}}$ of N$_{2}$}

7 0
3 years ago
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A sample of gas X occupies 10 mº at a pressure of 120 kPa.
Mashutka [201]

Answer:

The new pressure of the gas comes out to be 400 KPa.

Explanation:

Initial volume of gas = V = 10\textrm{ m}^{3}

Initial pressure of gas = P = 120 KPa

Final volume of gas = V' = 3\textrm{ m}^{3}

Assuming temperature to be kept constant.

Assuming final pressure of the gas to be P' KPa

PV = P'V' \\120\textrm{ KPa}\times 10\textrm{ m}^{3} = \textrm{P'}\times 3\textrm{ m}^{3} \\\textrm{P'} = 400\textrm{ KPa}

New pressure of gas = 400 KPa

5 0
3 years ago
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