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2 years ago

A mineral sample has a mass of 75 g. When the sample is dropped

Chemistry

2 answers:

Elena-2011 [213]2 years ago

5 0

Answer:

3.75 g/mL

Explanation:

Density can be calculated using the following formula:

Density = mass (g) / volume (mL)

You have been given the mass of the mineral sample (75 g). To find the volume, you need to determine the amount of space that the sample takes up when it is placed in the water. This can be done by subtracting the initial water volume from the final water volume.

Volume = Final - Initial

Volume = 40 mL - 20 mL

Volume = 20 mL

Now, you can calculate the density of the mineral sample.

Density = mass / volume

Density = 75 g / 20 mL

Density = 3.75 g/mL

Ainat [17]2 years ago

4 0

Answer:

Explanation:

Givens

The volume is the tricky part of this question. You are using the graduated cylinder to measure volume. The rise in the reading of the graduated cylinder = the volume of the sample.

Volume = 40 mL - 20 mL = 20 mL

Mass = 75 grams

Formula

Density = mass / volume

Solution

Density = 75 / 20 = 3.75

Answer

Density = 3.75

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The reaction of hydrogen and iodine to produce hydrogen iodide has a Kc of 54.3 at 703 K. Given the initial concentrations of H2

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Answer:

[HI] = 0.7126 M

Explanation:

Step 1: Data given

Kc = 54.3

Temperature = 703 K

Initial concentration of H2 and I2 = 0.453 M

Step 2: the balanced equation

H2 + I2 ⇆ 2HI

Step 3: The initial concentration

[H2] = 0.453 M

[I2] = 0.453 M

[HI] = 0 M

Step 4: The concentration at equilibrium

[H2] = 0.453 - X

[I2] = 0.453 - X

[HI] = 2X

Step 5: Calculate Kc

Kc = [Hi]² / [H2][I2]

54.3 = 4x² / (0.453 - X(0.453-X)

X = 0.3563

[H2] = 0.453 - 0.3563 = 0.0967 M

[I2] = 0.453 - 0.3563 = 0.0967 M

[HI] = 2X = 2*0.3563 = 0.7126 M

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3 years ago

How many grams of sodium carbonate are produced when 5.3 moles of sodium phosphate reacts with aluminum carbonate?

Korvikt [17]

Answer: There is 842.54 grams of sodium carbonate are produced when 5.3 moles of sodium phosphate reacts with aluminum carbonate.

Explanation:

Chemical equation depicting reaction between sodium phosphate and aluminum carbonate is as follows.

$Al_{2}(CO_{3})_{3} + 2Na_{3}PO_{4} \rightarrow 2AlPO_{4} + 3Na_{2}CO_{3}$

As this equation contains same number of atoms on both reactant and product side. So, this equation is a balanced equation.

According to the equation, 2 moles of sodium phosphate is giving 3 moles of sodium carbonate.

Therefore, sodium carbonate formed by 5.3 moles of sodium phosphate is as follows.

$\frac{3}{2} \times 5.3 mol\\= 7.95 mol$

As number of moles is the mass of substance divided by its molar mass. So, mass of sodium carbonate ( molar mass = 105.98 g/mol) is as follows.

$No. of moles = \frac{mass}{molar mass}\\7.95 mol = \frac{mass}{105.98 g/mol}\\mass = 842.54 g$

Thus, we can conclude that there is 842.54 grams of sodium carbonate are produced when 5.3 moles of sodium phosphate reacts with aluminum carbonate.

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Answer:

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