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3 years ago

What is the density of a mineral with a mass of 41.2 g and a volume 8.2 cm3?

Chemistry

2 answers:

Tanya [424]3 years ago

7 0

Answer : The density of a mineral is, 5.024 g/ml

Solution : Given,

Mass of mineral = 41.2 g

Volume of mineral = $8.2cm^3=8.2ml$ $(1cm^3=1ml)$

Formula used :

$Density=\frac{Mass}{Volume}$

Now put all the given values in this formula, we get the density of mineral.

$Density=\frac{41.2g}{8.2ml}=5.02g/ml$

Therefore, the density of a mineral is, 5.024 g/ml

dezoksy [38]3 years ago

4 0

Hey there!:

mass = 41.2 g

Volume = 8.2 cm³

Therefore:

D = m / V

D = 41.2 / 8.2

D = 5.02 g/cm³

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H2(g) + Br2(l) ⇄ 2HBr(g) Kc = 4.8 × 108

elena-14-01-66 [18.8K]

Answer:

1.5 × 10⁻⁹M

Explanation:

1. Equilibrium equation

H₂(g) + Br₂(l) ⇄ 2HBr(g)

2. Equilibrium constant

The liquid substances do not appear in the expression of the equilibrium constant.

$k_c=\dfrac{[HBr(g)]^2}{[H_2]}=4.8\times 10^8M$

3. ICE table.

Write the initial, change, equilibrium table:

Molar concentrations:

H₂(g) + Br₂(l) ⇄ 2HBr(g)

I 0.400 0

C - x +2x

E 0.400 - x 2x

4. Substitute into the expression of the equilibrium constant

$4.8\times 10^8=\dfrac{(2x)^2}{0.400-x}$

5. Solve the quadratic equation

192,000,000 - 480,000,000x = 4x²

x² + 120,000,000x - 48,000,000 = 0

Use the quadratic formula:

$x=\dfrac{-120,000,00\pm\sqrt{(120,000,000)^2-4(1)(-48,000,000}}{2(1)}$

The only valid solution is x = 0.39999999851M

Thus, the final concentration of H₂(g) is 0.400 - 0.39999999851 ≈ 0.00000000149 ≈ 1.5 × 10⁻⁹M

8 0

3 years ago

How would you prepare 500 ml of the following solutions : Sodium succinate buffer (0.1 mol/dm3 pH 5.64)

Nana76 [90]

Answer:

8.10g of sodium succinate must be added and 247mL of 0.1M HCl adding enough water until make 500mL

Explanation:

Succinic acid has a pKa₂ of 5.63

To solve this question we must find the amount of sodium succinate and 0.1M HCl that we have to add using H-H equation:

pH = pKa + log [A-] / [HA]

5.64 = 5.63 + log [Na₂Succ.] / [HSucc⁺]

0.01 = log [Na₂Succ.] / [HSucc⁺]

1.0233 = [Na₂Succ.] / [HSucc⁺] (1)

As:

0.1M = [Na₂Succ.] + [HSucc⁺] (2)

Replacing (2) in (1):

1.0233 = 0.1M - [HSucc⁺] / [HSucc⁺]

1.0233[HSucc⁺] = 0.1M - [HSucc⁺]

2.033[HSucc⁺] = 0.1M

[HSucc⁺] = 0.0494M

[Na₂Succ] = 0.0506M

Both [Na₂Succ⁺] and [HSucc⁺] ions comes from the same sodium succinate we have to find the moles of sodium succinate in 500mL of 0.1M. Then, based on the reaction:

Na₂Succ + HCl → HSucc⁺ + Cl⁻

The moles of HCl added = Moles HSucc⁺ we need:

Moles Na₂Succ:

0.500L * (0.1mol/L) = 0.0500 moles

Mass -Molar mass sodium succinate: 162.05g/mol-:

0.0500mol * (162.05g/mol) = 8.10g of sodium succinate must be added

Moles HCl:

0.0494M * 0.500L = 0.0247 moles HCl * (1L / 0.1mol) = 0.247L =

And 247mL of 0.1M HCl adding enough water until make 500mL

7 0

3 years ago

Convert 15.78 g of H2O2 to mols. Convert 15.3 mols Au to g

iren2701 [21]

Answer:

.46 moles H2O2

3,014 grams Au

Explanation:

H2O2:

15.78g (1 mol/34g) = .46 moles H2O2

Au:

15.3mol (197g/mol) = 3,014 grams Au

8 0

3 years ago

Solve and round to the correct number of significant figures: 129 ÷ 29.20

Scilla [17]

4.42

Because when you divide 129/29.20, you get a long string of numbers. 4.417808219178082...

So you round to the significant figure which in this case is 2 decimal places because 29.20 has 2 decimal places.

PS did you draw that car? Cuz im into drawing cars too.

5 0

3 years ago

In a reaction A+B--->C, reactant A has 5g of product C has 9g of product. How many grams should reactant B contain?

Rzqust [24]

According to the law of conservation of Mass:

In a chemical reaction mass can neither be created nor be destroyed

So, we can say that: Mass of A + Mass of B = Mass of C

In the given reaction,

One of the reactants weigh 5 grams and another one weighs x grams

The mass of the product of this reaction is 9 grams

Mass of reactant B:

Mass of A + Mass of B = Mass of C

5 + x = 9

x = 4 grams

5 0

3 years ago