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2 years ago

10

A gaseous compound has a density of 1.90 g/L at 51.1 ∘C and 1.09 bar . Assuming ideal behavior, calculate the molar mass of the

gas.

1 answer:

marysya [2.9K]2 years ago

5 0

Answer:

1.90

Explanation:

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HOCl dissociative into which 2 ions

trasher [3.6K]

Answer:

H+ and OCl-

Since this is an acid, the H+ will come off and what is left OCl- is the other part.

3 0

3 years ago

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Artist 52 [7]

Conductor = Radiator , Frying pan , Ceramic baking dish
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5 0

3 years ago

The correct answer for the addition of 5.8 g + 2.26g + 1.311g + 2 g is?

jeka94

Answer:

= 11.371g

Explanation:

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4 0

3 years ago

What is the concentration of a solution in which 10.0 g of AgNO3 is dissolved in 500 mL of solution?

Zigmanuir [339]

molar concentration of AgNO₃ solution = 0.118 mole/L

Explanation:

Because we have the volume of the solution and there is no information about the density of the solution I will asume that you ask for the molar concentration.

number of moles = mass / molecular weight

number of moles of AgNO₃ = 10 / 170 = 0.0588

molar concentration = number of moles / volume (L)

molar concentration of AgNO₃ solution = 0.0588 / 0.5

molar concentration of AgNO₃ solution = 0.118 mole/L

Learn more about:

molar concentration

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6 0

3 years ago

Purification of nickel can be achieved by electrorefining nickel from an impure nickel anode onto a pure nickel cathode in an el

Alexxandr [17]

Answer: 530 hours

Explanation:

The reduction of Nickel ions to nickel is shown as:

$Ni^{2+}+2e^-\rightarrow Ni$

$96500\times 2=193000Coloumb$ of electricity deposits 1 mole of Nickel

1 mole of Nickel weighs = 58.7 g

Given quantity = 18.0 kg = 18000 g (1kg=1000g)

58.7 g of Nickel is deposited by 193000 C of electricity

18000 g of Nickel is deposited by = $\frac{193000}{58.7}\times 18000=59182282.8C$ of electricity

$Q=I\times t$

where Q= quantity of electricity in coloumbs = 59182282.8C

I = current in amperes = 31.0 A

t= time in seconds = ?

$59182282.8C=31.0A\times t$

$t=1909105.9sec$

(1h=3600 sec)

$t=530hours$

Thus 530 hours are required to plate 18.0 kg of nickel onto the cathode if the current passed through the cell is held constant at 31.0 A

3 0

3 years ago