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3 years ago

Which of the following would not be considered a chemical reaction?

Chemistry

1 answer:

ikadub [295]3 years ago

8 0

Answer:

Boiling Water

Explanation:

Physical when water boils, the bubbles are caused by heat, and they are not a new substance — just the same old water, but now, because sufficient heat has been added, it is a gas instead of a liquid. ... If you boil water, it is a physical change because it is still water; it's just water vapor.

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What kind of data would you need to collect to carry out this experiment?

JulijaS [17]

You need to specify the experiment to get an answer. However, most experiments require qualitative data (descriptive, non-numerical data) and quantitative data (measured, numerical data).

4 0

4 years ago

How many grams of sulfuric acid is needed to neutralize 380 ml of solution with pH = 8.94

erma4kov [3.2K]

Answer : The mass of sulfuric acid needed is $16.23\times 10^{-5}g$ .

Solution : Given,

pH = 8.94

Volume of solution = 380 ml = $380\times 10^{-3}$ $(1ml=10^{-3}L)$

Molar mass of sulfuric acid = 98.079 g/mole

As we know,

$pH+pOH=14\\pOH=14-8.94=5.06$

$pOH=-log[OH^-]$

$5.06=-log[OH^-]$

$[OH^-]=0.00000871=8.71\times 10^{-6}mole/L$

Now we have to calculate the moles of $OH^-$ .

Formula used : $Moles=Concentration\times Volume$

$\text{ Moles of }[OH^-]=\text{ Concentration of }[OH^-]\times Volume\\\text{ Moles of }[OH^-]=(8.71\times 10^{-6}mole/L)\times (380\times 10^{-3}L)=3309.8\times 10^{-9}moles$

For neutralization, equal number of moles of $H^+$ ions will neutralize same number of $OH^-$ ions.

$\text{ Moles of }[OH^-]=\text{ Moles of }[H^+]=3309.8\times 10^{-9}moles$

As, $H_2SO_4\rightarrow 2H^++SO^{2-}_4$

From this reaction, we conclude that

2 moles of $H^+$ ion is given by the 1 mole of $H_2SO_4$

$3309.8\times 10^{-9}$ moles of $H^+$ ion is given by $\frac{3309.8\times 10^{-9}}{2}=1654.9\times 10^{-9}$ moles of $H_2SO_4$

Now we have to calculate the mass of sulfuric acid.

Mass of sulfuric acid = Moles of $H_2SO_4$ × Molar mass of sulfuric acid

Mass of sulfuric acid = $(1654.9\times 10^{-9}moles)\times (98.079g/mole)=162310.94\times 10^{-9}=16.23\times 10^{-5}g$

Therefore, the mass of sulfuric acid needed is $16.23\times 10^{-5}g$ .

3 0

3 years ago

When water changes from one state to another each process has a name what are the names of the processes that occur in each stat

Nastasia [14]

Ice, freezing, or melting then liquid evaporation or condensation, the vapor, deposition the ice again

4 0

3 years ago

Read 2 more answers

An alternative definition of electronegativity is Electronegativity= constant (I.E — E.A.) where I.E. is the ionization energy a

Kazeer [188]

Answer:

The electronengativity values of given elements is as follows.

Fluorine - 4

Chlorine -3

Bromine - 2.9

Iodine- 2.5

Explanation:

Electronegativity =consant (I.E-E.A)

The electron affinity and ionization energy values of the given elements is as follows.

(In attachment)

First we have to find the value of constant by using the fluorine atom to whom the electronengativity taken as "4".

Fluorine:

$4=constant[1678-(-327.8)]$

$Constant=0.0019942168$

By using this constant values we can find electronegatvity values of remaining elements.

Chlorine:

$Electronegativity=0.0019942168[1255+348.7]=3.1980\sim 3$

Therefore, electronegativity of chlorine is 3.

Bromine:

$Electronegativity=0.0019942168[1138+324.5]=2.91\sim 2.9$

Therefore, electronegativity of bromine is 2.9.

Iodine:

$Electronegativity=0.0019942168[1007+295.7]=2.59\sim 2.5$

Therefore, electronegativity of iodine is 2.5.

8 0

3 years ago

Hydrogen gas is explosive within the range of 4% - 75% v/v. Assuming that each student in your class produces 6 L of H2 and that

yan [13]

In order to compute this, we must first take a couple of assumptions of:
1) The laboratory size so we can calculate its volume
2) The number of students working in the lab so we know the total gas produced
Let the lab be
11 m × 9 m × 6 m
The volume then computes to be:
594 m³
We know that
1 Liter is 1 dm³
1 m = 10 dm
1 m³ = 1000 dm³
Therefore, the room volume in liters is:
594,000 Liters
Let there be 30 students in the laboratory
Total gas being produced:
6 × 30
= 180 Liters
This works out to be:
0.03% of Hydrogen by volume
Therefore, there is no risk of explosion given our assumption of size and students.

5 0

3 years ago