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2 years ago

Which of the following statements about complete metamorphosis is TRUE?

Chemistry

1 answer:

azamat2 years ago

7 0

ill answer if u answer this FAST

pls and ty brainly.com/question/22200936

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Zn(s) + 2HCl(aq) mc029-1.jpg H2(g) + ZnCl2(aq) Which product is a substance that is dissolved in solution?

nexus9112 [7]

The product that is dissolved in the solution would be the salt zinc chloride. It is a substance that is soluble in water so it should be dissolved in the solution. Also, from the reaction, the sign (aq) is written. It means that this substance is in aqueous solution.

8 0

2 years ago

The amount of resistance to a change in motion an object demonstrates is a direct function of its:

Lelechka [254]

Answer:

Newton second law maybe?

7 0

2 years ago

What is the reason why carbonated beverages be kept cold?

Makovka662 [10]

Option A) Decreased temperature keeps gases like carbon dioxide dissolved.

Carbonation is made with CO2 which is also know as liquid carbonic. The low temperature favors higher solubility of CO2 in water

3 0

2 years ago

A 0.334 g sample of an unknown compound occupies 245 ml at 298 K and 1.22 atm. What is the molar mass of the unknown compound.

marysya [2.9K]

Answer:

27.4 g/mol

Explanation:

Assuming the compound is a gas and that it behaves ideally, we can solve this problem by using the PV=nRT formula, where:

P = 1.22 atm

V = 245 mL ⇒ 245 mL / 1000 = 0.245 L

n = ?

R = 0.082 atm·L·mol⁻¹·K⁻¹

T = 298 K

Inputting the data:

1.22 atm * 0.245 L = n * 0.082 atm·L·mol⁻¹·K⁻¹ * 298 K

Solving for n:

n = 0.0122 mol

With the calculated number of moles and given mass, we calculate the molar mass:

0.334 g / 0.0122 mol = 27.4 g/mol

6 0

2 years ago

Find the pH of a 0.010 M HNO2 solution.

lidiya [134]

Data:
Molar Mass of HNO2
H = 1*1 = 1 amu
N = 1*14 = 14 amu
O = 3*16 = 48 amu
------------------------
Molar Mass of HNO2 = 1 + 14 + 48 = 63 g/mol

M (molarity) = 0.010 M (Mol/L)

Now, since the Molarity and ionization constant has been supplied, we will find the degree of ionization, let us see:
M (molarity) = 0.010 M (Mol/L)
Use: Ka (ionization constant) = $5.0*10^{-4}$
$\alpha^2 (degree\:of\:ionization) = ?$

$Ka = M * \alpha^2$
$5.0*10^{-4} = 0.010* \alpha^2$
$0.010\alpha^2 = 5.0*10^{-4}$
$\alpha^2 = \frac{5.0*10^{-4}}{0.010}$
$\alpha^2\approx500*10^{-4}$

$\alpha\approx\sqrt{500*10^{-4}}$
$\alpha \approx 2.23*10^{-3}$

Now, we will calculate the amount of Hydronium [H3O+] in nitrous acid (HNO2), multiply the acid molarity by the degree of ionization, we will have:

$[ H_{3} O^+] = M* \alpha$
$[ H_{3} O^+] = 0.010* 2.23*10^{-3}$
$[ H_{3} O^+] \approx 0.0223*10^{-3}$
$[ H_{3} O^+] \approx 2.23*10^{-5} \:mol/L$

And finally, we will use the data found and put in the logarithmic equation of the PH, thus:

Data:
log10(2.23) ≈ 0.34
pH = ?
$[ H_{3} O^+] = 2.23*10^{-5}$

Formula:
$pH = - log[H_{3} O^+]$

Solving:
$pH = - log[H_{3} O^+]$
$pH = -log2.23*10^{-5}$
$pH = 5 - log2.23$
$pH = 5 - 0.34$
$\boxed{\boxed{pH = 4.66}}\end{array}}\qquad\quad\checkmark$

Note:. The pH <7, then we have an acidic solution.

6 0

3 years ago