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3 years ago

Is Dry Ice a pure substance or a Mixture ?

Chemistry

1 answer:

r-ruslan [8.4K]3 years ago

3 0

Answer:

Dry Ice is a pure substance.

Explanation:

Dry Ice is the solid form of Carbon Dioxide which is formed when gaseous Carbon Dioxide molecules sublime at very low temperatures (-109.5 Fahrenheit).

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Como puedo clasificarlos

EastWind [94]

<em>Que quieres clasificar?.... Yo te puedo ayudar si quieres pero dime que quieres clasificar.</em>

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2 years ago

Fter a radioactive atom decays, it is the same element that it was before with no measurable change in mass. Which kind of decay

Alborosie

After a radioactive atom decays, it is the same element that it was before with no measurable change in mass. the decay that is present is gamma decay because gamma decay has photons which has no mass unlike alpha and beta decay.

6 0

2 years ago

Read 2 more answers

Calculate the solubility of CaF2 in g/L (Ksp = 4.0 x 10-8). 2. What is the pH of a solution containing a hydrogen ion concentrat

Pepsi [2]

Answer:

$\large \boxed{1. \text{ 0.17 g/L; 2. 3.52; 3. Cl; 4. (a) +3; (b) +4; (c) +6}}$

Explanation:

1. Solubility of CaF_2

(a) Molar solubility

CaF₂ ⇌ Ca²⁺ + 2F⁻

$K_{\text{sp }} = \text{[Ca$^{2+}$]}\text{[F$^{-}$]}^{2}= 4.0 \times 10^{-8}\\s(2s)^{2}=4.0 \times 10^{-8}\\4s^{3} = 4.0 \times 10^{-8}\\s^{3} = 1.0 \times 10^{-8}\\s =2.2 \times 10^{-3}\text{ mol/L}$

(b) Mass solubility

$\text{Solubility} = 2.2 \times 10^{-3} \text{ mol/L} \times \dfrac{\text{78.07 g}}{\text{1 L }} = \text{0.17 g/L}\\\\\text{The solubility of CaF$_{2}$ is $\large \boxed{\textbf{0.17 g/L}}$}$

2. pH

pH = -log [H⁺] = -log(3.0 × 10⁻⁴) = 3.52

3. Oxidizing and reducing agents

Zn + Cl₂ ⟶ ZnCl₂

$\rm \stackrel{\hbox{0}}{\hbox{Zn}} + \stackrel{\hbox{0}}{\hbox{ Cl}_{2} }\longrightarrow \stackrel{\hbox{+2}}{\hbox{Zn}}\stackrel{\hbox{-1}}{\hbox{Cl}_{2}}$

The oxidation number of Cl has decreased from 0 to -1.

Cl has been reduced, so Cl is the oxidizing agent.

4. Oxidation numbers

(a) Al₂O₃

$\stackrel{\hbox{$\mathbf{+3}$}}{\hbox{Al}_{2}}\stackrel{\hbox{-2}}{\hbox{O}_{3}}$

1O = -2; 3O = -6; 2Al = +6; 1Al = +3

(b) XeF₄

$\stackrel{\hbox{$\mathbf{+4}$}}{\hbox{Xe}}\stackrel{\hbox{-1}}{\hbox{F}_{4}}$

1F = -1; 4F = -4; 1 Xe = +4

(c) K₂Cr₂O₇

$\stackrel{\hbox{${+1}$}}{\hbox{K}_{2}}\stackrel{\hbox{$\mathbf{+6}$}}{\hbox{Cr}_{2}}\stackrel{\hbox{-2}}{\hbox{O}_{7}}$

1K = +1; 2K = +2; 1O = -2; 7O = -14

+2 - 14 = -12

2Cr = + 12; 1 Cr = +6

8 0

3 years ago

If the theoretical yield of RX is 56.0 g , what is the percent yield ?

maks197457 [2]

the complete question in attached figure

Let
x------------------- > actual yield
y------------------- > theoretical yield
z------------------- > percent yield
we have that
z=x/y

we know
x=47 g
y=56 g

therefore

z=47/56=0.839 ---------------- > 83.9%

the answer is the option C 83.9%

4 0

3 years ago

How many molecules are in 5 moles of C10H210?

Pavlova-9 [17]

Answer:

3.0 x 10²⁴molecules

Explanation:

Given parameters:

Number of moles of compound = 5moles

Unknown:

Number of molecules = ?

Solution:

A mole is substance that contains the Avogadro's number of particles;

1 mole = 6.02 x 10²³ molecules

5 moles of the compound will give 5 x 6.02 x 10²³ molecules

= 3.0 x 10²⁴molecules

3 0

2 years ago