The density of lead is 11.3 g/mL. What is the mass of 45 mL of the metal?

How many particles can be stored in a 4.0 L container at room temperature (23 C) and standard atmospheric pressure

velikii [3]

Answer: 9.91×10²³ particles

Explanation:

To find the amount of particles, you will need to use the Ideal Gas Law with what we are given.

Ideal Gas Law: PV=nRT

After we find moles, we can use Avogadro's number to convert to particles.

$n=\frac{PV}{RT}$

P=101.3kPa=1.00 atm

V=4.0 L

T=23°C+273.15=296.15 K

R=0.08206 Latm/Kmol

$n=\frac{(1.00 atm)(4.0 L)}{(0.08206Latm/Kmol)(296.15K)}$

$n=0.164595 mol$

Now that we have moles, we can convert to particles.

$0.164595mol*\frac{6.022*10^2^3 particles}{mol} =9.91*10^2^2 particles$

5 0

3 years ago

HELP ME! If I get an F on my test I’m getting kicked out:(

satela [25.4K]

Answer:

It is just slightly less abundant than its alkali cousin, sodium. Potassium is less dense than water, so it can float on water. However, chemically, potassium reacts with water violently. It will give off hydrogen and eventually catch fire.

3 0

3 years ago

Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the following electron transfe

Vesna [10]

Answer:

In the given chemical reaction:

Species Oxidized: I⁻

Species Reduced: Fe³⁺

Oxidizing agent: Fe³⁺

Reducing agent: I⁻

As the reaction proceeds, electrons are transferred from I⁻ to Fe³⁺

Explanation:

Redox reaction is a chemical reaction involving the simultaneous movement of electrons thereby causing oxidation of one species and reduction of the other species.

The chemical species that gets reduced by gaining electrons is called an oxidizing agent. Whereas, the chemical species that gets oxidized by losing electrons is called a reducing agent.

Given redox reaction: 2Fe³⁺ + 2I⁻ → 2Fe²⁺ + I₂

Oxidation half-reaction: 2 I⁻ + → I₂ + 2 e⁻ ....(1)

Reduction half-reaction: [ Fe³⁺ + 1 e⁻ → Fe²⁺ ] × 2

⇒ 2 Fe³⁺ + 2 e⁻ → 2 Fe²⁺ ....(2)

In the given redox reaction, Fe³⁺ (oxidation state +3) accepts electrons and gets reduced to Fe²⁺ (oxidation state +2) and I⁻ (oxidation state -1) loses electrons and gets oxidized to I₂ (oxidation state 0).

Therefore, Fe³⁺ is the oxidizing agent and I⁻ is the reducing agent and the electrons are transferred from I⁻ to Fe³⁺.

5 0

4 years ago

As the concentration of a KOH solution increases, the number of moles of HCl needed to neutralize the KOH solution?

Soloha48 [4]

B) increasesAnswer:

Explanation:

8 0

3 years ago

A flashbulb of volume 2.70 mL contains O2(g) at a pressure of 2.30 atm and a temperature of 30.0 °C. How many grams of O2(g) doe

Sholpan [36]

P = 2.30 atm

Volume in liter = 2.70 mL / 1000 => 0.0027 L

Temperature in K = 30.0 + 273 => 303 K

R = 0.082 atm

molar mass O2 = 31.9988 g/mol

number of moles O2 :

P * V = n * R* T

2.30 * 0.0027 = n * 0.082 * 303

0.00621 = n * 24.846

n = 0.00621 / 24.846

n = 0.0002499 moles of O2

Mass of O2:

n = m / mm

0.0002499 = m / 31.9988

m = 0.0002499 * 31.9988

m = 0.008 g

3 0

4 years ago