Atoms of which of the following elements have the smallest atomic radius?

3Al + 3NH4ClO4 → Al2O3 + AlCl3 + 3NO + 6H2O<br> How many moles of AlCl3 are produced?

zhuklara [117]

Answer: 1 mol of $AlCl_3$ will be produced from this reaction.

Explanation: Reaction follows,

$3Al+3NH_4ClO_4\rightarrow Al_2O_3+AlCl_3+3NO+6H_2Oc$

As seen from the balanced chemical equation above, we get

For every 3 moles of Aluminium and 3 moles of $NH_4ClO_4$ , 1 mole of $Al_2O_3$ is formed.

For every 3 moles of Aluminium and 3 moles of $NH_4ClO_4$ , 1 mole of $AlCl_3$ is formed.

For every 3 moles of Aluminium and 3 moles of $NH_4ClO_4$ , 3 moles of $NO$ is formed.

For every 3 moles of Aluminium and 3 moles of $NH_4ClO_4$ , 6 moles of $H_2O$ is formed.

7 0

4 years ago

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How do particles move when they are changing phases?

Arisa [49]

They speed up when they get hotter and they slow down when they get colder. I think

6 0

3 years ago

This is for girls only!!!!!! if you are a boy go away

Sladkaya [172]

Money so i can get a nice body with the money hahah

4 0

3 years ago

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f the Ksp for HgBr2 is 2.8×10−14, and the mercury ion concentration in solution is 0.085 M, what does the bromide concentration

goldfiish [28.3K]

Answer:

0.057 M

Explanation:

Step 1: Given data

Solubility product constant (Ksp) for HgBr₂: 2.8 × 10⁻⁴

Concentration of mercury (II) ion: 0.085 M

Step 2: Write the reaction for the solution of HgBr₂

HgBr₂(s) ⇄ Hg²⁺(aq) + 2 Br⁻

Step 3: Calculate the bromide concentration needed for a precipitate to occur

The Ksp is:

Ksp = 2.8 × 10⁻⁴ = [Hg²⁺] × [Br⁻]²

[Br⁻] = √(2.8 × 10⁻⁴/0.085) = 0.057 M

7 0

3 years ago

Sodas are made fizzy by the carbon dioxide ( CO ) dissolved in the liquid. An amount of carbon 2 dioxide equal to about 8.0 L of

eduard

Answer:

A) The number of moles of Carbon dioxide in 2.0 L bottle of soda = 0.325 mole

B) The mass of Carbon dioxide in 2.0 L bottle of soda = 14.3 g

Explanation:

Complete Question

Soda are made fizzy by the carbon dioxide (CO₂) dissolved int he liquid. An amount of carbon dioxide equal to about 8.0 L of carbon dioxide gas at atmospheric pressure and 300.0 K can be dissolved can be dissolved in a 2-L bottle of soda. The molar mass of CO₂ IS 44 g/mol.

A) How many moles of carbon dioxode are in the 2-L? (1L = 0.001 m³)

B) What is the mass of the carbon dioxide in the 2-L bottle of soda?

Solution

Assuming that CO₂ is an ideal gas.

A) The amount of carbon dioxide in 2.0 L of soda bottle is equal to the amount of Carbon dioxide in about 8.0 L of carbon dioxide gas at atmospheric pressure and 300.0 K

From the ideal gas equation, we know that

PV = nRT

P = pressure of the gas = atmospheric pressure = 101,325 Pa

V = volume of the gas = 8.0 L = 0.008 m³

n = number of moles of the ideal gas = ?

R = molar gas constant = 8.314 J/mol.K

T = absolute temperature of the gas in Kelvin = 300 K

101325 × 0.008 = n × 8.314 × 300

n = (101325×0.008) ÷ (8.314 × 300)

n = 0.324993986 = 0.325 mole of Carbon dioxide.

B) The mass of Carbon dioxide in 2.0 L bottle of soda

Mass = (Number of moles) × (Molar mass)

= 0.325 × 44.0

= 14.3 g

Hope this Helps!!!

7 0

3 years ago