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2 years ago

Consider the reaction below.

Chemistry

2 answers:

gtnhenbr [62]2 years ago

6 0

Answer:

The correct answer is:

Explanation:

It is right on edge

Svetradugi [14.3K]2 years ago

5 0

Answer:

Na+ Cl- to NaCL

Explanation:

Both Na and Cl do not interact with the full formula

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Tanks of compressed gas must be kept away from heat sources. If a compressed–gas tank is heated too much, it may explode and cau

scoundrel [369]

If it is heated while it is being compressed or held inside a container as such, the pressure build up while in the container and the pressure can become so much that the container will burst.

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2 years ago

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Write the lewis structure for ch2clcoo−. assign a formal charge for any atom with a non-zero formal charge.

Murljashka [212]

The Lewis structure of Chloroacetate (H₂CClCO₂) is given below. In structure it is shown that carbon has a double bond with one oxygen atom and two single bonds with CH₂Cl and O⁻.

Formal Charge;
Formal charge is caculated as,

Formal charge = # of valence e⁻ - [# of lone pair of e⁻ + 1/2 # of bonded e⁻]

Formal charge on Oxygen (Highlighted Red);

Formal charge = 6 - [ 6 + 2/2]

Formal charge = 6 - [6 + 1]

Formal charge = 6 - [7]

Formal charge = -1

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2 years ago

If you gently shake a carbon dioxide fire extinguisher, you will feel the presence of liquid within the extinguisher What condit

scoundrel [369]

When we wish to convert a gas to liquid we have to either

a) decrease temperature

b) increase pressure

In case of fire extinguisher the CO2 is found to be in liquid state, this is as the CO2 is pressurized at high pressure which keeps CO2 in liquid state

the ideal pressure and temperature conditions when CO2 gas can be converted to CO2 gas

Pressure = 5 - 73 atm

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2 years ago

Calculate the amount, in moles, of PO43- present at equilibrium when excess Sr3(PO4)2 is added to 750. mL 1.2 M Sr(NO3)2(aq). As

Crank

Answer:

1.8 × 10⁻¹⁶ mol

Explanation:

(a) Calculate the solubility of the Sr₃(PO₄)₂

Let s = the solubility of Sr₃(PO₄)₂.

The equation for the equilibrium is

Sr₃(PO₄)₂(s) ⇌ 3Sr²⁺(aq) + 2PO₄³⁻(aq); Ksp = 1.0 × 10⁻³¹

1.2 + 3s 2s

$K_{sp} =\text{[Sr$^{2+}$]$^{3}$[PO$_{4}^{3-}$]$^{2}$} = (1.2 + 3s)^{3}\times (2s)^{2} = 1.0 \times 10^{-31}\\\text{Assume } 3s \ll 1.2\\1.2^{3} \times 4s^{2} = 1.0 \times 10^{-31}\\6.91s^{2} = 1.0 \times 10^{-31}\\s^{2} = \dfrac{1.0 \times 10^{-31}}{6.91} = 1.45 \times 10^{-32}\\\\s = \sqrt{ 1.45 \times 10^{-32}} = 1.20 \times 10^{-16} \text{ mol/L}\\$

(b) Concentration of PO₄³⁻

[PO₄³⁻] = 2s = 2 × 1.20× 10⁻¹⁶ mol·L⁻¹ = 2.41× 10⁻¹⁶ mol·L⁻¹

(c) Moles of PO₄³⁻

Moles = 0.750 L × 2.41 × 10⁻¹⁶ mol·L⁻¹ = 1.8 × 10⁻¹⁶ mol

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2 years ago

What is the limiting reactant for the reaction below given that you start with 10.0 grams of Al (molar mass 26.98 g mol-1) and 1

mezya [45]

Answer:

Explanation:

4 Al + 3 O₂ → 2 Al₂O₃

You need to figure out which one has the smaller mole ratio. Convert both substances from grams to moles.

(10.0 g Al)/(26.98 g/mol) = 0.3706 mol Al

(19.0 g O₂)/(32.00 g/mol) = 0.5938 mol O₂

Now, use the mole ratios of reactant to product to see which substance produces the least amount of product.

(0.3706 mol Al) × (2 mol Al₂O₃/4 mol Al) = 0.1853 mol Al₂O₃

(0.5938 mol O₂) × (2 mol Al₂O₃/3 mol O₂) = 0.3958 mol Al₂O₃

Since aluminum produces the least amount of product, this is the limiting reagent.

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2 years ago