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2 years ago

PC13 ionic or covalent

Chemistry

1 answer:

Juli2301 [7.4K]2 years ago

5 0

Answer:

The bond between Phosphorus and Chlorine in PCl3 is covalent as chlorine needs one electron and phosphorus has metallic character and easily donate electron

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Balance the following redox reaction by inserting the appropriate coefficients. SO4^2- + NH3 = SO3^2- + H2O + N2

Harlamova29_29 [7]

SO₄²⁻ +NH₃ → SO₃²⁻ + H₂O +N₂

The balanced of the above redox reaction is as below

3SO₄²⁻ + 2NH₃ → 3SO₃²⁻ + 3 H₂O + N₂

Explanation

According to the law of mass conservation the number of atoms in the reactant side must be equal to number of atoms in product side.

Inserting coefficient 3 in front of SO₄² , 2 in front of NH₃, 3 in front of SO₃²⁻ and 3 in front of H₂O balance the equation above. This is because the number of atoms are equal in both side.

for example there are 2 atoms of N in both side of the reaction.

6 0

3 years ago

Read 2 more answers

What material was added to powdered rock during tuttle and bowen's experiments?

Rzqust [24]

Answer:

water was added to powdered rock

Explanation:

4 0

3 years ago

How many moles of neon atoms are there in a neon sign that has 2.4 * 20^ 24 atoms of neon? *

Whitepunk [10]

Answer:

4 moles of neon

Explanation:

Given data:

Number of moles of neon = ?

Number of atoms of neon = 2.4×10²⁴ atoms

Solution:

The given problem will solve by using Avogadro number.

It is the number of atoms , ions and molecules in one gram atom of element, one gram molecules of compound and one gram ions of a substance.

The number 6.022 × 10²³ is called Avogadro number.

For example,

18 g of water = 1 mole = 6.022 × 10²³ molecules of water

1.008 g of hydrogen = 1 mole = 6.022 × 10²³ atoms of hydrogen

For given neon atoms:

1 mol = 6.022 × 10²³ atoms

2.4×10²⁴ atoms × 1 mol / 6.022 × 10²³ atoms

0.4×10¹ mol = 4 mol

3 0

3 years ago

How many moles of HCl are in 30.00mL of a 0.1000M HCl solution? A. 0.003000mol. B. 300.0mol C. 0.03000mol D. 3.000mol

Katyanochek1 [597]

Given the volume of HCl solution = 30.00 mL

Molarity of HCl solution = 0.1000 M

Molarity, moles and volume are related by the equation:

Molarity = $\frac{Moles of solute}{Volume of solution (L)}$

Converting volume of HCl from mL to L:

$30.00 mL * \frac{1 L}{1000mL}=0.030000 L$

Calculating moles of HCl from volume in L and molarity:

$0.03000 L * \frac{0.1000mol}{L}= 0.003000 mol HCl$

The final moles would be reported to 4 sig figs. So the correct answer will be 0.03000 mol HCl

Correct option: C. 0.03000mol

7 0

3 years ago

The true absorbance for a 1.0 x 10 −5 M solution is 0.7526. If the percentage stray light for a spectrophotometer is 0.56%, calc

Korvikt [17]

Answer:

The percentage deviation is $\Delta M = 1.87$ %

Explanation:

From the question we are told that

The concentration is of the solution is $C = 1.0*10^{-5} M$

The true absorbance A = 0.7526

The percentage of transmittance due to stray light $z = 0.56$ % $=\frac{0.56}{100} = 0.0056$

Generally Absorbance is mathematically represented as

$A = -log T$

Where T is the percentage of true transmittance

Substituting value

$0.7526 = - log T$

$T = 10^{-0.7526}$

$= 0.177$

$= 17.7$ %

The Apparent absorbance is mathematically represented

$A_p = -log (T +z)$

Substituting values

$A_p = -log(0.177 + 0.0056)$

$= -log(0.1826)$

= 0.7385

The percentage by which apparent absorbance deviates from known absorbance is mathematically evaluated as

$\Delta A = \frac{A -A_p}{A} * \frac{100}{1}$

$= \frac{0.7526 - 0.7385}{0.7526} * \frac{100}{1}$

$\Delta A = 1.87$ %

Since Absorbance varies directly with concentration the percentage deviation of the apparent concentration from know concentration is

$\Delta M = 1.87$ %

6 0

4 years ago