All categories

3 years ago

Which element is least likely to undergo a chemical reaction

Chemistry

1 answer:

Maksim231197 [3]3 years ago

6 0

Answer:

Neon is the least likely to undergo chemical reaction.

Explanation:

The other elements given in the option do not have 8 electrons in their outermost shell, so they will be quite willing to undergo chemical reactions in order to become stable.

You might be interested in

Taro is a _______ meaning that it was brought to the hawaiian islands by boat

harkovskaia [24]

Are there any options to choose from?

3 0

3 years ago

A chemical reaction has Hf,reactants = –1,023 kJ and Hf,products = –935.3 kJ. Which graph can be used to represent this reaction

natita [175]

Hey there!

The pathway will resemble a hill , The minimum amount of energy the reagents need to make the complex activated, is the activation energy , The difference in heights of the products and reactants will be equivalent to the difference in energies.:

ΔH = ( -1,023 kj ) - ( - 935,3 kj )

ΔH = -87.7 Kj

7 0

4 years ago

Read 2 more answers

Please help

Jet001 [13]

Answer:

they are tinyb particles

Explanation:

8 0

3 years ago

The equilibrium constant Kp for the reaction I2(g) + Br2(g) ⇀↽ 2 IBr(g) + 11.7 kJ is 280 at 150◦C. Suppose that a quantity of IB

mixas84 [53]

Answer:

$\large \boxed{\text{0.0120 atm }}$

Explanation:

The balanced equation is

I₂(g) + Br₂(g) ⇌ 2IBr(g)

Data:

Kp = 280

p(IBr) = 0.200 atm

1. Set up an ICE table.

Let p = the initial pressure of IBr. Then

$\begin{array}{ccccccc}\rm \text{I}_{2}& + & \text{Br}_{2} & \, \rightleftharpoons \, & \text{2IBr} & & \\0 & & 0 & & p & & \\+x & & +x & & -2x & &\\x & & x} & & 280 & & \\\end{array}$

2. Calculate p(I₂)

$\begin{array}{rcl}K_{\text{p}}&=&\dfrac{p_{\text{IBr}}^{2}} {p_{\text{I}_2}^{2}}\\\\280&=&{\dfrac{0.200^{2}}{x^{2}}&&\\\\280x^{2} & = &0.0400\\x^{2} & = &\dfrac{0.0400}{280 }\\\\& = & 1.429 \times 10^{-4}\\x & = & \textbf{0.0120 atm}\\\end{array}\\\text{The partial pressure of iodine is $\large \boxed{\textbf{0.0120 atm }}$}$ }

Check:

$\begin{array}{rcl}{\dfrac{0.200^{2}}{0.0120^{2}}}&=&280\\\\280& =& 280\\\end{array}$

8 0

3 years ago

Consider the reaction:

Fofino [41]

The mass in grams of NH₃ produced from the reaction is 3.4 g

<h3>Balanced equation</h3>

We'll begin by writing the balanced equation for the reaction. This illustrated below:

N₂ + 3H₂ -> 2NH₃

From the balanced equation above,

1 dm³ of N₂ reacted to produced 2 dm³ NH₃

<h3>How to determine the volume of NH₃ produced</h3>

From the balanced equation above,

1 dm³ of N₂ reacted to produced 2 dm³ NH₃

Therefore,

2.24 dm³ of N₂ will react to produce = 2.24 × 2 = 4.48 dm³ of NH₃

<h3>How to determine the mass of NH₃ produced</h3>

We'll begin by obtained the mole of 4.48 dm³ of NH₃. Details below:

22.4 dm³ = 1 mole NH₃

Therefore,

4.48 dm³ = 4.48 / 22.4

4.48 dm³ = 0.2 mole of NH₃

Finally, we shall determine the mass of NH₃ as follow:

Molar mass of NH₃ = 17 g/mol
Mole of NH₃ = 0.2 mole
Mass of NH₃ =?

Mass = mole × molar mass

Mass of NH₃ = 0.2 × 17

Mass of NH₃ = 3.4 g

Learn more about stoichiometry:

brainly.com/question/13196642

#SPJ1

4 0

1 year ago