A very small electronegativity difference leads to a:

Use the following equation to answer question 1-4. Make sure you balance first.

worty [1.4K]

<h3>Answer:</h3>

5.2 mol H₂O

<h3>General Formulas and Concepts:</h3>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

Brackets
Parenthesis
Exponents
Multiplication
Division
Addition
Subtraction

Left to Right

<u>Chemistry</u>

<u>Stoichiometry</u>

Using Dimensional Analysis

<h3>Explanation:</h3>

<u>Step 1: Define</u>

[RxN - Balanced] 6HCl + Fe₂O₃ → 2FeCl₃ + 3H₂O

[Given] 10.4 mol HCl

<u>Step 2: Identify Conversions</u>

[RxN] 6 mol HCl = 3 mol H₂O

<u>Step 3: Stoichiometry</u>

Set up: $\displaystyle 10.4 \ mol \ HCl(\frac{3 \ mol \ H_2O}{6 \ mol \ HCl})$
Multiply/Divide: $\displaystyle 5.2 \ mol \ H_2O$

4 0

3 years ago

How do I complete and balance this chemical equation?

GalinKa [24]

I’m I’m pretty sure this is a combustion reaction, so that means the products would be CO2 + H2O.

6 0

4 years ago

For the first order process: AB The half-life of A is 62.1 seconds. If a sample of A initially has 250.0 g, what mass (in g) of

vodomira [7]

<u>Answer:</u> The mass of sample A after given time is 99.05 g.

<u>Explanation:</u>

All the radioactive reactions follows first order kinetics.

The equation used to calculate half life for first order kinetics:

$t_{1/2}=\frac{0.693}{k}$

We are given:

$t_{1/2}=62.1s$

Putting values in above equation, we get:

$k=\frac{0.693}{62.1}=0.011s^{-1}$

Rate law expression for first order kinetics is given by the equation:

$k=\frac{2.303}{t}\log\frac{[A_o]}{[A]}$

where,

k = rate constant = $0.011s^{-1}$

t = time taken for decay process = 84.2 s

$[A_o]$ = initial amount of the reactant = 250 g

[A] = amount left after decay process = ?

Putting values in above equation, we get:

$0.011s^{-1}=\frac{2.303}{84.2s}\log\frac{250}{[A]}$

$[A]=99.05g$

Hence, the mass of sample A after given time is 99.05 g.

8 0

3 years ago

1s22s22p63s33p4 is the electron configuration of ??

Len [333]

It’s chlorine (Cl) having the atomic number 17

4 0

3 years ago

`One way to make ammonia is to synthesize it directly from elemental nitrogen and hydrogen (though this isn't that easy). The eq

White raven [17]

Answer: A. 1.5 g

Explanation:

$N_2+3H_2\rightarrow 2NH_3$

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

$\text{Number of moles of nitrogen}=\frac{7.0g}{28g/mol}=0.25 moles$

According to stoichiometry:

1 mole of $N_2$ requires = 3 moles of $H_2$

Thus 0.25 moles of $N_2$ will require = $\frac{3}{1}\times 0.25=0.75moles$ of $H_2$

Mass of $H_2$ required = $moles\times {\text {Molar mass}}=0.75mol\times 2g/mol=1.5g$

The minimum amount of $H_2$ in grams that would be required to completely react with this amount of $N_2$ is 1.5 grams.

7 0

3 years ago

Read 2 more answers