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3 years ago

How many moles of hcl are required to neutralize aqueous solutions of these bases:

2 answers:

8 0

The answers are a.) 0.03 mol KOH requires 0.03 mol HCl, b.) 2 mol NH3 requires 2 mol HCl and c.) 0.1 mol Ca(OH)2 requires 0.2 mol HCl.
Solution:
We need to write the balanced equations for each reactions to find out the stoichiometry for each reactants.
a.) HCl (aq) + KOH (aq) → KCl (aq) + H2O(ℓ)
From the balanced equations, we can see that 1 HCl reacts with 1 KOH, therefore if 0.03 mol KOH is reacted then 0.03 mol HCl must also be present.

b.) HCl(aq) + NH3(aq) ) → NH4Cl(aq)
If 2 moles of NH3 are reacted then 2 moles of HCl must also be present since 1 HCl reacts with 1 NH3 from the balanced reaction.

c.) 2HCl(aq) + Ca(OH)2(s) → CaCl2(aq) + 2H2O(ℓ)
We can see that 2 HCl react with 1 Ca(OH)2, hence if 0.1 mol of Ca(OH)2 is reacted then 0.2 mol HCl must also be present.

MatroZZZ [7]3 years ago

6 0

A) Chemical reaction: KOH + HCl → KCl + H₂O.
n(HCl) : n(KOH) = 1 : 1.
n(HCl) = 0.03 mol.
b) Chemical reaction: HCl + NH₃ → NH₄Cl.
n(HCl) : n(NH₃) = 1 : 1.
n(HCl) = 2 mol.
c) Chemical reaction: Ca(OH)₂ + 2HCl → CaCl₂ + 2H₂O.
n(HCl) : n(Ca(OH)₂) = 2 : 1.
n(HCl) = 0.2 mol.

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2 years ago

Given the following reaction: 2N2O5=2N2O4+O2, if the rate of oxygen production is 0.15M/min, determine:

astraxan [27]

Answer:

a. $r_{N_2O_5}=-0.075M/min$

b. $r_{N_2O_4}=0.075M/min$

Explanation:

Hello.

In this case, according to the balanced chemical reaction, we can write the law of rate proportions:

$\frac{r_{N_2O_5}}{-2} =\frac{r_{N_2O_4}}{2} =\frac{r_{O_2}}{1}$

Thus, we proceed as follows:

a. Since the rate of oxygen production is 0.15 M/min, we can make the following setup:

$\frac{r_{N_2O_5}}{-2} =\frac{r_{O_2}}{1}\\\\r_{N_2O_5}=\frac{r_{O_2}}{-2} =\frac{0.15M/min}{-2}\\\\ r_{N_2O_5}=-0.075M/min$

b. Since the rate of oxygen production is 0.15 M/min, we can make the following setup:

$\frac{r_{N_2O_4}}{2} =\frac{r_{O_2}}{1}\\\\r_{N_2O_4}=\frac{r_{O_2}}{2} =\frac{0.15M/min}{2}\\\\ r_{N_2O_4}=0.075M/min$

Best regards!

8 0

3 years ago

A chemist determines by measurements that 0.0200 moles of chlorine gas participate in a chemical reaction. Calculate the mass of

Schach [20]

Answer:

1.4200 g

Explanation:

The chlorine gas has a molecular formula Cl2. In table periodic, the molar mass of one atom of chlorine is 35.5 g/mol, so the molar mass of Cl2 is 71 g/mol.

Molar mass, mass and number of moles are related by the equation below:

$n = \frac{m}{MM}$

Where n is the number of moles, m is the mass, and MM is the molar mass of the compound.

So, for 0.0200 moles of Cl2 produced:

$0.0200 = \frac{m}{71}$

m = 71x0.0200

m = 1.4200

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4 years ago

A pure sample of a new chemical compound was analyzed and was found to have the following mass percentages: Al 31.5 %; O 56.1 %;

rjkz [21]

Answer:

The answer to your question is empirical formula Al₃O₉S

Explanation:

Data

Al = 31.5 %

O = 56.1 %

S = 12.4 %

Process

1.- Look for the atomic masses of the elements

Al = 27 g

O = 16

S = 32

2.- Represent the percentages as grams

Al = 31.5 g

O = 56.1 g

S = 12.4 g

3.- Convert these masses to moles

27 g of Al ----------------- 1 mol

31.5 g ---------------------- x

x = 1.17 moles

16 g of O ---------------- 1 mol

56.1 g of O ------------- x

x = 3.5 mol

32 g of S --------------- 1 mol

12.4 g of S ------------- x

x = 0.39 moles

4.- Divide by the lowest number of moles

Al = 1.17 / 0.39 = 3

O = 3.5 / 0.39 = 8.9 ≈ 9

S = 0.39 / 0.39 = 1

5.- Write the empirical equation

Al₃O₉S

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3 years ago