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3 years ago

Amning At Home -Chemisu

Chemistry

1 answer:

levacccp [35]3 years ago

4 0

Answer:first one: 3.0g second one: 10g H2O(I)

Explanation:

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What Is the answers?

Yuki888 [10]

Answer:

oxygen is responsible for rusting

5 0

2 years ago

Read 2 more answers

How many atoms are there in 7.80 moles of germanium

Orlov [11]

<h3>Answer:</h3>

4.70 × 10²⁴ atoms Ge

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

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

Brackets
Parenthesis
Exponents
Multiplication
Division
Addition
Subtraction

Left to Right

<u>Chemistry</u>

<u>Atomic Structure</u>

Using Dimensional Analysis
Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.

<h3>Explanation:</h3>

<u>Step 1: Define</u>

7.80 mol Ge

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

Avogadro's Number

<u>Step 3: Convert</u>

$\displaystyle 7.80 \ mol \ Ge(\frac{6.022 \cdot 10^{23} \ atoms \ Ge}{1 \ mol \ Ge} )$ = 4.69716 × 10²⁴ atoms Ge

<u>Step 4: Check</u>

<em>We are given 3 sig figs. Follow sig fig rules and round.</em>

4.69716 × 10²⁴ atoms Ge ≈ 4.70 × 10²⁴ atoms Ge

8 0

2 years ago

Scenario: You are testing two different

chubhunter [2.5K]

Answer:1 × 10-8 M

Explanation:

5 0

3 years ago

Read 2 more answers

What are the empirical and molecular formulas of a hydrocarbon if combustion of 2.10 g of the compound yields 6.59 g co2 and 2.7

mariarad [96]

The empirical formula of hydrocarbon is CH2

The molecular formula of the hydrocarbon is C6H12

<u><em>Explanation</em></u>

Hydrocarbon is made up of carbon and hydrogen

<h3><u><em> </em></u>Empirical formula calculation</h3>

Step 1: find the moles CO2 and H2O

moles =mass/molar mass

moles of CO2 = 6.59 g/ 44 g/mol = 0.15 moles

moles of H2O = 2.70 g / 18 g/mol = 0.15 moles

Step 2: Find the moles ratio of Co2:H2O by diving each mole by smallest mole(0.15)

that is for CO2 = 0.15/0.15 =1

For H2O = 0.15/0.15 =1

therefore the mole ratio of Co2 : H2O = 1:1 which implies that 1 mole of Co2 and 1 mole of H2O is formed during combustion reaction.

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

therefore since there 1 atom of C in product side there must be 1 atom of C in reactant side.

In addition there is 2 H atom in product side which should be the same in reactant side.

From information above the empirical formula is therefore = CH2

Molecular formula calculation

[CH2}n= 84 g/mol

[12+ (1x2)] n = 84 g/mol

14 n = 84 g/mol

n = 6

multiply the each subscript in CH2 by 6

Therefore the molecular formula = C6H12

5 0

3 years ago

Consider the reaction below.

Law Incorporation [45]

Answer:

<u>First choice: 0.042</u>

Explanation:

Given decomposition reaction:

1PCl₅ (g) ⇄ 1PCl₃ + 1Cl₂(g)

Equilibrium constant:

$K_{eq}=\frac{[PCl_3]^1[Cl_2]^1}{[PCl_5]^1}$

Stoichiometric coefficients and powers equal to 1 are not usually shown as they are understood, but I included them in order to shwow you how they intervene in the equilibrium expressions: each concentration is raised to a power equal to the respective stoichiometric coefficient in the equilibrium equation.

So, your calculations are:

$K_{eq}=\frac{(0.020M)(0.020M)}{0.0095M}=0.042M$

6 0

3 years ago