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2 years ago

10

Which type of reaction is represented by the generic equation AB + CD AD + CB? combustion decomposition single replacement doubl

e replacement

2 answers:

Ksju [112]2 years ago

6 0

Answer:

Double Replacement

Explanation:

MariettaO [177]2 years ago

4 0

it is a double replacement

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How many total atoms are in 0.240 g of P2O5?

RSB [31]

The answer is 1.02 × 10²⁵ atoms.

1. Calculate molar mass (Mr) of P2O5 which is the sum of atomic masses (Ar) of its elements:
Ar(P) = 31 g/mol
Ar(O) = 16
Mr(P2O5) = 2 * Ar(P) + 5 * Ar(O) = 2 * 31 + 5 * 16 = 62 + 80 = 142 g/mol

2. Calculate number of moles (n) which is the quotient of a sample mass (m) and the molar mass (Mr):
n = m/Mr
m = 0.240 g
Mr = 142 g/mol
n = 0.240 / 142 = 0.0017 mol

3. Avogadro's number is the number of units atoms in 1 mole of substance:
<span>6.023 × 10²³ atoms per 1 mol
x atoms are per 0.0017 mol

</span>6.023 × 10²³ atoms : 1 mol = x atoms : 0.0017 mol
x = 6.023 × 10²³ atoms * 0.0017 mol : 1 mol
x = 0.0102 × 10²³ = 1.02 × 10² × 10²³ = 1.02 × 10²⁵ atoms

3 0

2 years ago

Identify the correct formula for Beryllium Phosphate.

ivanzaharov [21]

<span>The correct formula for Beryllium phosphate is Be3(PO4)2 Beryllium has a charge of +2 and phosphate has a charge of -3. So to make the charge equal to zero, 3x +2 = 6, and 2 x-3 = -6 -6 + +6 = 0</span>

4 0

3 years ago

Read 2 more answers

A sample of 1.00 moles of oxygen at 50°C and 98.6 kPa, occupies what volume?

enyata [817]

Answer:

27.22 dm³

Explanation:

Given parameters:

number of moles = 1 mole

temperature= 50°C, in K gives 50+ 273 = 323K

Pressure= 98.6kpa in ATM, gives 0.973 ATM

Solution:

Since the unknown is the volume of gas, applying the ideal gas law will be appropriate in solving this problem.

The ideal gas law is mathematically expressed as,

Pv=nRT

where P is the pressure of the gas

V is the volume

n is the number of moles

R is the gas constant

T is the temperature

Input the parameters and solve for V,

0.973 x V = 1 x 0.082 x 323

V= 27.22 dm³

5 0

2 years ago

5.40 g B determine the number of atoms

sdas [7]

Atomic mass Boron ( B ) = 10.811 u.m.a

10.811 g -------------- 6.02x10²³ atoms
5.40 g ----------------- ?? atoms

5.40 x ( 6.02x10²³) / 10.811 =

3.0069x10²³ atoms

4 0

2 years ago

How many moles of ethanol are produced starting with 500.g glucose?

Monica [59]

<h3>Answer:</h3>

5.55 mol C₂H₅OH

<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> </u>

<u>Chemistry</u>

<u>Atomic Structure</u>

Reading a Periodic Tables
Moles

<u>Stoichiometry</u>

Using Dimensional Analysis
Analyzing Reactions RxN

<h3>Explanation:</h3>

<u>Step 1: Define</u>

[RxN - Balanced] C₆H₁₂O₆ → 2C₂H₅OH + 2CO₂

[Given] 500. g C₆H₁₂O₆ (Glucose)

[Solve] moles C₂H₅OH (Ethanol)

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

[RxN] 1 mol C₆H₁₂O₆ → 2 mol C₂H₅OH

[PT] Molar mass of C - 12.01 g/mol

[PT] Molar Mass of H - 1.01 g/mol

[PT] Molar Mass of O - 16.00 g/mol

Molar Mass of C₆H₁₂O₆ - 6(12.01) + 12(1.01) + 6(16.00) = 180.18 g/mol

<u>Step 3: Stoichiometry</u>

[DA] Set up conversion: $\displaystyle 500 \ g \ C_6H_{12}O_6(\frac{1 \ mol \ C_6H_{12}O_6}{180.18 \ g \ C_6H_{12}O_6})(\frac{2 \ mol \ C_2H_5OH}{1 \ mol \ C_6H_{12}O_6})$
[DA} Multiply/Divide [Cancel out units]: $\displaystyle 5.55001 \ mol \ C_2H_5OH$

<u>Step 4: Check</u>

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

5.55001 mol C₂H₅OH ≈ 5.55 mol C₂H₅OH

8 0

2 years ago