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2 years ago

A 1.000-g sample of lead shot reacted with oxygen to give 1.077 g of product. Calculate the empirical formula of the lead oxide

Chemistry

2 answers:

Alex_Xolod [135]2 years ago

7 0

The empirical formula of lead oxide is PbO

<u><em>Calculation</em></u>

Step 1: find the mass of oxygen that reacted

=mass of the product- mass of lead

= 1.077 g - 1.000 =0.077 g

Step 2: find the mole of each reactant

moles = mass/molar mass

the molar mass of Pb =207 g/mol while that of O = 16g/mol from periodic table

moles of lead(Pb) is therefore = 1.000 g / 207 g/mol =0.0048 moles

moles of O2 =0.077g/16 g/mol =0.0048 moles

Step 3: find the mole ratio

that is divide each mole by smallest number of mole (0.0048)

Pb = 0.0048/0.0048 =1

O=0.0048/0.0048 =1

from mole ratio above in 1 atom of Pb of the product we have 1 atom of O therefore the empirical formula is PbO

Evgesh-ka [11]2 years ago

3 0

It mean it consisted of 1 g of lead and 0.077 g of O2.
divide these numbers by molar mas.
1/82=0.012 Pb /0.004 = 3
0.077/16= 0.004 O /0.004 =1
Pb3O

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Solution: Which of the following chemical reactions is/are NOT possible according to Dalton's atomic theory?a. reaction 1: CCl4 → CH4b. reaction 2: N2 + 3H2 → 2NH3c. reaction 3: 2H2 + O2 → 2H2O + Au

Problem

Which of the following chemical reactions is/are NOT possible according to Dalton's atomic theory?

a. reaction 1: CCl4 → CH4

b. reaction 2: N2 + 3H2 → 2NH3

c. reaction 3: 2H2 + O2 → 2H2O + Au

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2 years ago

Determine total H for bonds broken and formed, the overall change in H, and the final answer with units. Is it ENDOthermic or EX

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E(Bonds broken) = 1371 kJ/mol reaction
E(Bonds formed) = 1852 kJ/mol reaction

ΔH = -481 kJ/mol.
The reaction is exothermic.

<h3>Explanation</h3>

2 H-H + O=O → 2 H-O-H

There are two moles of H-H bonds and one mole of O=O bonds in one mole of reactants. All of them will break in the reaction. That will absorb

E(Bonds broken) = 2 × 436 + 499 = 1371 kJ/mol reaction.
ΔH(Breaking bonds) = +1371 kJ/mol

Each mole of the reaction will form two moles of water molecules. Each mole of H₂O molecules have two moles O-H bonds. Two moles of the molecule will have four moles of O-H bonds. Forming all those bond will release

E(Bonds formed) = 2 × 2 × 463 = 1852 kJ/mol reaction.
ΔH(Forming bonds) = - 1852 kJ/mol

Heat of the reaction:

$\Delta H_{\text{rxn}} = \Delta H(\text{Breaking bonds}) + \Delta H(\text{Forming bonds})\\\phantom{ \Delta H_{\text{rxn}}} = +1371 + (-1852) \\\phantom{ \Delta H_{\text{rxn}}} = -481 \; \text{kJ} / \text{mol}$

$\Delta H_{\text{rxn}}$ is negative. As a result, the reaction is exothermic.

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