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2 years ago

What is the average isotope mass?

Chemistry

2 answers:

Aleksandr [31]2 years ago

8 0

Answer:

the atomic mass of an element is the average mass of the atoms of an element measured in atomic mass unit (amu, also known as daltons, D). The atomic mass is a weighted average of all of the isotopes of that element, in which the mass of each isotope is multiplied by the abundance of that particular isotope

Explanation:

Average atomic mass = f1M1 + f2M2 + … + fnMn where f is the fraction representing the natural abundance of the isotope and M is the mass number (weight) of the isotope. The average atomic mass of an element can be found on the periodic table, typically under the elemental symbol.

Aliun [14]2 years ago

5 0

Answer:

he atomic mass of an element is the average mass of the atoms of an element measured in atomic mass unit (amu, also known as daltons, D). The atomic mass is a weighted average of all of the isotopes of that element, in which the mass of each isotope is multiplied by the abundance of that particular isotope.

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When 2.5 mol of O2 are consumed in their reaction, ________ mol of CO2 are produced

Vika [28.1K]

The given question is incomplete. The complete question is:

The combustion of propane (C3H8) in the presence of excess oxygen yields $CO_2$ and $H_2O$

$C_3H_8(g)+5O_2 (g)\rightarrow 3CO_2(g)+4H_2O (g)$

When only 2.5 mol of $O_2$ are consumed in order to complete the reaction, ________ mol of $CO_2$ are produced.

Answer: Thus when 2.5 mol of $O_2$ are consumed in their reaction, 1.5 mol of $CO_2$ are produced

Explanation:

The balanced chemical equation is:

$C_3H_8(g)+5O_2 (g)\rightarrow 3CO_2(g)+4H_2O (g)$

According to stoichiometry :

5 moles of $O_2$ produce = 3 moles of $CO_2$

Thus 2.5 moles of $O_2$ will produce = $\frac{3}{5}\times 2.5=1.5$ moles of $CO_2$

Thus when 2.5 mol of $O_2$ are consumed in their reaction, 1.5 mol of $CO_2$ are produced

4 0

2 years ago

प्रश्न 5. 'पुष्प की अभिलाषा' कविता में पुष्प के दवारा क्या अभिलाषा व्यक्त की गई

Kay [80]

Please ask in English

4 0

2 years ago

What is the ionic charge for the calcium ion in CaCO3?

Lunna [17]

<span>The ionic charge of Calcium (Ca) in calcium carbonate (CaCO3) is 2+. CaCO3 has a neutral ionic charge sin CO3 has a 2- charge.</span>

3 0

3 years ago

Find the "density" of a copper sample whose mass is 134.4 grams and whose volume is 15.0mL

Sonja [21]

Answer:

8.96 g/mL

Explanation:

density = mass / volume

density = 134.3g / 15.0 mL

density = 8.96 g/mL

3 0

2 years ago

The reaction of ethane gas (C2H6) with chlorine gas produces C2H5Cl as its main product (along with HCl). In addition, the react

Kazeer [188]

Answer:

The percent yield of chloro-ethane in the reaction is 82.98%.

Explanation:

$C_2H_6+Cl_2\rightarrow C_2H_5Cl+HCl$

Moles of ethane = $\frac{300.0 g}{30 g/mol}=10 mol$

Moles of chlorine gases = $\frac{650.0 g}{71 .0 g/mol}=9.1549 mol$

As we can see that 1 mol of ethane react with 1 mole of chlorine gas.the 10 moles will require 10 mole of chlorine gas, but only 9.1549 moles of chlorine gas is present.

This means that chlorine gas is in limiting amount and amount of formation of chloro-ethane will depend upon amount of chlorine gas.

According to reaction , 1 mol of chloro ethane gives 1 mol of chloro-ethane.

Then 9.1549 moles of chlorien gas will give:

$\frac{1}{1}\times 9.1549 mol=9.1549 mol$ of chloro-ethane

Mass of 9.1549 moles of chloro-ethane:

9.1549 mol × 64.5 g/mol = 590.4910 g

Theoretical yield of chloro-ethane: 590.4910 g

Given experimental yield of chloro-ethane: 490.0 g

$\% Yield=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

$\%Yield (C_2H_5Cl)=\frac{490.0 g}{590.4910 g}\times 100=82.98\%$

The percent yield of chloro-ethane in the reaction is 82.98%.

6 0

2 years ago