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3 years ago

For the following chemical reaction, if 40.0 grams of O2 are completely reacted, how many grams of CO2 will be produced?

Chemistry

1 answer:

e-lub [12.9K]3 years ago

7 0

Hey there!:

Molar mass:

O2 = 31.99 g/mol ; CO2 = 44.01 g/mol

Given the reaction:

C2H4 + 3 O2 --> 2 CO2 + 2 H2O

3 * 31.99 g O2 ------------ 2 * 44.01 g CO2

40.0 g O2 ------------------- mass of CO2 ??

mass of CO2 = 40.0 * 2 * 44.01 / 3 * 31.99

mass of CO2 = 3520.8 / 95.97

mass of CO2 = 36.68 g

Hope that helps!

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In a nuclear reaction, the total mass and total atomic number remains the same.

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For the given fission reaction:

$^{235}_{92}\textrm{U}+^1_0\textrm{n}\rightarrow ^A_Z\textrm{Sr}+^{143}_{54}\textrm{Xe}+3^1_0\textrm{n}$

To calculate A:

Total mass on reactant side = total mass on product side

235 + 1 = A + 143 + 3

A = 90

To calculate Z:

Total atomic number on reactant side = total atomic number on product side

92 + 0 = Z + 54 + 0

Z = 38

The isotopic symbol of strontium is $_{38}^{89}\textrm{Sr}$

Hence, the isotopic symbol of barium is $_{56}^{138}\textrm{Ba}$ and that of strontium is $_{38}^{89}\textrm{Sr}$

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