Which is a process that causes an organism’s poorly suited characteristics to disappear?

Remember to balance the equations first

Semenov [28]

mol CO₂ = 9.6

mol N₂ = 4.8

mol O₂ = 0.8

mol H₂O = 8

<h3>Further explanation</h3>

Reaction

4C₃H₅O₉N₃ → 12CO₂ + 6N₂ + O₂ + 10H₂O

mol CO₂

$\tt \dfrac{12}{4}\times 3.2=9.6$

mol N₂

$\tt \dfrac{6}{4}\times 3.2=4.8$

mol O₂

$\tt \dfrac{1}{4}\times 3.2=0.8$

mol H₂O

$\tt \dfrac{10}{4}\times 3.2=8$

8 0

3 years ago

Given that Kp = 3.5 x 10-4 for the reaction 2 CO(g) <=> C(graphite) + CO2(g), what is the partial pressure of CO2(g) at eq

spin [16.1K]

Answer: The partial pressure of carbon dioxide at equilibrium is 0.0056 atm

Explanation:

The given chemical equation follows:

$2CO(g)\rightleftharpoons C\text{ (graphite)}+CO_2(g)$

Initial: 4.00

At eqllm: 4.00-2x x x

The expression of $K_p$ for above reaction follows:

$K_p=\frac{p_{CO_2}}{(p_{CO})^2}$

The partial pressure of pure solids and liquids are taken as 1 in the equilibrium constant expression.

We are given:

$K_p=3.5\times 10^{-4}$

Putting values in above expression, we get:

$3.5\times 10^{-4}=\frac{x}{(4-2x)^2}\\\\x=0.0056,718.28$

Neglecting the value of x = 718.28 because equilibrium pressure cannot be greater than initial pressure

Partial pressure of $CO_2$ = 0.0056 atm

Hence, the partial pressure of carbon dioxide at equilibrium is 0.0056 atm

4 0

3 years ago

(a) Calculate the density of a 374.5-g sample of copper if it has a volume of 41.8 cm3. (b) A student needs 15.0 g of ethanol fo

o-na [289]

Answer:

For a: The density of the sample of copper is $8.96g/cm^3$

For b: The volume of ethanol needed is 19.0 mL

For c: The mass of mercury is 340. grams

Explanation:

To calculate density of a substance, we use the equation:

$\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}$ ......(1)

For a:

Mass of copper = 374.5 g

Volume of copper = $41.8cm^3$

Putting values in equation 1, we get:

$\text{Density of copper}=\frac{374.5g}{41.8cm^3}\\\\\text{Density of copper}=8.96g/cm^3$

Hence, the density of the sample of copper is $8.96g/cm^3$

For b:

Mass of ethanol = 15.0 g

Density of ethanol = 0.789 g/mL

Putting values in equation 1, we get:

$0.789g/mL=\frac{15.0g}{\text{Volume of ethanol}}\\\\\text{Volume of ethanol}=\frac{15.0g}{0.789g/mL}=19.0mL$

Hence, the volume of ethanol needed is 19.0 mL

For c:

Volume of mercury = 25.0 mL

Density of mercury = 13.6 g/mL

Putting values in equation 1, we get:

$13.6g/mL=\frac{\text{Mass of mercury}}{25.0mL}\\\\\text{Mass of mercury}=(13.6g/mL\times 25.0mL)=340.g$

Hence, the mass of mercury is 340. grams

5 0

3 years ago

How many moles of oxygen (o) are in a sample of 3.98x10^23 atoms

gregori [183]

1 mol ------- 6,02·10²³
X ------------ 3,98·10²³
X = 3,98·10²³/6,02·10²³
X= 0,6611 moles of oxygen
________________________
:)

5 0

3 years ago

Wht is a electric charge

9966 [12]

Answer:

Electric charge is the physical property of matter that causes it to experience a force when placed in an electromagnetic field. There are two types of electric charge: positive and negative (commonly carried by protons and electrons respectively).

Explanation:

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6 0

4 years ago