23. The cell has a

Using venn diagram, compare and contrast cotton balls and pine cones

Irina-Kira [14]

Cotton Balls are soft and pine cones are hard.

8 0

3 years ago

Isoflurane, shown here, is a common inhalation anesthetic. write its molecular formula and calculate its percent composition by

Natalka [10]

Molecular formula of Isoflurane is C₃H₂ClF₅O.

Now calculate the percent composition by mass, which means percent of each element in the compound.

Mass of Isoflurane = 184.49 g/mol

Mass of carbon in the compound = 3 x 12.011 = 36.033g

Mass of hydrogen in the compound = 2 x 1.008 = 2.016g

Mass of chlorine in the compound = 1 x 35.453 = 35.453 g

Mass of fluorine in the compound = 5 x 18.998 = 94.99g

Mass of Oxygen in the compound = 1 x 16 = 16 g

Carbon’s percentage = Mass of carbon in the compound /mass of isoflurane x 100 =36.033/184.49 x 100 =19.53%

Hydrogen’s Percentage = Mass of hydrogen in the compound/mass of isoflurane x 100 = 2.016/184.49 = 1.09%

Chlorine’s percentage = Mass of chlorine in the compound/mass of isoflurane x 100 = 35.453/184.49 =19.22%

Flourine’s percentage = Mass of fluorine in the compound/mass of isoflurane x 100 = 94.99/184.49 x 100 = 51.49%

Oxygen’s percentage = Mass of Oxygen in the compound/mass of isoflurane x 100 =16/184.49 x 100 = 8.67%

7 0

3 years ago

Cuando los volcanes entran en erupción lanzan al exterior porciones de materia muy variada ¿cuales fueron los productos de la er

DENIUS [597]

Answer:

The Etna volcano when it previously erupted released a lot of smoke, and then volcanic lava.

Explanation:

The eruption of this volcano was on the Italian island of Sicily.

Where there were large columns of smoke and after that the volcanic magma in a viscoelastic state was released into the external environment.

Some sources claim that the eruption of this volcano reached the areas of Zaffanera.

7 0

3 years ago

How many moles of oxygen is required to produce 7.8 moles of water?

Olin [163]

Answer:

3.5

Explanation:

8 0

3 years ago

The gas left in a used aerosol can is at a pressure of 103 kPa at 25.0 °C. If the can heats up to 50.0 °C, what is the pressure

Anton [14]

The question mentions a change in temperature from 25 to 50 °C. With that, the aim of the question is to determine the change in volume based on that change in temperature. Therefore this question is based on Gay- Lussac's Gas Law which notes that an increase in temperature, causes an increase in pressure since the two are directly proportional (once volume remains constant). Thus Gay-Lussac's Equation can be used to solve for the answer.
Boyle's Equation: $\frac{P_{1} }{T_{1} }$ = $\frac{P_{2} }{T_{2} }$
Since the initial temperature (T₁) is 25 C, the final temperature is 50 C (T₂) and the initial pressure (P₁) is 103 kPa, then we can substitute these into the equation to find the final pressure (P₂).
$\frac{P_{1} }{T_{1} }$ = $\frac{P_{2} }{T_{2} }$ ∴ by substituting the known values, ⇒ (103 kPa) ÷ (25 °C) = (P₂) ÷ (50 °C)
⇒ P₂ = (4.12 kPa · °C) (50 °C)
= 206 kPa
Thus the pressure of the gas since the temperature was raised from 25 °C to 50 °C is 206 kPa

3 0

3 years ago