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3 years ago

What do we call the process by which cells obtain the energy that they need?

Chemistry

1 answer:

REY [17]3 years ago

3 0

Cellular Respiration is the process in which cells break down food molecules to release the stores chemical energy.

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Identify the type of reaction shown by this chemical equation: 2AI + 6HCI - 2AlCl3 + 3H2

ArbitrLikvidat [17]

Answer:

Single displacement reaction

Explanation:

2AI + 6HCI —> 2AlCl3 + 3H2

From the above reaction, we see clearly that Al displaces H from HCl. This is clearly a single displacement reaction.

5 0

2 years ago

What does it mean to standardize the naoh solution why can the molarity of the naoh solution not be determined accurately?

ruslelena [56]

A standard solution is a solution (in this case sodium hydroxide) whose concentration (molarity) is known very precisely. The molarity of the sodium hydroxide solution cannot be determined accurately because solid sodium hydroxide is highly hygroscopic (absorbs water from the air) and cannot be accurately weighed. Sodium hydroxide form sodium carbonate because it absorbs carbon dioxide from the air.

5 0

3 years ago

Read 2 more answers

What can be done in a laboratory to correctly identify flame tests that are the same color

IgorC [24]

You can separate your lab materials for each flame test and color code them using non-flammable labels.

It helps a ton when I do lab tests ....

4 0

2 years ago

Which wavelength bands are just outside the visible range?

Norma-Jean [14]

Answer: The ultraviolet or UV portion

Explanation:

The term comes from the fact that this type of radiation is slightly beyond the violet region of visible wavelengths

7 0

1 year ago

Assuming gasoline is isooctane, with a density of g/mL, what is the theoretical yield of carbon dioxide produced by the combusti

Vesna [10]

This is an incomplete question, here is a complete question.

Assuming gasoline is 89.0% isooctane, with a density of 0.692 g/mL, what is the theoretical yield (in grams) of CO₂ produced by the combustion of 1.80 × 10¹⁰ gallons of gasoline (the estimated annual consumption of gasoline in the U.S.)?

Answer : The theoretical yield of carbon dioxide is $1.453\times 10^{14}g$

Explanation : Given,

Volume of isooctane = $1.80\times 10^{10}gallons$

First we have to convert volume into liters, we use the conversion factor:

1 gallon = 3.785 L

So, $1.80\times 10^{10}gallon\times (\frac{3.785L}{1gallon})=6.813\times 10^{10}L$

Now we have to calculate the mass of isooctane.

$\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}$

Volume of isooctane = $6.813\times 10^{10}L=6.813\times 10^{13}mL$ (Conversion factor: 1 L = 1000 mL)

Density of isooctane = 0.692 g/mL

Now put all the given values in above equation, we get:

$0.692g/mL=\frac{\text{Mass of isooctane}}{6.813\times 10^{13}mL}\\\\\text{Mass of isooctane}=(0.692g/mL\times 6.813\times 10^{13}mL)=4.714\times 10^{13}g$

Now we have to calculate the number of moles.

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

Given mass of isooctane = $4.714\times 10^{13}g$

Molar mass of isooctane = 114.22 g/mol

Now put all the given values in equation 1, we get:

$\text{Moles of isooctane}=\frac{4.714\times 10^{13}g}{114.22g/mol}=4.127\times 10^{11}mol$

The chemical equation for the combustion of isooctane is:

$2C_8H_{18}+25O_2\rightarrow 16CO_2+18H_2O$

By Stoichiometry of the reaction we can say that,

As, 2 moles of isooctane produces 16 moles of carbon dioxide.

So, $4.127\times 10^{11}mol$ of isooctane will produce = $\frac{16}{2}\times 4.127\times 10^{11}mol=3.3016\times 10^{12}mol$ of carbon dioxide

Now we have to calculate the mass of carbon dioxide.

Molar mass of carbon dioxide = 44.00 g/mol

Moles of carbon dioxide = $3.3016\times 10^{12}mol$

Now put all the given values in equation 1, we get:

$3.3016\times 10^{12}mol=\frac{\text{Mass of carbon dioxide}}{44.00g/mol}\\\\\text{Mass of carbon dioxide}=(3.3016\times 10^{12}mol\times 44.00g/mol)=1.453\times 10^{14}g$

Hence, the theoretical yield of carbon dioxide is $1.453\times 10^{14}g$

6 0

3 years ago