The ability to put in a light bulb with greater ease is because the bottom half is what type of simple machine?

If an atom has the same amount of protons and electron, its net charge will be

DiKsa [7]

I’m pretty sure the answer would be natural

3 0

2 years ago

Read 2 more answers

Why are digestive enzymes in a cell enclosed in a membrane

erastova [34]

The membrane keeps the digestive materials from leaking out into the cytoplasm and destroying the cell.

7 0

2 years ago

a metal object has a mass of 9.0g and a volume of 1.5ml. what is the density of the object? density= mass/volume

weeeeeb [17]

The density of the metal object=6.0 $\frac{g}{m l}$

Given:

Volume of the metal object=1.5ml

Mass of the metal object=9.0g

To find:

Density of the metal object

Step by Step Explanation:

Solution:

According to the formula, Density of the metal object can be calculated as

$\rho=\frac{m}{v}$

Where, m=mass of the metal object

$\rho$ =density of the metal object

v=volume of the metal object

We know the values of v=1.5ml and m=9.0g

Substitute these values in the above equation we get

$\rho=\frac{m}{v}$

$\rho$ =9.0/1.5

=6.0 $\frac{g}{m l}$

Result:

Thus the density of the metal object is 6.0 $\frac{g}{m l}$

4 0

2 years ago

Please, What is the mass of oxygen in 72.0g of water? [ H= 1.0; O = 16.0]

yarga [219]

Convert 72g of water into moles of water using molecular weights.

So water is H2O so add up those molecular weights (H=1 and O=16)

2(1)+(16) = 18 g/mol

Then convert so 72g / (18 g/mol) = 4 mol

Now you can convert mol of water to mol of oxygen. So 4 mol of water is 4 mol of oxygen. Then use oxygen molecular weight to find grams again.

4 mol oxygen * 16 g/mol = 64g of oxygen

If we were doing hydrogen instead of oxygen there would be 8 mol hydrogen in 4 mol of water (2 H’s in every H2O molecule) and since we have 74 grams and oxygen is 64 grams, Hydrogen should be 8 grams. Math to check below

8 mol hydrogen * 1 g/mol = 8g of hydrogen

It all adds to 72 so we are correct.

5 0

2 years ago

A mixture of hydrocarbons contains 38.3% hexane, C6H14, 13.9% octane, C8H18, and 47.8% decane, C10H22. The mixture is combusted

GaryK [48]

Answer:

52.206 kg

Explanation:

From the given information:

Mass of hexane C6H14 = $19.3*10^3 \ g \times \dfrac{38.3}{100}$

= 7391.9 g

Mass of octane C8H18 = $19.3*10^3 \ g \times \dfrac{13.9}{100}$

= 2682.7 g

Mass of decane C10H22 = $19.3*10^3 \ g \times \dfrac{47.8}{100}$

= 9225.4 g

However, recall that:

number of moles of an atom = mass/molar mass

∴

For hexane, no of moles = 7391.9 g/86.18 g/mol

= 85.77 moles

For octane, no of moles = 2682.7 g/114.23 g/mol

= 23.49 moles

For decane, no of moles = 9225.4 g/142.29 g/mol

= 64.84 moles

Therefore:

number of moles of CO2 produced = (6 × 85.77)+(23.49)+(10×64.84) moles

= 1186.51 moles

Finally, the mass of CO2 produced is:

= 1186.51 mol × 44 g/mol

= 52206.44 g

= 52.206 kg

4 0

2 years ago