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3 years ago

List all the physical properties of the iceberg.

Chemistry

1 answer:

Semmy [17]3 years ago

3 0

Answer: My answer is in the explanation

Explanation:

Physical and mechanical characteristics of iceberg ice were studied from samples collected near the shores of eastern Newfoundland. Although the physical characteristics show considerable diversity, iceberg ice has some common features and is generally porous, lacks significant concentrations of dissolved materials, contains internal cracks and has an irregular interlocking grain structure.

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If you chip a tooth, most likely you will go to the dentist to have the missing material filled in. Currently the material used

AnnZ [28]

ti\his answer is radiation

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3 years ago

What is the density of 1.00 mol of carbon monoxide gas at STP?

Ksju [112]

Answer:

Density = mass / volume.

If this is an ideal gas then 1mol will take up 22.4L of volume (fact about ideal gases you should remember)

Since you have 1mol then you know the volume of the gas that you have (22.4L)

Now, just convert 1mol of CO to grams.The ptable tells you that the mass of 1 mol of C is 12g and the mass of 1 mol of O is 16g. So the mass of 1 mol of CO is......... :):)

Now you have the mass and the volume, so just divide :) enjoy

6 0

2 years ago

15.89 percent carbon, 21.18 percent oxygen, and 62.93 percent osmium. what is the empirical formula

otez555 [7]

Answer:

OsCO or COOs

Explanation:

Data given

Carbon = 15.89 %

Oxygen = 21.18 %

Osmium = 62.93%

Empirical formula = ?

Solution:

First find the masses of each component

Consider total compound is 100g

As we now

mass of element = % of component

So,

15.89 g of C = 15.89 % Carbon

21.18 g of O = 21.18 % Oxygen

62.93 g of Os = 62.93% Osmium

Now convert the masses to moles

For Carbon

Molar mass of C = 12 g/mol

no. of mole = mass in g / molar mass

Put value in above formula

no. of mole = 15.89 g/ 12 g/mol

no. of mole = 1.3242

mole of C = 1.3242

For Oxygen

Molar mass of O = 16 g/mol

no. of mole = mass in g / molar mass

Put value in above formula

no. of mole = 21.18 g/ 16 g/mol

no. of mole =

mole of O = 1.3238

For Os

Molar mass of Os = 190 g/mol

no. of mole = mass in g / molar mass

Put value in above formula

no. of mole = 62.93 g/ 190 g/mol

no. of mole =

mole of Os = 1.3312

Now we have values in moles as below

C = 1.3242

O = 1.3238

Os = 1.3312

Divide the all values on the smalest values to get whole number ratio

C = 1.3242 /1.3238 = 1.0003

O = 1.3238 /1.3238 = 1

Os = 1.3312 /1.3238 = 1.0056

So all have round value 1 mole

C = 1

O = 1

Os = 1

So the empirical formula will be (OsCO) i.e. all 3 atoms in simplest small ratio

7 0

3 years ago

By what quantity must the heat capacity be divided to obtain the specific heat of that material

masha68 [24]

Heat capacity of an object, is the amount of heat energy or thermal energy (unit: Joule) needed to raise the temperature of the object by 1 degree celsius. Unit of heat capacity is J/°C

Larger object will surely need larger amount of thermal energy to raise its temperature. If you compare 1 litre of water with 0.5 litre of water, the 1L water will have two times the heat capacity.

It will be more useful to compare specific heat capacity, because then it is the amount of heat energy or thermal energy (unit: Joule) needed to raise the temperature of 1 unit mass of the object by 1 degree celsius. You can then compare between 1 unit mass of water and 1 unit mass of iron.
Water has higher specific heat capacity than iron, meaning that you need more energy to heat up 1kg of water, then to heat up 1kg of iron.

The unit will then be J/(kg °C) or J/(g °C).

6 0

3 years ago

I need help with part B . please

myrzilka [38]

So it's good to map out what you know you have and work from there:
We have two liter measurements and one mole measurement, and we need to find the moles.

For this problem, think of it this way: 46 liters of gas = 1.4 moles.
If one side changes, the other has to as well (if the liters decrease, the moles decrease. if the liters increase, so do the moles.) What you can do is put this into a fraction:

 1.4 moles
 46 L 

if we know that each liter of gas is equal to x amount of moles, we know that 11.5 liters equals some amount of moles. You can put this into a fraction too, and make it equal to the other fraction:

1.4 moles = x moles
46 L 11.5 L

Then get your calculator out and do some algebra.

11.5 * (1.4/46) = x

The answer should come out to be: 0.35 moles

8 0

3 years ago