Alai is comparing the physical property of two materials. He is hitting each with a hammer to observe what happens. What physical property of the materials is Alai most likely observing?a)solublity
b)conductivity
c)hardness
d)odor

Answers

Answer 1

Answer: Since Alai is hitting each with a hammer, the physical property which he must be comparing on the two materials must be hardness. Solubility can be tested when you put them in a solvent. Odor can be tested with smell. Conductivity can be tested with electricity. Hardness can be tested with its resistance to the force that hits it.

Answer 2

Answer:

Alai is hitting each with a hammer, the physical property which he must be compared the two materials must be hardness.

What is a physical property?

A physical property is a characteristic of matter that is not associated with a change in its chemical composition. Familiar examples of physical properties include density, colour, hardness, melting and boiling points, and electrical conductivity.

Alai is hitting each with a hammer, the physical property which he must be compared to the two materials must be hardness.

Solubility can be tested when you put them in a solvent.

Odour can be tested with a smell.

Conductivity can be tested with electricity. Hardness can be tested with its resistance to the force that hits it.

Hence, Alai is comparing hardness.

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Which list of phases of H2O is arranged in order of increasing entropy

Answers

The list of phases of H2O that is arranged in order of increasing entropy is from solid then liquid then gas. Gaseous water has the most entropy because of the random movement of water molecules. And Solid having the least entropy because the water molecules are arranged in a specific order.

i get this which list of phases of H2O is arranged in order of increasing entropy

Jordan wonders why there is dew on the grass in the morning. He asks a few friends to see what they think. His friend Tasha says that there is dew on the grass because it always rains at night. Did Jordan find a scientific answer?

Answers

No because dew is water droplets that come from condensation rather than from rain coming at night

Jordan did not find a scientific answer if a warm clear day is followed by a cool clear evening Dew will likely form

When 8.00 × 1022 molecules of ammonia react with 7.00 × 1022 molecules of oxygen according to the chemical equation shown below, how many grams of nitrogen gas are produced?4 NH3(g) + 3 O2(g) → 2 N2(g) + 6 H2O(g)

Answers

Answer: 1.848 g

Explanation: To calculate the moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given molecules}}{\text {Avogadro's number}}$ ....(1)

For ammonia:

Putting values in above equation, we get:

$\text{Moles of ammonia}=(8.00* 10^(22))/(6.023* 10^(23))=0.132mol$

$\text{Moles of oxygen}=(7.00times 10^(22))/(6.023* 10^(23))=0.116mol$

For the reaction:

$4NH_3(g)+3O_2(g)\rightarrow 2N_2(g)+6H_2O(g)$

By Stoichiometry of the reaction,

4 moles of ammonia combine with 3 moles of Oxygen

Thus 0.132 moles of ammonia will combine with= $(3)/(4)* 0.132=0.009mol$ of oxygen

Thus ammonia is the limiting reagent as it limits the formation of product.

4 moles of ammonia produces 2 moles of nitrogen

0.132 moles of ammonia will produce= $(2)/(4)* 0.132=0.066 moles$ of nitrogen

Molar mass of nitrogen = 28 g/mol

Amount of nitrogen produced= ${text {no of moles}}* {text {molar mass}}=0.066* 28=1.848g$

Final answer:

In the given chemical reaction, 8.00 x 10²² molecules of ammonia would produce 37.3 grams of nitrogen gas.

Explanation:

In this chemical reaction, every 4 molecules of ammonia (NH₃) produce 2 molecules of nitrogen gas (N₂). Given you have 8.00 x 10²² molecules of ammonia, this would produce (8.00 x 10²² / 2) x 2 = 8.00 x 10²² molecules of nitrogen gas, according to the reaction stoichiometry.

One molecule of nitrogen gas (N₂) has a molar mass of 28 g/mol. To convert molecules to moles, we need Avogadro's number (6.022 x 10²³ molecules = 1 mol). So, the number of moles of nitrogen gas is (8.00 x 10²² molecules / 6.022 x 10²³ molecules/mol) = 1.33 mole.

Now, by using the molar mass of nitrogen gas, we can find the mass. So, the mass of nitrogen gas = molar mass x moles = 28 g/mol x 1.33 mol = 37.3 grams.

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The fuel used in many disposable lighters is liquid butane, C4H10. Butane has a molecular weight of 58.1 grams in one mole. How many carbon atoms are in 3.00 g of butane?

Answers

First, calculate the number of mols of C4H10 in 3.00 g of C4H10.

3.00g C4H10 / 58.1 g C4H10 = .0516 mol C4H10
There are 4 atoms of carbon per mol of C4H10
Multiply .0516 mol C4H10 by 4 (number of atoms of carbon)=.20654 mol Carbon.
To convert to atoms, multiply that by avogadro's number, 6.022 x 10^23
which equals 1.2438 x 10^23 atoms of Carbon

Answer:

1.2433 *10^23 carbon atoms

Explanation:

First you need to calculate the grams of the empirical formula.

C4H10

Carbon = 12.01 g x 4

Hydrogen = 1.008 x 10

Sum those together to get = 58.12 g

Divide the 3.00g by the total g in the compound.

3.00/58.12 = 0.0516

Then times 0.0516 by the number of carbon atoms

0.0516 x 4 = .20646

Then multiple by Avogadro's number

.20646 x 6.022x10^23 = 1.2433x10^23

Rounded to 1.24x10^23 carbon atoms

What is the molality of a solution

Answers

Answer:

The formula for molality is m = moles of solute / kilograms of solvent. In problem solving involving molality, we sometimes need to use additional formulas to get to the final answer. One formula we need to be aware of is the formula for density, which is d = m / v, where d is density, m is mass and v is volume

Explanation:

it is a measure of the concentration of a solute in a solution in terms of amount of substance in a specified amount of mass of the solvent. This contrasts with the definition of molarity which is based on a specified volume of solution.

10. A quantity of a gas has an absolute pressure of 400 kPa and an absolute temperature of 110 degrees kelvin. When the temperature of the gas is raised to 235 degrees kelvin, what is the new pressure of the gas? (Assume that there''s no change in volume.)A. 1.702 kPa
B. 3.636 kPa
C. 854.46 kPa
D. 510 kPa

Answers

Answer : (C) 854.46 KPa.

Solution : Given,

Initial pressure = 400 KPa

Initial temperature = 110 K

Final temperature = 235 K

According to the Gay-Lussac's law, the absolute pressure is directly proportional to the absolute temperature at constant volume of an ideal gas.

P ∝ T

Formula used :

$(P_(1))/(P_(2))=(T_(1))/(T_(2))$

where,

$P_(1)$ = initial pressure

$P_(2)$ = final pressure

$T_(1)$ = initial temperature

$T_(2)$ = final temperature

Now put all the values in above formula, we get

$(400)/(P_(2))=(110)/(235)$

By rearranging the terms, we get the value of new/final pressure.

$P_(2)$ = 854.5454 KPa $\approx$ 854.55 KPa

Given that N and V are constants:

$P=(NRT)/(V)\n(400)=(8.31)(110)(N)/(V)\n400=914.59(N)/(V)\n(400)/(914.59)=(N)/(V)\n\nP=(8.31)(235)(N)/(V)\nP=(1953.90)(400)/(914.59)\nP=854.55\n854.55=about~854.46$

C. 854.46 kPa

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