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4 years ago

What happens to an earthquake’s p-waves when they strike the liquid core?

Chemistry

1 answer:

padilas [110]4 years ago

6 0

Answer:

They bounce off.

Explanation:

They change into S-waves. They change into R-waves.

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What volume would a 0. 250 mole sample of h2 gas occupy if it had a which a a pressure of 1. 70 atm and a temperature of 35 C?

frosja888 [35]

The volume of 0. 250 mole sample of $H_{2}$ gas occupy if it had a pressure of 1. 70 atm and a temperature of 35 °C is 3.71 L.

Calculation,

According to ideal gas equation which is known as ideal gas law,

PV =n RT

P is the pressure of the hydrogen gas = 1.7 atm
Vis the volume of the hydrogen gas = ?
n is the number of the hydrogen gas = 0.25 mole
R is the universal gas constant = 0.082 atm L/mole K
T is the temperature of the sample = 35°C = 35 + 273 = 308 K

By putting all the values of the given data like pressure temperature universal gas constant and number of moles in equation (i) we get ,

1.7 atm×V = 0.25 mole ×0.082 × 208 K

V = 0.25 mole ×0.082atm L /mole K × 308 K /1.7 atm

V = 3.71 L

So, volume of the sample of the hydrogen gas occupy is 3.71 L.

learn more about ideal gas equation

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4 0

2 years ago

You have a solution of 600 mg of caffeine dissolved in 100 mL of water. The partition coefficient for aqueous caffeine extracted

klio [65]

Answer:

159 mg caffeine is being extracted in 60 mL dichloromethane

Explanation:

Given that:

mass of caffeine in 100 mL of water = 600 mg

Volume of the water = 100 mL

Partition co-efficient (K) = 4.6

mass of caffeine extracted = ??? (unknown)

The portion of the DCM = 60 mL

Partial co-efficient (K) = $\frac{C_1}{C_2}$

where; $C_1=$ solubility of compound in the organic solvent and $C_2$ = solubility in aqueous water.

So; we can represent our data as:

$K=(\frac{A_{(g)}}{60mL} )$ ÷ $(\frac{B_{(mg)}}{100mL} )$

Since one part of the portion is A and the other part is B

A+B = 60 mL

A+B = 0.60

A= 0.60 - B

4.6= $(\frac{0.6-B(mg)}{60mL} )$ ÷ $(\frac{B_{(mg)}}{100mL})$

4.6 = $\frac{(\frac{0.6-B(mg)}{60mL} )}{(\frac{B_{(mg)}}{100mL})}$

4.6 × $(\frac{B_{(mg)}}{100mL})$ = $(\frac{0.6-B(mg)}{60mL} )$

4.6 B $*\frac{60}{100}$ = 0.6 - B

2.76 B = 0.6 - B

2.76 + B = 0.6

3.76 B = 0.6

B = $\frac{0.6}{3.76}$

B = 0.159 g

B = 159 mg

∴ 159 mg caffeine is being extracted from the 100 mL of water containing 600 mg of caffeine with one portion of in 60 mL dichloromethane.

4 0

3 years ago

Read 2 more answers

.One ballon is filled with Hydrogen (H2) gas, the other balloon is filled with methane (CH4). Both balloons have the same temper

Neko [114]

Answer:

C. The balloon with CH4 has the same moles of gas molecules as the balloon with H2

Explanation:

Based on combined gas law, gases under the same pressure, temperature and volume have the same number of moles. With this information we can say the rigth statement is:

<h3>C. The balloon with CH4 has the same moles of gas molecules as the balloon with H2</h3>

7 0

3 years ago

Helga [31]

Answer: THE ANSWER IS OZONE WEEEE a layer in the earth's stratosphere at an altitude of about 6.2 miles (10 km) containing a high concentration of ozone, which absorbs most of the ultraviolet radiation reaching the earth from the sun.

Explanation:

6 0

3 years ago

In experiment 1, how many moles of benzoic acid are present? how many moles of sodium bicarbonate are contained in 1 ml of a 10%

nexus9112 [7]

First, let us calculate the moles of solute or sodium bicarbonate is in the 1 ml solution.

<span>moles = 1 mL * (1 g / 9 mL) = 0.11 moles</span>

The molar mass of sodium bicarbonate is 84 g/mol, therefore the mass is:

mass = 0.11 moles * 84 g/mol

6 0

3 years ago