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3 years ago

1). The Kinetic Molecular Theory 5 points

Chemistry

1 answer:

Rus_ich [418]3 years ago

7 0

Answer:

D- Kinetic Molecular Theory

Explanation:

. Gases consist of large numbers of tiny particles that are far apart relative to their size.

.Collision between gas particles and between particles and container walls are elastic collisions.

.Gas particles are in continuous motion. possess kinetic energy.

. Gas molecules have negligible intermolecular forces.

. Gas molecules have an average kinetic energy proportional to the ideal gas's absolute temperature.

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Suppose you have three monodisperse polymer samples, A, B, and C, with molar masses of 100,000 g/mol, 200,000 g/mol, and 300,000

EastWind [94]

Answer:

a) Number-average molar mass: 163,700g/mol

Weight-average molar mass: 200,000g/mol

b) Number-average molar mass: 200,000g/mol

Weight-average molar mass: 233,300g/mol

Explanation:

The number-average molar mass is based on mole% and weight-average molar mass is based on weight%, thus:

a) In equal proportions by weight:

number-average molar mass:

1g A× $\frac{1mol}{100,000g}$ = 1x10⁻⁵ moles A

1g B× $\frac{1mol}{200,000g}$ = 5x10⁻⁶ moles B

1g C× $\frac{1mol}{300,000g}$ = 3,33x10⁻⁶ moles C

Total moles are:

1x10⁻⁵ A + 5x10⁻⁶ B + 3,33x10⁻⁶ C = 1,833x10⁻⁵ moles.

Percent A: $\frac{1x10^{-5}}{1,833x10^{-5}}$ ×100 = 54,5%

Percent B: $\frac{5x10^{-6}}{1,833x10^{-5}}$ ×100 = 27,3%

Percent C: $\frac{3,33x10^{-6}}{1,833x10^{-5}}$ ×100 = 18,2%

number-average molar mass:

0,545*100,000g/mol + 0,273*200,000g/mol + 0,182*300,000g/mol = 163,700g/mol

weight-average molar mass:

0,333*100,000g/mol + 0,333*200,000g/mol + 0,333*300,000g/mol = 200,000g/mol

b) In molar ratio 1:1:1

weight-average molar mass:

1mol A× $\frac{100,000g}{1mol}$ = 100,000g A

1mol B× $\frac{200,000g}{1mol}$ = 200,000g B

1mol C× $\frac{300,000g}{1mol}$ = 300,000g C

Total mass is:

100,000 A + 200,000 B + 300,000 C = 600,000 g.

Percent A: $\frac{100,000}{600,000}$ ×100 = 16,7%

Percent B: $\frac{200,000}{600,000}$ ×100 = 33,3%

Percent C: $\frac{300,000}{600,000}$ ×100 = 50,0%

Weight-average molar mass:

0,167*100,000g/mol + 0,333*200,000g/mol + 0,500*300,000g/mol = 233,300g/mol

number-average molar mass:

0,333*100,000g/mol + 0,333*200,000g/mol + 0,333*300,000g/mol = 200,000g/mol

I hope it helps!

4 0

4 years ago

What is the density of a block of marble that occupies 310 cm3 and has a mass of 853 g?1. Diamond has a density of 3.26 g/cm3 .2

Vedmedyk [2.9K]

Answer:53gm

Explanation:

5 0

3 years ago

If the temperature of a fixed amount of a gas is doubled at constant volume, what happens to the pressure?

EastWind [94]

Temperature and pressure are directly proportional. Pressure will also have to increase ( doubling).

4 0

4 years ago

If you have 10cm of snow with a volume of 40mL and a density of 0.5 g/mL how many inches of rain is this?

Lelu [443]

Density is the mass of compound divided by its volume can be shown as follows:

$d = 0.5 g /mL = m /V = m /40 = 0.5$

$m = 20 g$

40 mL of snow having 20 g of mass calculated from density.

Now, 10 cm of snow = 3.93 inches = 20 g

As, 10 inches of rain will produce 11 inches of ice as the volume of ice is bigger than rain water.

10 inches rain = 11 inches snow

3.93 inches of snow produced by

$= (3.93 * 10) /11 = 3.57 inches rain.$

Thus, 3.57 incehs of rain produces by 10 cm snow.

4 0

3 years ago

Rewrite the equation below using the correct conventions for stoichiometric coefficients. 2 BaCl2 + 2 H2SO4 → 2 BaSO4 + 4 HCl

vichka [17]

Answer:

$BaCl2+H2SO4 \rightarrow BaSO4+2HCl$

Explanation:

The given equation is:

$2 BaCl2+2H2SO4 \rightarrow2BaSO4+4HCl$

Based on the reaction stoichiometry:

2 moles of barium chloride (BaCl2) reacts with 2 moles of sulfuric acid (H2SO4) to form 2 moles of barium sulfate (BaSO4) and 4 moles of HCl

Although the reaction is balanced, the correct convention is to depict reactions in terms of the lowest molar ratio. Therefore the coefficients (2,2,4 and 4) can be divided by 2 to give:

$BaCl2+H2SO4 \rightarrow BaSO4+2HCl$

6 0

3 years ago