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3 years ago

A balloon full of air has a volume of 1.00L at a temperature of 23 °C. What is the balloon's volume at 33°C?

Chemistry

1 answer:

igomit [66]3 years ago

5 0

Answer:

V2= 1.03L

Explanation:

Start off with what you are given.

V^1: 1.00L

T^1: 23°C

V^2?

T^2: 33°C

If you know your gas laws, you have to utilise a certain gas law called Charles' Law:

V^1/T^1 = V^2/T^2

Remember to convert Celsius values to Kelvin whenever you are dealing with gas problems. This can be done by adding 273 to whatever value in Celsius you have.

(23+273 = 296) (33+273 = 306)

Multiply crisscross

1.00/296= V^2/306

296V^2 = 306

Dividing both sides by 296 to isolate V2, we get

306/296 = 1.0337837837837837837837837837838

V2= 1.03L

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A sample of CH4 is confined in a water manometer. The temperature of the system is 30.0 °C and the atmospheric pressure is 98.70

kakasveta [241]

Explanation:

The given data is as follows.

$P_{atm}$ = 98.70 kPa = 98700 Pa,

T = $30^{o}C$ = (30 + 273) K = 303 K

height (h) = 30 mm = 0.03 m (as 1 m = 100 mm)

Density = 13.534 g/mL = $13.534 g/mL \times \frac{10^{6}cm^{3}}{1 m^{3}} \times \frac{1 kg}{1000 g}$

= 13534 $kg/m^{3}$

The relation between pressure and atmospheric pressure is as follows.

P = $P_{atm} + \rho gh$

Putting the given values into the above formula as follows.

P = $P_{atm} + \rho gh$

= $98700 Pa + 13534 \times 9.81 \times 0.03 m$

= 102683.05 Pa

= 102.68 kPa

thus, we can conclude that the pressure of the given methane gas is 102.68 kPa.

8 0

3 years ago

Kc for the reaction N2O4 <=> 2NO2 is 0.619 at 45 degrees C If 50.0g of N2O4 is introduced into an empty 2.10L container, w

Nadya [2.5K]

Answer:

p(N2O4) = 0.318 atm

p(NO2) = 7.17 atm

Explanation:

Step 1: Data given

Kc = 0.619

Temperature = 45.0 °C

Mass of N2O4 = 50.0 grams

Volume = 2.10 L

Molar mass N2O4 = 92.01 g/mol

Step 2: The balanced equation

N2O4 ⇔ 2NO2

Step 3: Calculate moles N2O4

Moles N2O4 = 50.0 grams / 92.01 g/mol

Moles N2O4 = 0.543 moles

Step 4: The initial concentration

[N2O4] = 0.543 moles/2.10 L = 0.259 M

[NO2]= 0 M

Step 5: Calculate concentration at the equilibrium

For 1 mol N2O4 we'll have 2 moles NO2

[N2O4] = (0.259 -x)M

[NO2]= 2x

Step 6: Calculate Kc

Kc = 0.619= [NO2]² / [N2O4]

0.619 = (2x)² / (0.259-x)

0.619 = 4x² / (0.259 -x)

x = 0.1373

Step 7: Calculate concentrations

[N2O4] = (0.259 -x)M = 0.1217 M

[NO2]= 2x = 0.2746 M

Step 8: The moles

Moles = molarity * volume

Moles N2O4 = 0.1217 M * 2.10 = 0.0256 moles

Moles NO2 = 0.2746 M * 2.10 = 0.577 moles

Step 9: Calculate partial pressure

p*V = n*R*T

⇒ with p = the partial pressure

⇒ with V = the volume = 2.10 L

⇒ with n = the number of moles

⇒ with R = the gas constant = 0.08206 L*atm/mol*K

⇒ with T = the temperature = 45 °C = 318 K

p = (nRT)/V

p(N2O4) = (0.0256 *0.08206 * 318)/ 2.10

p(N2O4) = 0.318 atm

p(NO2) = (0.577 *0.08206 * 318)/ 2.10

p(NO2) = 7.17 atm

6 0

3 years ago

Balanced or Unbalanced<br><br> CH4+4Ci2=CCi4+4HCi

Volgvan

Answer:

balanced

Explanation:

its balance since all the elments add up on both sides

7 0

3 years ago

a student poured water in to a paper cup and let it freeze,when she came to take it out she saw the side pushed out

Zina [86]

Great Question!

Everything around us is made up of matter. (Matter is just a fancy word for stuff.) If you cut matter up as small as you possibly can - much smaller than you can see with your eyes, or even a microscope - then you get what scientists like to call atoms. There's lots of different kinds of atoms, like oxygen, nitrogen, and hydrogen atoms. You may have learned about some of these in school. When you put several atoms together, they "bond" (or stick) together and you get what's called molecules.

A water molecule is what you get when you put together two hydrogen atoms and one oxygen atom. The shape of the water molecule has the oxygen atom in the middle and the two hydrogen atoms stuck to it on the sides, and it sort of makes a triangle. It looks a little bit like this, where the O is the Oxygen atom, the H's are the Hydrogen atoms, and the lines are the bonds between them:

/ \

H H

Other molecules (for example, different types of chemicals) have different shapes.

When a liquid (like water) is frozen, all of the molecules start sticking to each other and holding on very tightly. Because different types of molecules have different shapes, they hold on to each other in different places. Most of the time, when they start holding on to each other, they get closer together. When the molecules get closer together, they take up less space, so the frozen solid ends up being smaller than the unfrozen liquid.

Water, however, is a bit weird. When the water molecules start holding on to each other really tightly, they make a pattern that actually takes up /more/ space than they did when they weren't stuck together. (This pattern is what you see if you look at ice crystals.) So, when water freezes, the molecules take up more space, and the ice ends up being even /bigger/ than the water was.

If you were to put that water in a closed container in the freezer, then it would still get bigger. What happens to the container depends on what sort of a container it is. For example, if the container were made of thin plastic, it would probably stretch a bit as the water freezes. But if you were to put it in a very full, tightly sealed glass container, then the frozen water would be pushing so hard that the glass might break. This is why if you put a glass bottle of juice in the freezer, you're supposed to take the lid off until it's frozen all the way.

3 0

3 years ago

A compound has the empirical formula . a 256-ml flask, at 373 k and 750. torr, contains 0.527 g of the gaseous compound. give th

CaHeK987 [17]

<span>Answer: From the ideal gas law, MM=mRTPV; where MM = molecular mass; m = mass; P = pressure in atmospheres; V= volume in litres; R = gas constant with appropriate units. So, 0.800â‹…gĂ—0.0821â‹…Lâ‹…atmâ‹…Kâ’1â‹…molâ’1Ă—373â‹…K0.256â‹…LĂ—0.987â‹…atm = 97.0 gâ‹…molâ’1. nĂ—(12.01+1.01+2Ă—35.45)â‹…gâ‹…molâ’1 = 97.0â‹…gâ‹…molâ’1. Clearly, n = 1. And molecular formula = C2H2Cl2. I seem to recall (but can't be bothered to look up) that vinylidene chloride, H2C=C(Cl)2 is a low boiling point gas, whereas the 1,2 dichloro species is a volatile liquid. At any rate we have supplied the molecular formula as required.</span>

4 0

3 years ago