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3 years ago

8

6.0 L of gas in a piston at a pressure of 1.0 atm are compressed until the volume is 3.5 L. What is the new pressure inside the

piston?

1 answer:

Ne4ueva [31]3 years ago

7 0

Answer:

<u>1.7 atm</u>

Explanation:

The formula you would want to use it P2=p1v1/v2

Plug in the numbers and solve

(1)(6)/3.5

Let me know if you need any other help!

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How molecules of N2 gas can be present in a 2.5 L flask at 50°C and 650 mmHg?

ratelena [41]

Answer:

0.482 ×10²³ molecules

Explanation:

Given data:

Volume of gas = 2.5 L

Temperature of gas = 50°C (50+273 = 323 k)

Pressure of gas = 650 mmHg (650/760 =0.86 atm)

Molecules of N₂= ?

Solution:

PV= nRT

n = PV/RT

n = 0.86 atm × 2.5 L /0.0821 atm. mol⁻¹. k⁻¹. L × 323 k

n = 2.15 atm. L /26.52 atm. mol⁻¹.L

n = 0.08 mol

Number of moles of N₂ are 0.08 mol.

Number of molecules:

one mole = 6.022 ×10²³ molecules

0.08×6.022 ×10²³ = 0.482 ×10²³ molecules

5 0

3 years ago

True or false. The greater the distance that the plane moves from an object, the lower the force that will be applied when the

Nadya [2.5K]

Answer:

I think its false-

Explanation:

4 0

3 years ago

Read 2 more answers

Choose the isotope that would be most stable.<br> carbon-14<br> barium-56<br> lead-82<br> radon-85

shutvik [7]

The most stable isotope would be lead-82.

4 0

3 years ago

When the pressure that a gas exerts on a sealed container changes from 1100 bar to 75.5 bar, the temperature changes from k to 2

Serjik [45]

Gay-Lussac's law gives the relationship between pressure and temperature of gas. For a fixed amount of gas, pressure is directly proportional to temperature at constant volume.
P/T = k
where P - pressure , T - temperature and k - constant
$\frac{P1}{T1} = \frac{P2}{T2}$
parameters for the first instance are on the left side and parameters for the second instance are on the right side of the equation
substituting the values in the equation
$\frac{1100 bar}{T} = \frac{75.5 bar}{298 K}$
T = 4342 K
initial temperature was 4342 K

7 0

3 years ago

If the volume of the original sample in Part A ( P1 = 242 torr , V1 = 27.0 L ) changes to 80.0 L , without a change in the tempe

Brrunno [24]

The new pressure is 81.675 torr

Since temperature and moles are held constant, we use Boyle's Law:

A gas law known as Boyle's law asserts that a gas's pressure is inversely proportional to its volume when it is held at a fixed temperature and of a given mass.

To put it another way, as long as the temperature and volume of the gas remain constant, the pressure and volume of the gas are inversely proportional to one another.

The Anglo-Irish chemist Robert Boyle proposed Boyle's law in the year 1662.

P1V1=P2V2. Simply plug in your values. The units can remain in torr. Converting to atmospheres is not needed.

(242 torr)(27.0 L)=P2(80.0 L)

P2=[(242)(27)]/80 = 81.675 torr

Hence The new pressure is 81.675 torr

Learn more about Boyle's Law here

brainly.com/question/26040104

#SPJ4

3 0

1 year ago