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valkas [14]
2 years ago
14

A 5.00 L flask at 25˚ C contains 0.200 mol of Cl2 . What is the pressure in the flask?

Chemistry
2 answers:
hichkok12 [17]2 years ago
8 0

Answer:

Your answer would be:
0.98atm.

Explanation:

The pressure of a gas can be calculated by using the following expression:

PV = nRT

P = pressure

V = volume
-----------------------------------

n = number of moles

R = gas law constant

T = temperature

P × 5 = 0.2 × 0.0821 × 298

5P = 4.893

P = 4.893 ÷ 5 = 0.98atm

P = 0.98atm

In conclusion, the pressure of a 5.00 L flask at 25 degrees C. that contains 0.200 mol of Cl2 is 0.98atm.



Have a great rest of your day
#TheWizzer

kow [346]2 years ago
8 0

Answer:

Hello, senzawahl SORRY IF I SPELLED YOUR NAME INCORRECT
Prime here ready to solve your question :)


so your correct answer is 0.98atm.

Explanation:



Stay safe


-prime

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5 0
3 years ago
Diana raises a 1000. N piano a distance of 5.00 m using a set of pulleys. She pulls
Alina [70]

Answer:

a) 250 N

b) 50 N

c) 5000 J

d) 4

e) 3.33

Explanation:

Given that weight of piano (F_r) = 1000 N, distance moved by pulley (d_r) = 5 m and the rope used (d_e) =20 m

a) The effort applied (F_e) if it was an ideal machine is:

F_e=\frac{F_rd_r}{d_e} = \frac{1000*5}{20}=250N

b) If the actual effort  = 300 N

The force to overcome friction = actual effort - F_e = 300 - 250 = 50 N

c) Work output = F_rd_r=1000*5=5000J

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e) Input force = 300 N, Therefore:

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5 0
3 years ago
A 25.0-mL sample of an H2SO4 solution requires 50.0 mL of 0.150 M NaOH to completely react with the H2SO4. What was the concentr
Nitella [24]
V( H₂SO₄) = 25.0 mL in liters = 25.0 / 1000 = 0.025 L
 M(H₂SO₄) = ?

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number of moles NaOH :

n = M x V

n = 0.150 x <span> 0.05 
</span>
n = 0.0075 moles of NaOH 

H₂SO₄(aq) + 2 NaOH(aq) = Na₂SO₄(aq) + 2 H₂O(l)

1 mole H₂SO₄ ---------- 2 mole NaOH
? mole H₂SO₄ ---------- 0.0075 moles NaOH

moles = 0.0075 * 1 / 2

= 0.00375 moles of H₂SO₄

M(H₂SO₄) = n / V

M = 0.00375 / <span> 0.025

</span>= 0<span>.15 M
</span>
hope this helps!

8 0
3 years ago
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