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sergiy2304 [10]
3 years ago
7

The volume of a given quantity of a gas must increase if:

Chemistry
1 answer:
professor190 [17]3 years ago
5 0
<span>D the temperature decreases and the pressure increases</span>
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If 125 ml of o2 gas exerts a pressure of 1.0 atm inside a cylinder, what will the pressure be if the cylinder compressed the vol
Lelu [443]
<h2>Hello!</h2>

The answer is: The new pressure is 1.67 atm.

<h2>Why?</h2>

From the statement, we know that the temperature remains constant and the gas volume is changing, meaning that the new pressure will be different than the first pressure.

Since the temperature remains constant, we can calculate the new pressure using the Boyle's Law.

The Boyle's Law states that:

P_{1}V_{1}=P_{2}V_{2}

Where,  

P is the pressure of the gas.

V is the volume of the gas.

Then, the given information is:

V_{1}=125ml=0.125L\\P_{1}=1atm\\V_{2}=75ml=0.075L

Remember, 1 L is equal to 1000 mL.

So,

125mL*\frac{1L}{1000mL}=\frac{125mL*1L}{1000mL}=0.125L\\\\75mL*\frac{1L}{1000mL}=\frac{75mL*1L}{1000mL}=0.075L

So, calculating the new volume, we have:

P_{1}V_{1}=P_{2}V_{2}\\\\1atm*0.125L=P_{2}*0.075L\\\\P_{2}=\frac{1atm*0.125L}{0.075l}=1.67atm

Hence, the new pressure is 1.67 atm.

Have a nice day!

7 0
3 years ago
A sample in made of copper and zinc. It has a high melting point, can conduct electricity in a solid and liquid state, and is ma
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2 years ago
Suppose a 0.025M aqueous solution of sulfuric acid (H2SO4) is prepared. Calculate the equilibrium molarity of SO4−2. You'll find
FromTheMoon [43]

<u>Answer:</u> The concentration of SO_4^{2-} at equilibrium is 0.00608 M

<u>Explanation:</u>

As, sulfuric acid is a strong acid. So, its first dissociation will easily be done as the first dissociation constant is higher than the second dissociation constant.

In the second dissociation, the ions will remain in equilibrium.

We are given:

Concentration of sulfuric acid = 0.025 M

Equation for the first dissociation of sulfuric acid:

       H_2SO_4(aq.)\rightarrow H^+(aq.)+HSO_4^-(aq.)

            0.025          0.025       0.025

Equation for the second dissociation of sulfuric acid:

                    HSO_4^-(aq.)\rightarrow H^+(aq.)+SO_4^{2-}(aq.)

<u>Initial:</u>            0.025            0.025      

<u>At eqllm:</u>      0.025-x          0.025+x        x

The expression of second equilibrium constant equation follows:

Ka_2=\frac{[H^+][SO_4^{2-}]}{[HSO_4^-]}

We know that:

Ka_2\text{ for }H_2SO_4=0.01

Putting values in above equation, we get:

0.01=\frac{(0.025+x)\times x}{(0.025-x)}\\\\x=-0.0411,0.00608

Neglecting the negative value of 'x', because concentration cannot be negative.

So, equilibrium concentration of sulfate ion = x = 0.00608 M

Hence, the concentration of SO_4^{2-} at equilibrium is 0.00608 M

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3 years ago
How many moles are in 4.5 g of<br> Sodium Chloride, NaCl?
Sergeu [11.5K]

Answer:

The answer to the question is 0.07 moles

6 0
2 years ago
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