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2 years ago

If a gas at 25.0 °C occupies 3.60 liters at a pressure of 1.00 atm, what will be its volume at a pressure of 2.50 atm?

2 answers:

8 0

Since the temperature is constant, therefore, this problem can be solved based on Boyle's law.
Boyle's law states that: " At constant temperature, the pressure of a certain mass of gas is inversely proportional to its pressure".

This can be written as:
P1V1 = P2V2
where:
P1 is the initial pressure = 1 atm
V1 is the initial volume = 3.6 liters
P2 is the final pressure = 2.5 atm
V2 is the final volume that we need to calculate

Substitute with the givens in the above mentioned equation to get the final volume as follows:
P2V1 = P2V2
1(3.6) = 2.5V2
3.6 = 2.5V2
V2 = 3.6 / 2.5 = 1.44 liters

yaroslaw [1]2 years ago

6 0

(1.00 atm) (3.60 liters) =(2.5 atm ) (x); x= 1.44 L

I hope that helped

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1 year ago

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Under standard conditions, a given reaction is endergonic (i.e., ΔG >0). Which of the following can render this reaction favo

sleet_krkn [62]

Answer:

Maintaining a high starting-material concentration can render this reaction favorable.

Explanation:

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Q is the reaction quotient

To make ΔG < 0 when ΔG° > 0 we need to make the term R.T.lnQ < 0. Since T is always positive we need lnQ to be negative, what happens when Q < 1. Q < 1 implies the concentration of reactants being greater than the concentration of products, that is, maintaining a high starting-material concentration will make Q < 1.

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2 years ago

The volume of distilled water that should be added to 10.0 mL of 6.00 M HCl(aq) in order to prepare a 0.500 M HCl(aq) solution i

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Answer:

110ml

Explanation:

Using the dilution equation, C1V1 = C2V2

Where C1 is the initial concentration of solution

C2 is final concentration of solution

V1 is intital volume of solution

V2 is final volume of solution.

From the question , C1=6M, C2=0.5M, V1=10ml, V2=?

$V2 =\frac{C1V1}{C2}$

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