Topic: Chemistry Homework Boyle's law.?**Question:**
do a few problems show work then maybe ill get it thanks :)
A sample of nitrogen at 20C was compressed from 300 mL to and its new pressure was found to be 400.0 Pa. what was the orginal pressure in kPa?
The pressure on 6.0 L of a gas is 200 kPa. What will be the volume if the pressure is doubled, keeping the temperature constant?
What would be the new volume if the pressure on 600 mL is increased from 90 kPa to 150 kPa?
EDIT!!!!! FIRST ONE MENT TO SAY:
A sample of nitrogen at 20C was compressed from 300 mL to 0.360 and its new pressure was found to be 400.0 Pa. what was the orginal pressure in kPa?

June 19, 2019 / By Tricia

Boyles Law is P1V1=P2V2 You can't use Boyle's law to solve this first one, unless you just left out the new Volume 6l200kpa=v400kpa which comes out to 3.0 L 600ml90kpa=v150kpa which comes out to 360 mL or 3.6L

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Did you like the answer? There are three parameters involved in a given mass of a gas, pressure, volume and temperature. Once we say that for a given mass of a gas, the mass is fixed. Thus there are three possibilities to find the nature of the gas that is how they behave when the quantities involved are changed. We keep the temperature constant and find how pressure and volume varies. Boyle' studied these relations and hence it is called Boyle's law. As per this law, When temperature remains constant the product of pressure and volume is a constant, PV is a constant. Similarly we can keep the volume constant and change the pressure and temperature. In that case P/T is a constant. And we can keep the pressure constant and change the volume and temperature. In that case V/T is a constant. Both the above two variations were studied by Charlie's and hence they are called Charlie's law. Combining the above three laws we write the gas equation PV = μR*T for any mass of a gas. R is a universal constant and μ is the number of moles. Among the four quantities P, V, T and μ, we can fix any two quantities and can write the relation between the other two. If the three quantities are known, then naturally the fourth one is fixed and cannot change. ======================================... Charles's Law was also known as the Law of Charles and Gay-Lussac, because Gay-Lussac published it in 1802 using much of Charles's unpublished data from 1787. However, in recent years the term has fallen out of favor, and Gay-Lussac's name is now generally associated with the law of combining volumes. Amontons's Law, Charles's Law, and Boyle's law form the combined gas law. The three gas laws in combination with Avogadro's Law can be generalized by the ideal gas law.

In case of nitrogen to calculate the stress you're able to be able to desire to correctly known the quantity which isn't given. The Boyle's regulation stats that stress of a gas at given Temperature is inversely proportional to its quantity If P will develop quantity reduces.or we are able to declare PV=consistent or P1V1=P2V2 so calculate for the given records.

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In case of nitrogen to calculate the pressure you need to know the volume which is not given. The Boyle's law stats that pressure of a gas at given Temperature is inversely proportional to its volume If P increases Volume reduces.or we can say PV=constant or P1V1=P2V2 so calculate for the given data.

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For all of these, just use the equation: P1V1 = P2V2 Just plug in the values you know and solve for the one you don't know.

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Basically, since you know that there are 2 mols of Na per 1 mol of O... The simplest way to do this would be to make a ratio: Since 1 mol of Na is 22.99 g and we have 2 mols of Na in 1 mol of Na2O, then it takes up, 45.98 g out of the total 61.98 g. so... 45.98/61.98 = x/6.2 --> x = aprox. 4.599 so basically 4.6g Hope that helps :D

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