0
How must the pressure be changed to double the of gas at a constant temperature?
Wiki User
∙ 10y ago
The absolute temperature must be doubled. (20'C + 273.15) = 293.15K. Doubled... (2) x (293.15) = 586.3K. (586.3K - 273.15) = 313.15'C. It must reach a temperature of 313.15'C in order to double the pressure.
Wiki User
∙ 15y ago
Wiki User
∙ 15y agoProvided the volume remains constant then Boyles law can be applied where PV is proportional to T. Hence p1 is proportional to 20C. i.e 293Kelvin. Hence to get 3xp1 to be proportional to 879Kelvin i.e 606C I believe.
Wiki User
∙ 10y agoAccording to Boyle's law, P1V1 = P2V2
Here we have P1V1 = 2P2V1
P1 = 2P2
P2 = (1/2)P1, the pressure would have to be reduced by one half.
Add your answer:
Earn +20 pts
What happens to pressure of constant mass of a gas at constant temperature when the volume is doubled?
Pressure is halved when ONLY volume is doubled (n and T are constant).Remember the General Gas Law:p.V = n.R.T(in which R=general gas constant)
According to the ideal gas law what happens to the volume of a gas when the number of moles double and all else is constant?
There are three variables in gas work that go into volume: amount of gas, pressure of gas, temperature of gas. If we double the amount of gas - the moles - and maintain the temperature and pressure, the volume must double.
Why if a gas is present at 27 Celsius its volume becomes doubled when temperature increases to 327 Celsius under constant pressure?
pV = nRT we can firstly assume that n (number of moles) and R (gas constant) do not change and as pressure is also kept constant, the temperature must be proportional to the volume. Thus if temperature is increased from 27C (300K) to 327C (600K) and is doubled, the volume must also double.
Why is it necessary to specify the temperature when giving a value for k?
The rate constant, k, varies with temperature, so the temperature at which it has been determined must be given. In general a 10 oC temperature increase will double the rate of a chemical reaction.
What temperature in degrees Fahrenheit would a fixed volume of gas need to be heated to in order to double its pressure if it starts out at?
To double the pressure, you will need double the temperature. Note that you have to use the absolute temperature (usually Kelvin) for this calculation. So, for example, if you start off at 100 degrees Celsius, you convert that to Kelvin (add 273 to convert from Celsius to Kelvin), double the number to get double the temperature, then convert back to Celsius (subtract 273 from the previous result).Similarly, if you start out at a certain number of degrees Fahrenheit, you must first convert that to Kelvin, then double the result, and finally convert this last result back to Fahrenheit.
When a sample of gas is compressed from 6.0 L to 2.0 L at a constant temperature the pressure of the gas double?
Are you stating or asking ? If that's a statement, then it's an incorrect one. At constant temperature, the product of (pressure) x (volume) is constant. So, if the volume changed by a factor of 3, the pressure must also change by a factor of 3 ... the pressure must triple.
Does doubling celsius temperature double pressure?
Using the Celsius temperature scale, it is not correct. But doubling the temperature using the Kelvin temperature scale, where zero is the absolute minimum gegree possible, will double pressure . p1/T1=p2/T2=constant.
What does Boyle's Law state?
Gases Boyle's law states that the Volume of a given amount of gas at constant Temperature varies inversely proportional to Pressure. You have a given volume of gas, and you double its pressure keeping Temperature constant, the volume will reduce by half.
Do Charles' law indicates that an increase in absolute temperature will cause a corresponding increase in volume?
Charles's law states that at constant pressure, the volume of a given mass of an ideal gas increases or decreases by the same factor as its absolute temperature. For fixed mass of an Ideal Gas at constant pressure the volume it occupies is directly proportional to its absolute temperature. So, if you double the absolute temperature of a gas while holding its pressure constant, the volume has to double. There is no such thing as an Ideal Gas. So, doubling the temperature of a real gas will not exactly double its volume. However, the general principle hold true. If you increase the temperature of any gas at constant pressure the volume it occupies will increase.
What happens to the pressure of a system when the volume is decreased if the temperature and number of gas particles are held constant according to Boyles Law?
When pressure double, the volume halves. However this is only true if the number of molecules and the temperature are both in a constant state.
What happens to the air pressure inside a balloon when it is squeezed to half its volume at constant temperature?
assuming the balloon is closed, the air pressure would double
What happens to the pressure if the temperature in K is doubled?
The initial pressure is halved. Use Boyle's law that relates pressure & volume at a constant temperature. P1V1 = P2V2 In this case the V1(initial volume) is doubled so V2 = 2V1 P2 = P1V1/V2 = P1V1/2V1 P2 = (1/2)*P1
If the volume of a container of air is reduced?
If the volume of a container of air is reduced by one half the partial pressure of the oxygen with in the container will be doubled. If the volume of a container of gas is reduced, the pressure inside the container will increase.
What happens to pressure of constant mass of a gas at constant temperature when the volume is doubled?
Pressure is halved when ONLY volume is doubled (n and T are constant).Remember the General Gas Law:p.V = n.R.T(in which R=general gas constant)
According to the ideal gas law what happens to the volume of a gas when the number of moles double and all else is constant?
There are three variables in gas work that go into volume: amount of gas, pressure of gas, temperature of gas. If we double the amount of gas - the moles - and maintain the temperature and pressure, the volume must double.
Why if a gas is present at 27 Celsius its volume becomes doubled when temperature increases to 327 Celsius under constant pressure?
pV = nRT we can firstly assume that n (number of moles) and R (gas constant) do not change and as pressure is also kept constant, the temperature must be proportional to the volume. Thus if temperature is increased from 27C (300K) to 327C (600K) and is doubled, the volume must also double.
What happens to the volume of a gas when the temperature doubles?
In a perfectly flexible and expandable container (pressure is constant) the volume of an ideal gas will double as the absolute temperature doubles. For a non-ideal gas and non-perfect container, your results will vary but will always be somewhat less than double.
