Other things being equal, pressure is proportional to temperature. The temperature must be in an absolute scale. So, just convert the temperatures to kelvin, and then compare them - see by what factor the temperature increases. The pressure will increase by the same factor.
If the pressure stays constant then Charles' Law could be applied.
V1/T1 = V2/T2
Temperature must be converted to absolute temperature by adding 273. O oC = 273 K
Substituting:
5.0 / 278 = V2 / 283
V2 = 5.0 x 283 / 278
V2 = 5.09 L
= 5.1 L (2 significant figures)
(323 times 2)/3 = 273x/1 where x = v2
646/3=273x
x= (215 + 1/3)/273 = 8x10(-1) liters, or 0.8 liters.
A 3.0 L sample of nitrogen gas has a pressure of 1.0 ATM and a temperature of 75 k, the new volume in liters of the sample when the pressure is 2.0 ATM and a temperature of 225 k is 4.5 L.
The Gay-Lussac law: P x T =k
5.0
90
Yes, it does affect the volume. The relationship between them can be explained by the equation pV=nRT (pressure x volume = number of moles of gas x molar gas constant x temperature). Therefore, there is a direct proportionality between temperature and volume. If the temperature doubles, so does the volume.
An Arrhenius equation is an equation which approximates the dependence of the rate of any chemical reaction on the temperature.
The universal gas equation is PV = nRT (Pressure x Volume = Number of moles x Universal Gas Constant x Temperature in Kelvin/Rankin). So - if Pressure is constant, the number of moles is constant, but the temperature increases from 25C (298 K) to 125C (398K) - a 34% increase, a similar 34% increase in volume will occur.
The temperature, pressure, and volume of gases can be related by the ideal gas equation. PV = nRT where P is pressure, V is volume, n is moles, R is that ideal gas constant, and T is the temperature in Kelvin.
I'd use a graph showing an exponential decrease: as pressure increases, volume decreases.
You can use the Ideal Gas Equation: pV=nRT or p1V1/T1 = p2V2/T2
Sound travels faster as temperature increases, so there is no limit. There is an equation to determine the speed of sound at a given temperature.
Air warms up when it gets compressed. The equation is PV = NrT where P is pressure, V is volume, N is a number of molecules, r is the gas constant and T is the temperature.
For a fixed mass of gas, the gas will become compressed by pressure and its volume will decrease. This is why pressurized gas containers explode when breached: the container breach eliminates the barrier between the gas compressed by the container and the outside air; the pressurized gas immediately increases the volume it occupies in the explosive decompression until its density equals the density of the regular atmosphere.
Correct the transaction so that the double entry also increases the right hand side of the accounting equation so that the equation (always) balances.
when x increases y increases.. y=kx
Yes, it does affect the volume. The relationship between them can be explained by the equation pV=nRT (pressure x volume = number of moles of gas x molar gas constant x temperature). Therefore, there is a direct proportionality between temperature and volume. If the temperature doubles, so does the volume.
Newton's equation of cooling is a differential equation. If K is the temperature of a body at time t, then dK/dt = -r*(K - Kamb) where Kamb is the temperature of the surrounding, and r is a positive constant.
The potential energy of a spring is defined by this equation: U=.5kx2 U= potential energy (in joules) k= the spring constant x= the displacement of the spring from equilibrium. (the amount that the spring is stretched or compressed) This equation tells us that as a spring is compressed by a distance x, the potential energy increases proportionately to x2
An Arrhenius equation is an equation which approximates the dependence of the rate of any chemical reaction on the temperature.
If I remember correctly it is a little more complicated than that. The general equation PV=nRT for an ideal gas is elementary knowledge. The fact is that when you increase temperature many things can happen. It depends on how you treat your system. In general if you increase temperature in an open system the pressure will remain fairly constant, but the volume will increase. If it is a closed system in which the volume is not allowed to expand the pressure will increase with increased temperature. You also have to remember chemical properties also such as phase changes. Hope that rambling mess helps lol.
In the ideal gas equation the temperature is in kelvins.