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p1 is pressure 1 v1 is volume 1
p2 is pressure 2
v2 is volume 2
they are in the boyles law thing
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∙ 14y ago
This formula represents Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume, as long as the temperature remains constant. This means that if the pressure (P) on a gas increases, its volume (V) will decrease, and vice versa.
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Which of the following is not a valid equation for describing the behavior for gases?
(p1/v1) = (p2/v2)For Apex (P1 N1)= (P2N2 )
Can i know more Details of position Vector?
The position vector is four dimensional, a quaternion: p= w +ix + jy + kz = w = v where w=ct is a real number and v is a three dimensional vector v=ix +jy +kz. The product of positions is a transformation: p1p2 = (w1 +v1)(w2 +v2)= (w1w2 -v1.v2) + (w1v2 + w2v1 + v1xv2) The '.' and 'x' are the cosine ans sine of the angles between v1 and v2 thus: p1p2= (w1 +v1)(w2 +v2)= (w1w2 -v1v2cos(v1v2)) + (w1v2 + w2v1 + v1v2sin(v1v2)) If v1 is perpendicular to v2 then cos(v1v2) is zero and sin(v1v2) is +- 1. if v1 is parallel to v2 then sin(v1v2) is zero and cos(v1v2) is +-1. Einstein's Relativity "interval" is a contraction of p1p2= ct1ct2 - x1x2 -y1y2 -z1z2. p1p2 is also |p1p2|( Cos(p1 +p2) + sin(p1 +p2)). This implies that Einstein's "interval" is cos(p1 +p2) and the interval is zero when cos(p1 +p2) is zero or the sum of the angles p1 +p2 is a multiple of 90 degrees.
What must the pressure and volume be if the pressure of its container is reduced to half its original size?
initial volume = V1 final volume = V2 initial pressure = P1 final pressure = P2 = (1/2)P1 P1V1 = P2V2 P1V1 = (1/2)P1V2 P1 cancels; V1 = (1/2)V2 V2 = 2V2.
What happens to the air pressure inside a balloon when the balloon is squeezed to half its volume at constant temperature?
Assuming the temperature is constant and none of the air is let out of the balloon, if you half the volume, the air pressure will double. If you want it, here is the math: Air is approximately an ideal gas, so when the temperature is constant, it follows the gas law of P1*V1 = P2*V2 where P1 is the pressure at state 1 (i.e. before the balloon is squeezed), V1 is the volume at state 1, P2 is the pressure at state 2 (i.e. after the balloon is squeezed), and V2 is the volume at state 2. When you half the volume, mathematically saying V2 = 0.5*V1. When you substitute this in, your equation now becomes P1*V1 = P2*0.5*V1. The V1 on both sides will cancel, leaving you with P1 = 0.5*P2. Since you are asking about the pressure after you squeeze the balloon, you want to know P2. So if you divide both sides by 0.5, you now have P1/0.5 = P2 or equivalently P2 = 2*P1 and we see that the pressure is twice that of the original.
The temperature of an ideal gas is directly proportional to?
the equation for an ideal gas is pv / t = nr n * r is a constant for a closed system p pressure v volume t temperature in kelvin p1 v1 /t1 = p2 v2 /t2 if p1 = p2 v1/t1 = v2/t2 t2= v2/v1 *t1 directly proportional to the change in volume if v1 = v2 the same can be done and you will find that t is directly proportional to change in pressure. generally t is directly proportional to the product of pressure and volume. pv = nr t
As the pressure of a gas at 760 torr is changed to 380 torr at a constant temperature the volum of the gas will?
Boyle's law states that pressure is indirectly proportional to the volume. There fore as the pressure of a gas at 760 torr is changed to 380 torr, the volume will increase. Boyle's Law: P1 x V1 = P2 x V2 Rearranging leads to: P1 / P2 = V2 / V1 Substituting our values: 760 / 380 = V2 / V1 Thus the final volume will be twice the initial volume.
Find the ratio of linear momentum of two particles of masses 1.0kg and 4.0kg if their kinetic energy are same?
K = 1/2 m v2 K1 = K2 ===> 1/2 m1 v12 = 1/2 m2 v22 ===> 1 v12 = 4 v22 ===> V22 = 1/4 V12 === V2 = 1/2 V1Momentum = m v M1 = m1 v1 = 1 v1 M2 = m2 v2 = 4 (1/2 v1) = 2 v1 = 2 M1
What is polytropic process?
A polytropic process is a process where ( P ) ( V )^n is maintained throughout the process; commonly a compression or an expansion. The n is called the polytropic exponent and is often between 1.0 and k , the specific heat ratio. For a reversible, polytropic, and nonflow process : WB = [ ( P2 ) ( V2 ) - ( P1 ) ( V1 ) ] / [ 1 - n ] or WB = [ 1 / 1 - n ][ ( P1 ) ( V1 ] [ ( P2 / P1 )^B - 1 ] B = ( n - 1 ) / ( n ) For a reversible, polytropic, and steady flow process : WSF = [ n / 1 - n ] [ ( P1 ) ( V1 )] [ ( P2 / P1 )^B - 1 ] B = ( n - 1 ) / ( n )
What happens to the pressure of a gas when the volume of the container double in size?
You have for an Ideal Gas:PV = mRT/M( P2 ) ( V2 )/ (T2 ) ( m2 ) = ( P1 ) ( V1 ) / ( m1 ) ( T1 ) = R/M = ConstantV2 = ( V1 ) ( P1 /P2 ) ( T2/T1 ) ( m2 /m1 )You have :( P1 / P2 ) = 1.00( T2 / T1 ) = 1.00( m2 / m1 ) = 2.00V2 = ( V1 ) ( 1.000 ) ( 1.000 ( 2.000 ) = ( 2.000 ) ( V1 )
A sample of helium gas at 25 celsius is compressed from 200mL to 0.240 mL Its pressure is now 300mm Hg What was the original pressure of the helium?
To solve for the original pressure of the helium gas, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature. Using this law, we can set up the equation (P1)(V1) = (P2)(V2), where P1 is the original pressure, V1 is the original volume, P2 is the final pressure, and V2 is the final volume. Plugging in the values gives us (P1)(200 mL) = (300 mm Hg)(0.240 mL). Solving for P1 gives us P1 = (300 mm Hg)(0.240 mL) / 200 mL = 0.36 mm Hg. Therefore, the original pressure of the helium gas was 0.36 mm Hg.
The pressure of x mL of a gas was increased from 2 atm to 3 atm at constant temperature what will be the new volume?
P1V1 = P2V2 P1 = 2atm V1 = xmL P2 = 3atm V2 = ? Solve for V2: P1V1/P2 = V2 (2atm)(x mL)/3atm = 2/3x mL
At standard temperature a gas has a volume of 350 mL the temperature is then increased to 137 C and the pressure is held constant What is the new volume?
T1 = 273.15K. T2 = 410.15K. V1 = 350mL. V2 = ? P1 = P2. Since pressure is constant you can use the formula. V1/T1 = V2/T2 Rearrange the formula to get: V2 = T2V1/T1
