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The numbers (1 and 2) are subscripts such as p1v1. The subscript numbers distiquish them from others of the same letter that are going to be used in the same equation. In this case there are probably 2 Pressure variables and 2 Volume variables. Since you want to use p and v for pressure and volume but there are pressures and volumes at let's say different gauges in the system then we have to distiguish the two. p1 = pressure read from gauge one and v2 is volume read from gauge 2. This, among others, is part of the energy equation for thermodynamics p1v1 = p2v2. The P is for pressure and the V is for Volume.
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This occurs to Boyle's Law.
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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 )
What is the final pressure of a 2.00 ATM gas container that increased in temperature from 299 K to 333 K while the volume increased from 650 mL to 850 mL?
P1 = 2T1 = 299T2 = 333V1 = 0.65V2 = 0.85P2t = P1 * T2 / T1 = 2.227 ATMP2v = P1 * V1 / V2 = 1.529 ATMP2 = P2t * P2v = 3.41 ATM
How can temperature be measured by determining the change in volume?
P1/t1=p2/t2
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.
What is the average velocity when a person traveling on a straight line moves with a uniform velocity v1 for x distance and v2 for next equal distance?
Let t1 and t2 be the times for the two stages. Then t1 = x/v1 and t2 = x/v2 Total distance = x + x = 2x Total time = t1 + t2 = x/v1 + x/v2 = x*(1/v1 + 1/v2) Average velocity = total distance / total time = 2x divided by x/(1/v1 + 1/v2) = 2(1/v1 + 1/v2) which is the Harmonic mean of v1 and v2.
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 )
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
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
What is the formula for Gay-Lussac?
Gay-Lussac's Law states that the pressure of a sample of gas at constant volume, is directly proportional to its temperature in Kelvin. The P's represent pressure, while the T's represent temperature in Kelvin. P1 / T1 = constant After the change in pressure and temperature, P2 / T2 = constant Combine the two equations: P1 / T1 = P2 / T2 When any three of the four quantities in the equation are known, the fourth can be calculated. For example, we've known P1, T1 and P2, the T2 can be: T2 = P2 x T1 / P1
What is gay lussacs law formula?
Gay-Lussac's Law states that the pressure of a sample of gas at constant volume, is directly proportional to its temperature in Kelvin. The P's represent pressure, while the T's represent temperature in Kelvin. P1 / T1 = constant After the change in pressure and temperature, P2 / T2 = constant Combine the two equations: P1 / T1 = P2 / T2 When any three of the four quantities in the equation are known, the fourth can be calculated. For example, we've known P1, T1 and P2, the T2 can be: T2 = P2 x T1 / P1
What is the formula for gay lussacs law?
Gay-Lussac's Law states that the pressure of a sample of gas at constant volume, is directly proportional to its temperature in Kelvin. The P's represent pressure, while the T's represent temperature in Kelvin. P1 / T1 = constant After the change in pressure and temperature, P2 / T2 = constant Combine the two equations: P1 / T1 = P2 / T2 When any three of the four quantities in the equation are known, the fourth can be calculated. For example, we've known P1, T1 and P2, the T2 can be: T2 = P2 x T1 / P1
Which of the following is not a valid equation for describing the behavior for gases?
(p1/v1) = (p2/v2)For Apex (P1 N1)= (P2N2 )
What is the relationship between density and temperature of CNG?
At low pressures you can use the ideal gas equation: (P1*V1)/T1 = (P2*V2)/T2 At constant volume, the equation will be: P1/T1 = P2/T2 At higher pressures (appr. above 10 bar) the deviation to real gas becomes significant, hence the compression factor (Z) is introduced.
P1 v1 p2 v2 represents?
p1 is pressure 1 v1 is volume 1p2 is pressure 2v2 is volume 2they are in the boyles law thing
What is the volume at stp of 720.0 ml of a gas collected at 20.0 c and 3.00 ATM pressure?
While STP is at 25oC (298 K) and 1 ATM, the ideal gas law (P1.V1 / T1 = P2.V2 / T2) states the following solution: [T2/T1]*[P1/P2]*V1 = V2[(273+25.0) K / (273+20.0) K] * [3.00 atm / 1.00 atm] * 720.0 mL =[298.0 / 293.0] * [3.00] * 720.0 = 2197 mL
Charles Law formula?
Relates that if held under constant pressure the ratio of Vol/Temp remains constant. i.e, V1 / T1 = V2 / T2 (where T is in Kelvin)
What is the final pressure of a 2.00 ATM gas container that increased in temperature from 299 K to 333 K while the volume increased from 650 mL to 850 mL?
P1 = 2T1 = 299T2 = 333V1 = 0.65V2 = 0.85P2t = P1 * T2 / T1 = 2.227 ATMP2v = P1 * V1 / V2 = 1.529 ATMP2 = P2t * P2v = 3.41 ATM
