1. V1 = 550 mL / 1000 = 0.550 L
P1 = 758 mmHg / 760 = 0.997 1 atm
V2 = ¿?
P2 = (1/2 VECES MAYOR) = 0.997 + 0.5 = 1.497 = 1.5 atm
Aplicar Ley de Boyle = (V1 x P1 = V2 x P2)
V2 = (0.550 L x 1 atm) / 1.5 atm
V2 = 0.3663 L x 100 = 366.67 mL
2. Aplicar ley de Charles = ( V1/T1 = V2/T2)
V1 = 360 mL / 1000 = 0.360 L
T1 = 27 ºC + 273 = 300 K
T2 = - 23 ºC + 273 = 250 K
V2 = (0.360 L x 250 K) / 300 K
V2 = 0.3 L x 1000 = 300 Ml
3. Aplicar ley de los gases ideales = V x P = n x R x T
V = 11.5 pie3
1 pie3 --- 28.316 L
11.5 pie3 --- x
X = 325.634 L
T = 72 ºF
K = (ºF – 32) / 1.8 + 273
K = (72 – 32) / 1.8 + 27
K = 295.9
P = 1 atm
R = 0.0821 (L atm / mol K)
Calcular n (moles)
n = (325.634 L x 1 atm)/(0.0821 (L atm / mol K) x 295.9 K)
n = 13.404 moles
calcular Volumen
1 mol ---- 22.4 L
13. 404 mol ---- x
X = 300.25 L
Calcular el volumen en pie3
V = 300.25 / 28.317 = 10.603 pie3
4. Aplicar Ley de los gases ideales = V x P = n x R x T
V = 149 mL / 1000 = 0.149 L
T = 25 ºC + 273 = 298 K
P = 755 mmHg / 760 = 0.99 atm
V gas CN= ¿?
n = ( 0.149 L x 0.99 atm) /( R = 0.0821 (L atm / mol K) x 295 k)
n = 0.0061 moles
calcular volumen en CN
0.0061 mol ---- x
X = 0.136 L x 1000 = 136 mL
5. Aplicar ley general de los gases = ( V1 x P1 /T1 = V2 x P2/T2)
V1 = 333 mL / 1000 = 0.333 L
T1 = 25 ºC + 273 = 298 K
P1 = 750 mmHg / 760 = 0.986 atm
T2 = - 11 ºC + 273 = 262 K
P2 = 730 mmHg / 760 = 0.961 atm
Calcular V2
V2 = (0.333 L x 0.986 atm x 262 K) / (0.961 atm x 298 K)
V2 = 0.300 L x 1000 = 300 mL
6. Aplicar ley general de los gases = ( V1 x P1 /T1 = V2 x P2/T2)
T1 = 77 ºF
K = (ºF – 32)/1.8 + 273
K = (77 – 32)/ 1.8 + 273 = 298 K
P1 = 14.7 lb/pulg2
1 lb/pulg2 ---- 0.06805 atm
14.7 lb/pulg2 --- x
X = 1.00 atm
T2 = 70 ºF
K = (70 – 32)/ 1.8 + 273 = 294 K
P2 = 2000 lb/pulg2
2000 lb/pulg2 --- x
X = 136 atm
V2 = 10 cilindros capacidad c/u = 2 pie3 = 20 pie3 = 566.34 L
V1 = (566.34 L x 136 atm x 298 K) / ( 1 atm x 294 K)
V1 = 78127.2 L / 28.317 = 2757 pie3
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1. V1 = 550 mL / 1000 = 0.550 L
P1 = 758 mmHg / 760 = 0.997 1 atm
V2 = ¿?
P2 = (1/2 VECES MAYOR) = 0.997 + 0.5 = 1.497 = 1.5 atm
Aplicar Ley de Boyle = (V1 x P1 = V2 x P2)
V2 = (0.550 L x 1 atm) / 1.5 atm
V2 = 0.3663 L x 100 = 366.67 mL
2. Aplicar ley de Charles = ( V1/T1 = V2/T2)
V1 = 360 mL / 1000 = 0.360 L
T1 = 27 ºC + 273 = 300 K
V2 = ¿?
T2 = - 23 ºC + 273 = 250 K
V2 = (0.360 L x 250 K) / 300 K
V2 = 0.3 L x 1000 = 300 Ml
3. Aplicar ley de los gases ideales = V x P = n x R x T
V = 11.5 pie3
1 pie3 --- 28.316 L
11.5 pie3 --- x
X = 325.634 L
T = 72 ºF
K = (ºF – 32) / 1.8 + 273
K = (72 – 32) / 1.8 + 27
K = 295.9
P = 1 atm
R = 0.0821 (L atm / mol K)
Calcular n (moles)
n = (325.634 L x 1 atm)/(0.0821 (L atm / mol K) x 295.9 K)
n = 13.404 moles
calcular Volumen
1 mol ---- 22.4 L
13. 404 mol ---- x
X = 300.25 L
Calcular el volumen en pie3
V = 300.25 / 28.317 = 10.603 pie3
4. Aplicar Ley de los gases ideales = V x P = n x R x T
V = 149 mL / 1000 = 0.149 L
T = 25 ºC + 273 = 298 K
P = 755 mmHg / 760 = 0.99 atm
V gas CN= ¿?
R = 0.0821 (L atm / mol K)
Calcular n (moles)
n = ( 0.149 L x 0.99 atm) /( R = 0.0821 (L atm / mol K) x 295 k)
n = 0.0061 moles
calcular volumen en CN
1 mol ---- 22.4 L
0.0061 mol ---- x
X = 0.136 L x 1000 = 136 mL
5. Aplicar ley general de los gases = ( V1 x P1 /T1 = V2 x P2/T2)
V1 = 333 mL / 1000 = 0.333 L
T1 = 25 ºC + 273 = 298 K
P1 = 750 mmHg / 760 = 0.986 atm
V2 = ¿?
T2 = - 11 ºC + 273 = 262 K
P2 = 730 mmHg / 760 = 0.961 atm
Calcular V2
V2 = (0.333 L x 0.986 atm x 262 K) / (0.961 atm x 298 K)
V2 = 0.300 L x 1000 = 300 mL
6. Aplicar ley general de los gases = ( V1 x P1 /T1 = V2 x P2/T2)
T1 = 77 ºF
K = (ºF – 32)/1.8 + 273
K = (77 – 32)/ 1.8 + 273 = 298 K
P1 = 14.7 lb/pulg2
1 lb/pulg2 ---- 0.06805 atm
14.7 lb/pulg2 --- x
X = 1.00 atm
T2 = 70 ºF
K = (ºF – 32)/1.8 + 273
K = (70 – 32)/ 1.8 + 273 = 294 K
P2 = 2000 lb/pulg2
1 lb/pulg2 ---- 0.06805 atm
2000 lb/pulg2 --- x
X = 136 atm
V2 = 10 cilindros capacidad c/u = 2 pie3 = 20 pie3 = 566.34 L
V1 = (566.34 L x 136 atm x 298 K) / ( 1 atm x 294 K)
V1 = 78127.2 L / 28.317 = 2757 pie3