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A sample of oxygen occupies a volume of 45ml at 91 Degrees Celsius. What will be the volume of oxygen when temperature drops at 10 Degrees Celsius
V1/T1 = V2/T245/364 = V2/283V2= 34.99ml
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A balloon containing 0.56 mol of helium has a volume of 10.0 L. What volume will the balloon occupy if helium is lost and only 0.21 mol remain?
According to the ideal gas law pV1 = n1RT - at the beginning pV2 = n2RT - after part of helium is lost p (pressure), T(temperature), R (universal gas constant)...
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A balloon filled with helium has a volume of 37.1 L 37.1 L at 285 K. 285 K. What volume will the balloon occupy at 253 K? 253 K?
Volume =32.93L
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If the temperature of the helium balloon were increased from 30°C to 35°C and the volume of the balloon only expanded from 0.47L to 1.55L, how much pressure would be inside the balloon?
According to the gas law equation:p1V1/T1 = p2V2/T2where p1 - initial pressure, V1 - initial volume, T1 - initial temperature, p2 - final pressure, V2 - final volume, T2 -...
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a ballon filled with helium gas at 1.00atm occupies 11.9L. what volume would the volume occupy in the upper atmosphere, at a pressure of 0.17atm and a constant temperature?
The equation states that product of pressure and volume is a constant for a given mass of confined gas as long as the temperature is constant. For comparing the same...
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At standard temperature and pressure (0 ∘C and 1.00 bar), 1.00 mol of an ideal gas occupies a volume of 22.7 L. What volume would the same amount of gas occupy at the same pressure and 30 ∘C ?
t(0)=0 С T=273 K p=1.00 bar V=22.7 l N=1 mol t(1)=30 С T=303 K Find V=? According to the Boyle-Mariotte law P(0) V(0)/T(0) = const If p=const V(0)/T(0)= V(1)/T(1) V(1)=V(0)T(1)/T(0)=22.7...
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At standard temperature and pressure (0 ∘C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume would the same amount of gas occupy at the same pressure and 95 ∘C ?
P1 = P2 = 1.00 atm = constant;V1 = 22.4 L;T1 = 0 °C = 273.15 K;T2 = 95 °C = 368.15 K;V2 = unknown;Solution:(P1×V1)/(T1) = (P2×V2)/(T2);P1 = P2 =...
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a 275L helium balloon is heated from 20 degrees celsius to 40 degrees celsius. what is the final volume at constant pressure?
pV=nRT.VxT2/T1= 275 x 40/20 = 550.
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You have 200.0 cm3 of nitrogen (IV) oxide at a temperature of 303.0 K and a pressure of 101.0 kPa. What volume will the NO2 occupy ar 255.0 kPa and 371.0 K? cm3
97 sm3
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A gas at a constant temperature occupies a volume of 2.10 L and exerts a pressure of 98.3 kPa. What volume will the gas occupy at a pressure of 115.5 kPa?
Using the boyle's ruleV1P1=V2P2V1=2.1 V2=? P1=98.3 P2=115.5V2=V1P1/P2V2=2.1×98.3/115.5V2=1.79L
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