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A gas sample is prepared in which the components have the following partial pressures: nitrogen, 555 mmHg; oxygen, 149 mmHg; water vapor, 13 mmHg; argon, 7 mmHg. What is the total pressure of this mixture?
The law explains that a gas in a mixture exerts its own pressure independent of any other gas (if non-reactive gases) and the total pressure is the sum of the...
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If the initial temperature of an ideal gas at 2.250 atm is 62.0 degrees C, what final temperature would cause the pressure to be reduced to 1.750 atm?
This question is an example of Gay-Lussac's law relating temperature and pressure. This law states that the pressure of a given amount of gas held at constant volume is directly...
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A sample of chlorine gas occupies a volume of 946 mL at a pressure of 726 mmHg. What is the pressure of the gas (in mmHg) if the volume is reduced at constant temperature to 154 mL?
$P_1V_1=P_2V_2$ at $"constant temperature"$. $P_2=(P_1V_1)/V_2=(946*cancel(mL)xx(726*cancel(mm*Hg))/(760*cancel(mm*Hg)*atm^-1))/(154*cancel(mL))=??atm$ Note that you do NOT measure a pressure that is over $1*atm$ in $mm*Hg$. You do this and you will get mercury all over the...
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What is the initial pressure of a gas having an initial temperature of 90.5 K, an initial volume of 40.3 L, a final pressure of 0.83 atm, a final temperature of 0.54 K and a final volume of 2.7 L?
$PV = nRT$ $(PV)/T = nR$ $therefore (P_1V_1)/T_1 = (P_2V_2)/T_2$, the . $(P_1*"40.3 L")/("90.5 K")=("0.83 atm"*"2.7 L")/("0.54 K")$ $P_1 approx 9.3atm$
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If the initial temperature of an ideal gas at 2.250 atm is 62.00 $"^o$C, what final temperature would cause the pressure to be reduced to 1.500 atm?
So, we convert the temperatures to the absolute scale, and solve the quotient: $T_2=(T_1xxP_2)/P_1=(335.15*Kxx1.500*atm)/(2.250*atm)=223*K$ You should convert this temperature back to the $"Celsius scale"$. It is intuitively sound that a...
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If the initial temperature of an ideal gas at 2.250 atm is 62.00 °C, what final temperature would cause the pressure to be reduced to 1.600 atm?
Gay-Lussac's law: For a given mass and constant volume of an ideal gas, the pressure exerted on the sides of its container is directly proportional to its absolute temperature. Mathematically,...
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A gas takes up a volume of 17.5 liters, has a pressure of 2.31 atm, and a temperature of 299 K. lf the temperature is increased to 350 K and the pressure is decreased to 1.75 atm, what is the new volume of the gas?
And so.................. $V_2=(P_1xxV_1xxT_2)/(T_1xxP_2)$ $=(2.31*atmxx17.5*Lxx350*K)/(299*Kxx1.75*atm)<=30*L.$
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A sample of carbon dioxide gas at a pressure of 1.07 atm and a temperature of 166 °C, occupies a volume of 686 mL. If the gas is heated at constant pressure until its volume is 913 mL, the temperature of the gas sample will be ? °C.
The idea here is that the volume and the temperature of a gas have a direct relationship when the pressure and the number of moles of gas are being kept...
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An ideal gas sample is confined to 3.0 L and kept at 27°C. If the temperature is raised to 77°C and the initial pressure was 1500 mmHg, what is the final pressure?
Use the equation: $(P_1xxV_1)/T_1=(P_2xxV_2)/T_2$ The gas is confined in 3.0 L container ( rigid container) $=>$ the volume remains constant when the temperature is increased from from $27^oC$ to $77^oC$...
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What is the initial pressure of a gas having an initial temperature of 90.5K, an initial volume of 40.3 L, final pressure of .83 atm, a final temperature of .54 K and a final volume of 2.7L?
Use the . $(P_1V_1)/T_1=(P_2V_2)/T_2$ Given $V_1="40.3 L"$ $T_1="90.5 K"$ $P_2="0.83 atm"$ $V_2="2.7 L"$ $T_2="0.54 K"$ Unknown $P_1$ Equation $(P_1V_1)/T_1=(P_2V_2)/T_2$ Solution Rearrange the equation to isolate $P_1$ and solve. $P_1=(P_2V_2T_1)/(T_2V_1)$ $P_1=((0.83"atm"...
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