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Gay-Lussac's Law deals with pressure and temperature.
If we rearrange and get
Since temperature needs to be in Kelvin for all gas law calculations,
That answer = 317.866666666666667
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You have a sample of neon gas at a certain pressure, volume, and temperature. You double the volume, double the number of moles of neon, and double the Kelvin temperature. How does the final pressure (Pf) compare to the original pressure (Po) ?
The final pressure will double as well. If you use the equation, $PV = nRT$, to express the initial and the final states of your gas sample, you can...
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If a sample of N gas was put into a flexible container at an pressure of 25.5kPa, temperature of 35.9 C and a volume of 500. mL, what would the final temperature of the gas be if the pressure was changed to .625 atm and the volume was change to 625mL?
First look at the things that need to be converted $35.9 ^@"C" = "(35.9 + 273.15) K" = "309.0 K"$ $"25.5 kPa = 0.2467 atm"$ $"500 mL = 0.500 L"$...
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Container A holds 757 mL of ideal gas at 2.60 atm. Container B holds 164 mL of ideal gas at 4.80 atm. If the gases are allowed to mix together, what is the resulting pressure?
The ideal gas equation of state is $PV = nRT$ In this problem we may consider the temperature to be constant, so we can set up an equation that...
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The gas in a container is at a pressure of 3.00 atm at 25°C. Directions on the container wam the user not to keep it in a place where the temperature exceeds 52°C. What would the gas pressure in the container be at 52°C?
We apply $P_1/T_1=P_2/T_2$ The initial pressure, $P_1=3.00atm$ The initial temperature $T_1=25+273=298K$ The final temperature $T_2=52+273=325K$ The final pressure is $P_2=T_2/T_1*P_1$ $=325/298*3=3.27atm$
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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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A balloon has a volume of 2.9 L at 320 Kelvin. If the temperature is raised to 343 Kelvin, what will its volume be?
Using , $V_1/T_1 = V_2/T_2$ Therefore $V_2 = T_2.V_1/T_1$ = $ 343 . 2.9/320$ = 3.11 litre. However, this assumes that the material from which the balloon is made is...
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Nitrogen gas (N2) reacts with hydrogen gas (H2) to form ammonia (NH3). At 200°C in a closed container, 1.05 atm of nitrogen gas is mixed with 2.02 atm of hydrogen gas. At equilibrium the total pressure is 2.02 atm. What is the partial pressure of hydrogen gas at equilibrium?
First, write the balanced chemical equation for the equilibrium and set up an ICE table. $color(white)(XXXXXX)"N"_2 color(white)(X)+color(white)(X)"3H"_2 color(white)(l)⇌ color(white)(l)"2NH"_3$ $"I/atm": color(white)(Xll)1.05 color(white)(XXXl)2.02 color(white)(XXXll)0$ $"C/atm": color(white)(X)-x color(white)(XXX)-3x color(white)(XX)+2x$ $"E/atm": color(white)(l)1.05- x...
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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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A 3.00 liter sample of gas is at 288 K and 1.00 atm. If the pressure of the gas is increased to 2.00 atm and its volume is decreased to 1.50 liters, what will be the Kelvin temperature of the sample?
When you are given this much information in the context of a generic, unnamed gas, it's a good idea to consider the : $PV = nRT$ Before we...
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The pressure of 4.2 L of nitrogen gas in a flexible container is decreased to one-half its original pressure, and its absolute temperature is increased to double the original temperature. What is its volume now?
Your tool of choice for this problem will be the equation, which looks like this $color(blue)((P_1V_1)/T_1 = (P_2V_2)/T_2)" "$, where $P_1$, $V_1$, $T_1$ - the pressure, volume, and...
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