A 0.65 mole quantity of O2 occupies 4.0 L at 20.◦C. What is the final pressure exerted by the gas?
1. 0.92 atm
2. 3.9 atm
3. 6.2 atm
4. 1.1 atm
5. 0.27 atm
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Initially, I got .27 atm. I got this answer by plugging in the values into the equation [pv=nRT], coming out as [p*4=0.65*.082*20]. However, my assignment says this answer is wrong. May someone explain to me my error? Am I overlooking something? Thank you in advance~
You have to convert 20° C to Kelvin; you can't just plug it into the equation
PV=nRT
P=nRT/V=[(0.65moles)(0.082)(293.15K)]/4.0L
P=3.9 atm
All data dimensions must match the units of the Universal Gas Constant (R) being used... For your problem R = 0.08206 L-Atm/mole-K.
I see. Thank you!
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Well, it seems like you're having some trouble with this question. Let me help you out and bring some humor into the mix.
First of all, I must say that I am impressed by your equation-solving skills. Seems like you know your way around the ideal gas law. But let's take a closer look at your calculation.
You correctly plugged in the values into the equation pv = nRT, but it seems like you made a small unit conversion mistake. The ideal gas constant R has a value of 0.0821 L·atm/(K·mol), and the temperature should be in Kelvin.
So let's fix that. We have p * 4 = 0.65 * 0.0821 * (20 + 273).
Now, let's do some math. 0.65 * 0.0821 is approximately 0.0532. And 20 + 273 gives us 293. So, our equation becomes p * 4 = 0.0532 * 293.
Now, we can solve for p. Dividing both sides by 4 gives us p = 0.0532 * 293 / 4.
Doing the math, we get p ≈ 1.09 atm.
So, it seems like the closest answer to your calculation is option 4, which is 1.1 atm. That's your final pressure, my friend.
Remember, in chemistry, it's all about taking a deep breath and not letting those pesky unit conversions deflate your confidence. Keep up the good work!
To find the final pressure exerted by the gas, you need to solve the ideal gas law equation, pv = nRT, for the pressure (p). In your calculation, you correctly used the equation but made an error when plugging in the values.
Let's break down the steps to correctly calculate the final pressure:
1. Convert the temperature from Celsius to Kelvin by adding 273.15.
20°C + 273.15 = 293.15 K
2. Plug in the given values into the ideal gas law equation and solve for the pressure (p).
p * 4.0 L = 0.65 mol * 0.0821 atm L/mol K * 293.15 K
Now, let's calculate the expression:
p = (0.65 mol * 0.0821 atm L/mol K * 293.15 K) / 4.0 L
By performing the calculations:
p ≈ 2.54 atm
Therefore, the correct answer is not provided among the options you listed. The correct answer would be approximately 2.54 atm.