Answer:
The new volume is 7,606.96 Liter.
Explanation:
The combined gas equation is,
where,
= initial pressure of gas in the balloon = 0.918 atm
= final pressure of gas in the balloon = 0.0012 atm
= initial volume of gas in the balloon =
= final volume of gas in the balloon = ?
= initial temperature of gas in the balloon =
= final temperature of gas in the balloon =
Now put all the given values in the above equation, we get:
The new volume is 7,606.96 Liter.
Answer:
P=4184.36 torr
Explanation:
For this problem we can use the idea gas law,
where P is pressure, V is volume, n is moles of substance, R is the constant, and T is temperature, We will need to manipulate it and a couple values so that we can get our answer in torr. To do this, let's rearrange the equation to solve for P.
Next, let's convert T (32) to kelvin. To do this, add 273 to the value.
Next, let's convert 28g of N2 to moles of N2. To do this, divide 28 by the molar mass of N2 (28.02)
moles of N2
Next, we need to find out what value of R we need to use. Because you want your answer in torr, we will need to use the value of
Now that we have all of our values, let's plug them into the equation (I'll be excluding units for simplicity but they cancel out to leave units of torr in the answer)
P=4184.36 torr
<em>Very briefly</em>, I don't know what your periodic table looks like, but mine has nitrogen's molar mass as 14.01. If you have a different mass of nitrogen, this pretty drastically impacts the value. For example, if your nitrogen's molar mass was rounded to 14.0 (making N2 28g) then it would be one mole instead of .99 moles, raising the answer to 4228.70 torr. If you have any different values just plug them in in their proper spots. A similar concept applies to the Kelvin conversion.