balloon 0.113 mol of gas is as the balloon (at the mounta an dditional to volume
ID: 1061964 • Letter: B
Question
balloon 0.113 mol of gas is as the balloon (at the mounta an dditional to volume of 2.46 n psi) tempe and pressure), what is its final between with a moveable piston contains 0.553 mol of gas assume A volume of 25 mL.What is its volume if an additional 49. Which and a Assum has of gas to the cylinder? (Assume constant temperature and pressure.) ldeal Gas Law What is the volume occupied by 0.118 mol of helium gas at a m sure of 0.97 atm and a temperature of 305 K? Would the vol- ume be different if the gas was argon (under the same conditions)? 38. What is the volume occupied by 12.5 g of argon gas at a pres sure of 1.05 atm and a temperature of322 K? Would the volume be different if the sample were 12.5 g of helium (under identical conditions)? 39. What is the pressure in a 10.0 L cylinder filled with 0.448 mol of nitrogen gas at a temperature of 315 K? d0. What is the pressure in a 15.0 L cylinder filled with 32.7 g of oxygen gas at a temperature of 302 K? cylinder contains 28.5 L of oxygen gas at a pressure of 1.8 atm and a temperature of 298 K. How much gas (in moles) is in the cylinder? at is temperature of 0.52 mol of gas at a pressure of the atm and a volume of 11.8 L? automobile tire has a maximum rating of 38.0 psi The (while cold) to a volume of Land tire is inflated temperature its 120 gauge pressure of 36.0 psi at a 65.0 oC ing on a hot day, the tire warms to
Explanation / Answer
Question (36) Answer
Now We know that for Ideal gas pV = nRT
Because pressure and temperature are kept constant, you can solve this problem by using Avogadro's law, which states that, when those conditions are met, the volume occupied by an ideal gas is directly proportional to the number of moles of that gas present.other words, at constant pressure and temperature, the change in volume will be determined by the change in the number of moles.Since volume is directly proportional to number of moles, more moles will imply a bigger volume.
Mathematically, this can be written as
V1/n1=V2/n2,
where V1, n1 - the volume and the number of moles before adding more moles;
V2, n2 - the volume and number of moles after adding more moles.
The total number of moles will be n2=n1+nadded=0.553+0.365=0.918 moles
Plug your values into the equation and you'll get
V2 = (n2/n1)V1
= (0.918/0.553 )x 253 mL
V2 = 419.98 mL
As predicted, the volume increases with the increase in the number of moles of gas present.
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