Answer:
1. 0.224 moles of oxygen
3. 143.36 L oxygen gas
5. 0.059 atm
10. 5.14 atm
11. 307 K
Explanation:
1. You have to use the ideal gas law: PV=nRT where P is pressure in atm, V is volume in liters, n is number of moles, R is the constant 0.08206 L atm mol^-1 K^-1, and T is the temperature in Kelvins where K=degrees celsius+273.15 . By rearranging the equation, you solve for n, which is n=(PV)/(RT)
P= 28.3 atm
V=0.193 L
R= 0.08206 L atm mol^-1 K^-1
T= 24.5+273.15= 297.65 K
Plugging the values in,
n=(28.3 atm x 0.193 L)/(0.08206 L atm mol^-1 K^-1 x 297.65 K)
n= 0.224 moles of oxygen
3. At STP, there are 22.4 L of gas for every mole of gas present. So 6.4 moles of oxygen would mean that there are:
6.4 mol x 22.4 L= 143.36 L oxygen gas
5. You have to use the ideal gas law: PV=nRT where P is pressure in atm, V is volume in liters, n is number of moles, R is the constant 0.08206 L atm mol^-1 K^-1, and T is the temperature in Kelvins where K=degrees celsius+273.15 . By rearranging the equation, you solve for P, which is P=(nRT)/V
n= 0.72 g converting to moles, divide by molar mass of oxygen gas: 0.72 g/32g= 0.0225 moles
V=9.3 L
R= 0.08206 L atm mol^-1 K^-1
T= 23.0+273.15= 296.15 K
Plugging the values in,
P=(0.0225 moles x 0.08206 L atm mol^-1 K^-1 x 296.15 K)/ 9.3 L
P= 0.059 atm
10. Ideal gas law again using the same equation as 5 above: You have to use the ideal gas law: PV=nRT where P is pressure in atm, V is volume in liters, n is number of moles, R is the constant 0.08206 L atm mol^-1 K^-1, and T is the temperature in Kelvins where K=degrees celsius+273.15 . By rearranging the equation, you solve for P, which is P=(nRT)/V
n= 0.108 mol
R=0.08206 L atm mol^-1 K^-1
T=20.0+273.15= 293.15 K
V= 0.505 L
Plugging the values in,
P=(0.108 mol x 0.08206 L atm mol^-1 K^-1 x 293.15 K)/0.505 L
P= 5.14 atm
11. You have to use the ideal gas law: PV=nRT where P is pressure in atm, V is volume in liters, n is number of moles, R is the constant 0.08206 L atm mol^-1 K^-1, and T is the temperature in Kelvins where K=degrees celsius+273.15 . By rearranging the equation, you solve for Y, which is T=(PV)/(nR)
P= 0.988 atm
V= 1.20 L
n= 0.0470 mol
R=0.08206 L atm mol^-1 K^-1
Plugging the numbers in,
T=(0.988 atm x 1.20 L)/(0.0470 mol x 0.08206 L atm mol^-1 K^-1)
T= 307 K
