Answer:
1837.89 Lt
Explanation:
The chemical reaction for this situation is:
NaHCO₃ + HCl → NaCL + H₂O + CO₂ ₍g₎
Where the mola mass we need are:
M NaHCO₃ = 84 g/mol
M CO₂ = 44 g/mol
As we have 6.00 Kg of sodium bicarbonate, then:
6 Kg NaHCO₃ = 71.43 moles of NaHCO₃
Due the stoichiometry of this chemaicl reaction:
1 mol NaHCO₃ = 1 mol CO₂
71.43 moles NaHCO₃ = 71.43 moles CO₂
And considering that CO₂ is an ideal gas, we can use the following formula:
PV=nRT
V = (nRT)/P
n = 71.43 mol
R = 0.083 Ltxatm(molxK)
T = 37°C = 310 K
P = 1 atm
So: V = (71.43x0.083x310)/1
V CO₂ = 1837.89 Lt
Use the ideal gas law:
<em>PV=nRT
</em>p = pressure
v = volume
n = number of moles of sample
R = ideal gas constant = ~0.08206 (l*atm)/(K*mole)
T = Temp in Kelvin
Now we substitute while simultaneously solving for P(pressure)
P = (nRT)/V
P = (2.50 * 0.08206 * (27+273.15)) / 50
P = Now it's your turn.
<span>1.44x10^23 molecules of oxygen gas
The ideal gas law is
PV = nRT
where
P = pressure (800.0 Torr)
V = volume (5.60 L)
n = number of moles
R = Ideal gas constant (62.363577 L*Torr/(K*mol) )
T = absolute temperature (27C + 273.15 = 300.15 K)
Let's solve for n, the substitute the known values and solve.
PV = nRT
PV/RT = n
(800.0 Torr*5.60 L)/(62.363577 L*Torr/(K*mol)*300.15 K) = n
(4480 L*Torr)/(18718.42764 L*Torr/mol) = n
0.239336342 mol = n
So we have 0.239336342 moles of oxygen molecules. To get the number of atoms, we need to multiply by avogadro's number, so:
0.239336342 * 6.0221409x10^23 = 1.44x10^23</span>
First part is polar, second part is non-polar. Use the saying "like dissolves like". Substances that are alike in polarity are more likely to dissolve one another.
