I know the answer to your question but if you want me to answer this question first, I need your help with my question "How do I solve number 12? Quick please I need help ASAP!!!"
Answer:
v2=4.735L
Explanation:
using charles law
v1\t1 = v2\t2
v1= 4.5L
t1= 14+273= 287K ( temperature has to be in kelvins)
t2=29+273= 302K
v2=?
by substitution;
4.5\287 = v2\302
v2=(302 x 4.5)\287
v2=4.735L
Answer:
b) increases by a factor of about 2.
Explanation:
Ignore the nitrogen and oxygen. Each gas acts independently of the others.
You have 0.02 mol of CO₂ gas at some pressure in equilibrium with the CO₂ in solution.
According to Graham's Law,
S = kp
That is, the solubility of a gas in a liquid is directly proportional to its partial pressure above the liquid.
If you add another 0.02 mol of CO₂, you have doubled the number of moles.
According to Avogadro's Law, doubling the number of moles doubles the pressure.
According to Graham's Law, doubling the pressure doubles the solubility.
The solubility of CO₂ increases by a factor of two.
I've tried this like, probably 10 times, it never worksbut ig we'll see
Answer:
The pressure of CO2 = 0.48 atm
Explanation:
Step 1: Data given
Kp = 0.23
Step 2: The balanced equation
2NaHCO3(s) ↔ Na2CO3(s) + CO2(g) + H2O(g)
Step 3: Calculate the pressure of CO2
Kp = (p(CO2))*(p(H2O))
For 1 mol CO2 we have 1 mol H2O
x = p(CO2) = p(H2O)
Kp = 0.23 = x*x
x = √0.23
x = 0.48
pCO2 = x atm = 0.48 atm
The pressure of CO2 = 0.48 atm
