Answer:
Less than 7 so it is going to be acidic.
Explanation:
A buffer solution is one that resists changes in pH when small quantities of an acid or an alkali are added to it. An acidic buffer solution is simply one which has a pH of less than 7. Acidic buffer solutions are commonly made from a weak acid and one of its salts - often a sodium salt.
The balanced chemical reaction is:
CH4 + 2O2 —> CO2 + 2H2O
You need to convert mass to moles (divide by molar mass):
CH4 moles = 5 / 16 = 0.31 mol
O2 moles = 5 / 32 = 0.16 mol
To figure out which reactant is limiting, divide the actual moles by the corresponding coefficient in the reaction:
CH4: 0.31 / 1 = 0.31
O2: 0.16 / 2 = 0.08
O2 is the lower number, so it is the limiting reactant. From the reaction we know it takes 2 moles of O2 to react with each mole of CH4. Therefore, for however many moles of O2 we actually have, half as many moles of CH4 will react. Since we have 0.16 mol of O2, only 0.08 mol of CH4 will react, leaving behind 0.31 - 0.08 = 0.23 mol of CH4.
Now convert back to mass (multiply by molar mass) to find the mass of CH4 remaining:
0.23 x 16 = 3.68g
The closest answer is B.
The reaction equation is first order with respect to [H+]
when PH1 = -㏒[H+]1 so, when PH = 6
So by substitution:
∴ 6 = -㏒[H+]1
∴[H+]1 = 1 x 10^-6
and when PH2 = -㏒[H+]2 so, when PH2 = 2
so by substitution:
∴ 2 = -㏒[H]2
∴[H]2 = 1 x 10^-2
So the rate of reaction changes by the factor of:
[H2]2/[H]1 = (1 x 10^-2) / (1 x 10^-6) = 10000
It is 10000 times faster when PH decreases from 6 to 2
