Answer:
Water uses adhesive forces that allow it to stick to certain surfaces such as glass.
Explanation:
When the angle between vertical direction and the glass wall is small, surface tension is stronger and the component of gravity perpendicular to the glass wall is small. The result of this causes water to stick to the side of a glass.
Hope this helps!
Answer:
No, you cannot
Explanation:
One of the major properties a cancer drug must have is that, it must be highly specific. If a drug that poisons enzymes of anaerobic metabolism is used on a cancer patient, it should be noted that the drug will not only kill cancer cells but will also kill under cells that make use of anaerobic metabolism. Hence, this drug is not a specific to cancer cells but will also affect other normal cells in the patient's body. Thus, it would be wrong to use such drugs to treat cancer.
Answer:
0.124 M
Explanation:
The reaction obeys second-order kinetics:
![r = k[BrO^-]^2](https://tex.z-dn.net/?f=r%20%3D%20k%5BBrO%5E-%5D%5E2)
According to the integrated second-order rate law, we may rewrite the rate law in terms of:
![\dfrac{1}{[BrO^-]_t} = kt + \dfrac{1}{[BrO^-]_o}](https://tex.z-dn.net/?f=%5Cdfrac%7B1%7D%7B%5BBrO%5E-%5D_t%7D%20%3D%20kt%20%2B%20%5Cdfrac%7B1%7D%7B%5BBrO%5E-%5D_o%7D)
Here:
is a rate constant,
![[BrO^-]_t](https://tex.z-dn.net/?f=%5BBrO%5E-%5D_t)
is the molarity of the reactant at time t,
![[BrO^-]_o](https://tex.z-dn.net/?f=%5BBrO%5E-%5D_o)
is the initial molarity of the reactant.
Converting the time into seconds (since the rate constant has seconds in its units), we obtain:
Rearranging the integrated equation for the amount at time t:
![[BrO^-]_t = \dfrac{1}{kt + \dfrac{1}{[BrO^-]_o}}](https://tex.z-dn.net/?f=%5BBrO%5E-%5D_t%20%3D%20%5Cdfrac%7B1%7D%7Bkt%20%2B%20%5Cdfrac%7B1%7D%7B%5BBrO%5E-%5D_o%7D%7D)
We may now substitute the data:
![[BrO^-]_t = \dfrac{1}{0.056 M^{-1}s^{-1}\cdot 60.0 s + \dfrac{1}{0.212 M}} = 0.124 M](https://tex.z-dn.net/?f=%5BBrO%5E-%5D_t%20%3D%20%5Cdfrac%7B1%7D%7B0.056%20M%5E%7B-1%7Ds%5E%7B-1%7D%5Ccdot%2060.0%20s%20%2B%20%5Cdfrac%7B1%7D%7B0.212%20M%7D%7D%20%3D%200.124%20M)
Answer:
The empirical formula is C3H3O
Explanation:
Step 1: Data given
Suppose the mass of the molecule = 100 grams
The molecule contains:
65.5 % Carbon = 65.5 grams
5.5 % Hydrogen = 5.5 grams
29.0% Oxygen = 29.0 grams
Molar mass of C = 12 g/mol
Molar mass of H = 1.01 g/mol
Molar mass of O = 16 g/mol
Step 2: Calculate moles
Moles = mass / molar mass
Moles C = 65.5 grams / 12 g/mol = 5.46 moles
Moles H = 5.5 / 1.01 g/mol = 5.45 moles
Moles O = 29.0 grams / 16 g/mol = 1.8125 moles
Step 3: Calculate mol ratio
We divide by the smallest amount of moles
C: 5.46 / 1.8125 = 3
H = 5.45 / 1.8125 = 3
O = 1.8125/1.8125 = 1
The empirical formula is C3H3O
PH = 0.1289<span> for </span>1.50<span> M solution of weak acid with Ka value of </span><span>.73</span>
