Answer:
Explanation:
Given
Required
Calculate the number of moles
We'll apply the following formula to solve this question
Where
The above equation is an illustration of the ideal gas law
Substitute values for p, V, R and T in:
<em>Hence, there are 243.605 moles</em>
The atomic number, the number of protons and the number of electrons.
Answer:
A- Speed = distance/time
Explanation:
Would make sense and that's what I remember
Answer : The pH of buffer is 9.06.
Explanation : Given,
Concentration of HBrO = 0.34 M
Concentration of KBrO = 0.89 M
Now we have to calculate the pH of buffer.
Using Henderson Hesselbach equation :
![pH=pK_a+\log \frac{[Salt]}{[Acid]}](https://tex.z-dn.net/?f=pH%3DpK_a%2B%5Clog%20%5Cfrac%7B%5BSalt%5D%7D%7B%5BAcid%5D%7D)
![pH=pK_a+\log \frac{[KBrO]}{[HBrO]}](https://tex.z-dn.net/?f=pH%3DpK_a%2B%5Clog%20%5Cfrac%7B%5BKBrO%5D%7D%7B%5BHBrO%5D%7D)
Now put all the given values in this expression, we get:
Therefore, the pH of buffer is 9.06.
Answer:
1. Hydrogen will diffuse faster.
2. The ratio of diffusion of hydrogen gas to that of the unknown gas is 4 : 1
Explanation:
Let the rate of diffusion of hydrogen gas, H2 be R1
Let the molar mass of H2 be M1
Let the rate of diffusion of the unknown gas be R2.
Let the molar mass of the unknown gas be M2.
Molar mass of H2 (M1) = 2x1 =2g/mol
Molar mass of unknown gas (M2) = 16 times that of H2
= 16 x 2 = 32g/mol
1. Determination of the gas that will diffuse faster. This is illustrated below:
R1/R2 = √(M2/M1)
R1/R2 = √(32/2)
R1/R2 = √16
R1/R2 = 4
Cross multiply
R1 = 4R2
From the above calculations, we can see that the rate of diffusion H2 (R1) is four times the rate of diffusion of the unknown gas (R2).
Therefore, hydrogen will diffuse faster.
2. Again, from the calculations made above, the ratio of diffusion of hydrogen (R1) to that of the unknown gas (R2) is given by;
R1/R2 = 4
Therefore, the ratio of diffusion of hydrogen (R1) to that of the unknown gas (R2) is:
4 : 1
