Answer:
B: increase.
Explanation:
When we are considering two gases A and B in a container at room temperature .
We have to find the change on rate of reaction when the number of molecules of gases A is doubled
Let [A]=a and [B]=b
A+B
product
Rate of reaction
![R_1=k[A][B]=kab](https://tex.z-dn.net/?f=R_1%3Dk%5BA%5D%5BB%5D%3Dkab)
We know that concentration is increases with increase in number of moles
When the number of molecules of gases A is doubled then concentration of gases A increases.
Therefore ,[A]=2a
Rate of reaction
![R_2=k(2a)(b)=2kab](https://tex.z-dn.net/?f=R_2%3Dk%282a%29%28b%29%3D2kab)
![R_2=2R_1](https://tex.z-dn.net/?f=R_2%3D2R_1)
Hence, the rate of reaction is 2 times the initial rate of reaction.Therefore, the rate of reaction will increase when the number of molecules of gases A is doubled.
Answer: B: increase.
Answer:
The plum pudding model would have to be true as well because it shows that electrons are scattered within an atom.
Explanation:
I took the test and got it right :)
Answer : The pressure in torr and in atmospheres are, 745 torr and 0.980 atm respectively.
Explanation :
As we are given that the atmospheric pressure is, 745 mmHg.
Now we have to determine the pressure in torr and atm.
Conversions used:
1 atm = 760 mmHg
1 atm = 760 torr
1 mmHg = 1 torr
As, 760 mmHg = 1 atm
So, 745 mmHg = ![\frac{745mmHg}{760mmHg}\times 1atm=0.980atm](https://tex.z-dn.net/?f=%5Cfrac%7B745mmHg%7D%7B760mmHg%7D%5Ctimes%201atm%3D0.980atm)
and,
As, 1 mmHg = 1 torr
So, 745 mmHg = 745 torr
Therefore, the pressure in torr and in atmospheres are, 745 torr and 0.980 atm respectively.
Rate of Sulfur dioxide : 2730.44 mL/s
<h3>Further explanation </h3>
Graham's law: <em>the rate of effusion of a gas is inversely proportional to the square root of its molar masses or </em>
the effusion rates of two gases = the square root of the inverse of their molar masses:
![\rm \dfrac{r_1}{r_2}=\sqrt{\dfrac{M_2}{M_1} }](https://tex.z-dn.net/?f=%5Crm%20%5Cdfrac%7Br_1%7D%7Br_2%7D%3D%5Csqrt%7B%5Cdfrac%7BM_2%7D%7BM_1%7D%20%7D)
or
![\rm M_1\times r_1^2=M_2\times r_2^2](https://tex.z-dn.net/?f=%5Crm%20M_1%5Ctimes%20r_1%5E2%3DM_2%5Ctimes%20r_2%5E2)
MW of N₂ = 28 g/mol
MW SO₂ = 64 g/mol
![\tt 28\times 79^2=64\times r_2^2\\\\r_2^2=\dfrac{28\times 79^2}{64}=2730.44~mL/s](https://tex.z-dn.net/?f=%5Ctt%2028%5Ctimes%2079%5E2%3D64%5Ctimes%20r_2%5E2%5C%5C%5C%5Cr_2%5E2%3D%5Cdfrac%7B28%5Ctimes%2079%5E2%7D%7B64%7D%3D2730.44~mL%2Fs)