Explanation:
from the equation 1 mole of O2 will give 2 moles of H2O then 6.0 moles of O2 will give x
6.0*2 moles/ 1 mole
= 12 moles
this implies that, 6.0 moles of O2 will give = 12 moles of water
Actually Rb or Rubidium in zero state has the following
electron configuration:
<span>1s22s2</span><span>2p6</span><span>3s2</span><span>3p63d10</span><span>4s2</span><span>4p65s1</span>
However we can see that the ion has a 1 positive charge,
which means that it lacks 1 electron, therefore the answer from the choices is:
<span>d.
rb+: 1s22s22p63s23p64s23d104p6</span>
Explanation:
Rate law is defined as the rate of a reaction is directly proportional to the concentration of reactants at constant temperature.
![Rate \propto [\text{concentration of reactant}]^{n}](https://tex.z-dn.net/?f=Rate%20%5Cpropto%20%5B%5Ctext%7Bconcentration%20of%20reactant%7D%5D%5E%7Bn%7D)
= k ![[\text{concentration of reactant}]^{n}](https://tex.z-dn.net/?f=%5B%5Ctext%7Bconcentration%20of%20reactant%7D%5D%5E%7Bn%7D)
where, k = rate constant
n = order of reaction
For the given reaction, 
Hence, its rate will be as follows.
Rate = ![k[H_{2}][NO]](https://tex.z-dn.net/?f=k%5BH_%7B2%7D%5D%5BNO%5D)
Also, it is known that slowest step in a chemical reaction is the rate determining step.
Hence, for the given rate law correct reaction is as follows.
Step 1 :
(slow)
Balancing this equation it becomes
(slow)
Step 2:
(fast)