The chemical reaction would most likely be written as follows:
A + B = AB
We cannot simply use the usual method of converting grams to moles since we do not have any idea on what are the identities of A and B. The only method we could use is to use the law of conservation of mass where mass inflow in a process should be equal to the mass out in the process. The total inflow of mass would be the mass of A and B and the outflow would be the product AB.
mass of A + mass of B = mass of AB
10.0 g A + 10.0 g B = mass of AB
mass of AB = 20.0 g
Answer:
8.0 mol O₂
Explanation:
Let's consider the complete combustion reaction of C₉H₁₂.
C₉H₁₂ + 12 O₂ → 9 CO₂ + 6 H₂O
The molar ratio of C₉H₁₂ to O₂ is 1:12. The moles of O₂ required to react with 0.67 moles of C₉H₁₂ are:
0.67 mol C₉H₁₂ × (12 mol O₂/1 mol C₉H₁₂) = 8.0 mol O₂
8.0 moles of O₂ are required to completely react with 0.67 moles of C₉H₁₂.
Answer:
C) at equilibrium, the concentration of C will be much greater than the concentration of A or B.
Explanation:
A + B ⇌ C; ΔG° = -20 kJ·mol⁻¹
If ΔG is negative, the reaction is spontaneous and position of equilibrium lies to the right, so the equilibrium concentration of C is much greater than that of A or B.
A) is wrong. The molar ratio of A:B is 1:1. If their initial concentrations are 1 mol·L⁻¹, their final concentrations will be equal.
B) is wrong. The position of equilibrium lies to the right, so the concentration of C will be much greater than that of A.
D) and E) are wrong. ΔG says nothing about the rate of a reaction. It deals with the spontaneity and position of equilibrium not the speed at which equilibrium is achieved.
Element C will have 5 protons
Answer:
5.99
Explanation:
-log(10.25x10^-7)
- Hope this helps! Please let me know if you need further explanation.
