Cathode rays are a stream of electrons that are negatively charged particles. The particles move towards the anode or positively charged electrode as the posses negative charge. Electric current is the rate of flow of the charge.
Answer:
2.3*10^-19 M/s
Explanation:
Generally, reaction rate is the product of the rate constant, and the concentrations of the reactants in the system. Therefore, the rate of the reaction can be expressed as:
rate = k*![[CF_{3}CH_{2}F][OH]](https://tex.z-dn.net/?f=%5BCF_%7B3%7DCH_%7B2%7DF%5D%5BOH%5D)
The value of the rate constant k is 1.6*10^8 [1/(M*s)] at the given temperature.
![[CF_{3}CH_{2}F]](https://tex.z-dn.net/?f=%5BCF_%7B3%7DCH_%7B2%7DF%5D)
= 6.3*10^8 molecules/cm^3
![[OH]](https://tex.z-dn.net/?f=%5BOH%5D)
= 8.1*10^5 molecules/cm^3.
However, we need to convert to mol/(L(M). Therefore:
6.3*10^8 *(1000/6.023*10^23) = 1.05*10^-12
8.1*10^5 molecules/cm^3 *(1000/6.023*10^23) = 1.3*10^-15
Thus:
rate =k* = 1.6*10^8* 1.05*10^-12* 1.3*10^-15 =2.3*10^-19 M/s
Answer:
OD. 2HCl
Explanation:
A balanced equation needs the equal # of each element on BOTH sides.
By putting a 2 in front of HCl you now have 2 hydrogens on both sides and 2 chlorines. The Ca and CO3 are already balanced.
Answer:
5.37 × 10⁻⁴ mol/L
Explanation:
<em>A chemist makes 660. mL of magnesium fluoride working solution by adding distilled water to 230. mL of a 0.00154 mol/L stock solution of magnesium fluoride in water. Calculate the concentration of the chemist's working solution. Round your answer to 3 significant digits.</em>
Step 1: Given data
- Initial concentration (C₁): 0.00154 mol/L
- Initial volume (V₁): 230. mL
- Final concentration (C₂): ?
- Final volume (V₂): 660. mL
Step 2: Calculate the concentration of the final solution
We want to prepare a dilute solution from a concentrated one. We can calculate the concentration of the final solution using the dilution rule.
C₁ × V₁ = C₂ × V₂
C₂ = C₁ × V₁ / V₂
C₂ = 0.00154 mol/L × 230. mL / 660. mL = 5.37 × 10⁻⁴ mol/L
