Answer:
Doing experiments by scientific procedures is advantageous and helpful.
Explanation:
The scientific procedure should be followed while performing a experiment as it has many advantages like:
- Working in safe environment: Performing a experiment by scientific procedure ensures the safety of the experimenter.
- It reduces the chances of mistakes: The proper availability of the scientific equipment helps in reduction of the chances of the mistakes.
- A sequence of steps is followed: A proper sequence of steps is followed to perform a experiment step by step. Performing experiment without scientific procedure may cause the experimenter to forgot a step.
- More Accuracy: The readings of the experiment is more accurate by doing experiment by scientifically.
- Chemical changes can be observed: The physical and chemical changes can be observed and can be measured by the lab equipment to perform more accurately.
- less chance of risks: Performing in the safe scientific environment and using proper safety equipment reduces the chances of risks to the experimenter.
Answer:
The paper no longer has smooth edges
The paper has not produced gas when torn
The paper has not changed colours
The paper is still paper with the same chemical makeup
<span>Consider the following reaction:
2CH3OH(g)→2CH4(g)+O2(g)ΔH=+252.8kJ
Calculate the amount of heat transferred when 27.0g of CH3OH(g) is decomposed by this reaction at constant pressure.
27.0 g </span>CH3OH(g) (1 mol/ 32.05g) = 0.84 mol CH3OH(g)
ΔH =+252.8kJ = Q = 0.84 mol (252.8kJ) = 213 kJ
Answer:
Protons, neutrons, electrons..
Explanation:
Protons and neutrons consist of quarks which are stuck together by tiny things called gluons.
Hope this helps! :)
Answer: The value of 
for the half-cell reaction is 0.222 V.
Explanation:
Equation for solubility equilibrium is as follows.
Its solubility product will be as follows.
![K_{sp} = [Ag^{+}][Cl^{-}]](https://tex.z-dn.net/?f=K_%7Bsp%7D%20%3D%20%5BAg%5E%7B%2B%7D%5D%5BCl%5E%7B-%7D%5D)
Cell reaction for this equation is as follows.
Reduction half-reaction: 
, 
Oxidation half-reaction: 
, 
= ?
Cell reaction: 
So, for this cell reaction the number of moles of electrons transferred are n = 1.
Solubility product,
= 
Therefore, according to the Nernst equation
![E_{cell} = E^{o}_{cell} - \frac{0.0592 V}{n} log \frac{[AgCl]}{[Ag^{+}][Cl^{-}]}](https://tex.z-dn.net/?f=E_%7Bcell%7D%20%3D%20E%5E%7Bo%7D_%7Bcell%7D%20-%20%5Cfrac%7B0.0592%20V%7D%7Bn%7D%20log%20%5Cfrac%7B%5BAgCl%5D%7D%7B%5BAg%5E%7B%2B%7D%5D%5BCl%5E%7B-%7D%5D%7D)
At equilibrium, 
= 0.00 V
Putting the given values into the above formula as follows.
![0.00 = E^{o}_{cell} - \frac{0.0592 V}{1} log \frac{1}{[Ag^{+}][Cl^{-}]}](https://tex.z-dn.net/?f=0.00%20%3D%20E%5E%7Bo%7D_%7Bcell%7D%20-%20%5Cfrac%7B0.0592%20V%7D%7B1%7D%20log%20%5Cfrac%7B1%7D%7B%5BAg%5E%7B%2B%7D%5D%5BCl%5E%7B-%7D%5D%7D)
= 
= 0.577 V
Hence, we will calculate the standard cell potential as follows.
= 0.222 V
Thus, we can conclude that value of for the half-cell reaction is 0.222 V.
