Answer:
The correct approach is Option B (Peer Review).
Explanation:
- Rather made reference to someone as a scientific peer-review, it encourages the specialist who has not been essential to the study team to analyze the study objectively and pointed out everyone's mistakes. It serves as major self-regulation for scholars and aims to make the publishing process somewhat credible. Hence, the solution to this issue is Peer Examination.
- Funding organizations rarely have the capabilities to recognize out mistakes, whereas definitive analysis is a method of study that helps to make a definitive statement. The gathering of data is simply a process of scientific study.
Other approaches do not apply to the example mentioned. Although the one mentioned is right.
The answer is No you’re not.
Answer is: no, every sample does not have a negative charge.
Beside negatively charged electrons, atoms have positively charged protons, so atoms have neutral charge.
Atomic number is the number of protons, which is characteristic of a chemical element. For example, iron (Fe) is an element with atomic number 26, which means it has 26 protons and 26 electrons (in neutral atom, number of protons is equal to number of electrons).
The electron (symbol: e⁻) is a subatomic particle whose electric charge is negative one elementary charge.
Proton is a subatomic particle with a positive electric charge of +1e elementary charge.
Answer:
50.00 g of NO
Explanation:
Remember that the balanced chemical reaction equation is indispensable in solving any question that has to do with stoichiometry. Hence the first step in solving the problem is noting down the balanced chemical reaction equation.
2NO(g) + O2 (g)→ 2NO2(g)
Now we try to find out the reactant in excess. The reactant in excess gives the greater mass of product.
For O2;
From the balanced reaction equation;
32 g of O2 yields 92g of NO2
16.00g of O2 will yield 16.00×92/32 = 46g of NO2
For NO;
30g of NO yields 92g of NO2
80.00 g of NO yields 80.00 × 92/30 = 245.33 g of NO2
Hence NO is the reactant in excess.
If 1 mole of O2 reacts with 2 moles of NO2 according to the balanced reaction equation
Then 32 g of O2 reacts with 60g of NO according to the balanced reaction equation
16.00 g of O2 reacts with 16.00 × 60 /32 = 30 g of NO
Hence mass of excess reactant used in the reaction = total mass of NO- mass of NO reacted= 80.00g -30.00g = 50.00 g of NO
Hence the mass of excess reactant used in the reaction is 50.00 g of NO