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Dr Jazz
Answers (6)
It seems to me you should be calculating the moles of Fe to moles of SO4 and dividing by the smaller of the two to get an empirical ratio. If it comes out 1:1 => Fe^+2; if 2-Fe:3-SO4 => Fe^+3. From the experimental data, you should be able to make these
Water gas condenses to water liquid resulting in fewer molecules of gas and thus lower pressure. Since the atmospheric pressure is unchanged, the higher atm pressure pushes in on the walls of the bottle to compensate for the reduced pressure. Combination
Use ideal gas law to calculate the moles of NO produced from the given data. Apply to given reaction and be sure to consider limiting reagent concept. LR will dictate amount (moles) of product produced. Multiply mole wt of product x moles produced => gram
For a given reduction potential table, electron flow is from the more negative E-value to the more positive E-value. This would imply metals with a more negative E-value would undergo oxidation and the more positive E-value reduction. So, considering Zn =>
Either way is appropriate, but using a procedure for such preps is more reliable. See suggested procedure and example in answer to your next question.
Preparing Buffer Solutions with a Specific pH Value 1. Calculate [A-]:[HA] ratio using Henderson-Hasselbalch Equation. pH = pKa + log10([A-]/[HA]) 2. Ca. mole fraction of each component. Xi = ni/∑n 3. Ca. Molarity of each component. Mi = (MBuffer)(Xi) 4.
