Write a balanced reaction for each reaction.
0.4M NaI + 0.1M KMnO4 + 3M H2SO4
0.4M NaI + 0.1M FeCl3 + 3M H2SO4
0.4M NaI + 0.1M KMnO4 + 6M NaOH
1) The general equation for the reaction is :
4KMnO4 + 10NaI + 16H2SO4 <---> 5I2 + 4MnSO4 + 10NaSO4 + 2K2SO4 + 16H2O
In the given question, we have 0.4 moles NaI, 0.1 moles KMnO4 and 3 moles H2SO4.
Here KMnO4 is the limiting reagent, hence the equation becomes
0.4 NaI + 0.1 KMnO4 + 3 H2SO4 <---> 0.125 I2 + 0.1 MnSO4 + 0.25 NaSO4 + 0.05 K2SO4 + 0.4 H2O
2) The general reaction is:
2NaI + 2 FeCl3 + 3 H2SO4 <----> I2 + 2 FeSO4 + Na2SO4 + 6 HCl
According to given equation, the limiting reagent is FeCl3
So the solution is:
0.4 NaI + 0.1 FeCl3 + 3 H2SO4 <----> 0.05 I2 + 0.1 FeSO4 + 0.05 Na2SO4 + 0.3 HCl
3) The general reaction is:
20 NaI + 80 KMnO4 + 60 NaOH <---> 20 IO3 + 3 H20 + 40 K2MnO4 + 40 Na2MnO4
According to given question, the limiting reagent is NaOH
So the solution is:
0.4 NaI + 0.1 KMnO4 + 6 NaOH <---> 0.033 IO3 + 0.005 H20 + 0.0667 K2MnO4 + 0.0667 Na2MnO4
To find the limiting regent, we take one stoichiometric coefficient of one reactant and find the coefficients of others using the stoichiometry and find out which of the reactants are provided in lower quantity. It is the limiting reagent. If none of the other reactants is present in lower quantity, this means that the selected compound is the limiting reagent.
Write a balanced reaction for each reaction. 0.4M NaI + 0.1M KMnO4 + 3M H2SO4 0.4M NaI + 0.1M FeCl3 + 3M H2SO4 0.4M NaI...
KMnO4 + KI + H2SO4 -> MnSO4 + K2SO4 + I2 + H2O balanced: 2KMnO4 + 10KI + 8H2SO4 -> 2MnSO4 + 6K2SO4 + 5I2 + 8H2O give the overall balanced equation (I have it) but show using the half reaction method for each reaction
1) Write the balanced chemical equation for the neutralization reaction of H2SO4 and NaOH 2) why is it necessary to write the balanced chemical equation for the neutralization reaction before calculating the molarity of the unknown solution? 3) How many milliliters of 0.20 M Mg(OH)2 solution are needed to completely neutralize 35.0 mL of 0.15 ?M H3PO4
Write the balanced equation for the reaction of aqueous Pb(ClO3)2 with aqueous NaI. Include phases. chemical equation: What mass of precipitate will form if 1.50 L of highly concentrated Pb(ClO3)2 is mixed with 0.300 L 0.260 M NaI ? Assume the reaction goes to completion. mass of precipitate:
Write the balanced equation for the reaction of aqueous Pb(ClO3)2 with aqueous NaI. Include phases. chemical equation: What mass of precipitate will form if 1.50 L of highly concentrated Pb(ClO3)2 is mixed with 0.600 L 0.270 M NaI ? Assume the reaction goes to completion. mass of precipitate: g
A 0.205 M NaOH solution is used to titrate 20.0 mL of solution of H2SO4. Write a balanced equation for this acid base reaction If 45.6 mL of the NaOH solution is required to reach the endpoint, what is the molarity of the H2SO4solution. What is the PH of the solution if the hydroxide concentration [OH-] is 4.3 x 10-6M.
Write balanced equations and draw the structure for any reactions undergone by each alkyl halide with NaI/Acetone: 2-bromobutane, 2-bromo-2-methylpropane, 1-bromobutane, bromocyclohexane, 1-bromoadamantane and write out mechanism for the reaction 2-bromobutane in NaO/Acetone
Write out in full detail the balanced equation for: NaOH (aq) + KMnO4 (aq) + H2O2 (aq) =
Write balanced net ionic equation for the following reaction: Fe(OH)3(s)+H2SO4(aq)→? Express your answer as a chemical equation. Identify all of the phases in your answer. Write balanced net ionic equation for the following reaction: HClO3(aq)+NaOH(aq)→? Note that HClO3 is a strong acid. Express your answer as a chemical equation. Identify all of the phases in your answer.
Write the balanced neutralization reaction that occurs between H2SO4 and KOH in aqueous solution. Phases are optional. neutralization reaction: Suppose 0.750 L of 0.400 M H2SO4 is mixed with 0.700 L of 0.280 M KOH. What concentration of sulfuric acid remains after neutralization?
Determine the product if the following reaction. After, balance it: a) H2O2 + H2SO4 + KMnO4 = b) What would the reaction look like as a redox reaction? Write it out as a separate reduction and oxidation reaction.