Y2(CO3)3(aq) + HCl(aq) -->
YCl3(aq) + CO2(g) + H2O(l)
HCl(aq) + NaOH --> NaCl(aq) + H2O(l)
Consider the UNBALANCED equations above. A 0.346 g sample of impure
yttrium carbonate was reacted with 50.0 mL of 0.0965 M HCl. The
excess HCl from the first reaction required 8.84 mL of 0.104 M NaOH
to neutralize it in the second reaction. What was the mass
percentage of yttrium carbonate in the sample?
HCl reacts with Na2CO3 forming NaCl, H2O and CO2. This equation
is balanced as written. 2HCl(aq) + Na2Co3 (aq) -> 2NaCl (aq) +
H2O(l) + CO2(g).............................Part A---- what volume
of 2.25 M HCl in liters is nedded to react completely (with nothing
left over) with 0.500 L of 0.400 M Na2Co3. Use 3 sig figs and
units. Part B---- A 317 mL sample of unknown HCl solution reacts
completely with Na2CO3 to form 16.1 grams of CO2. What was the...
What salt is produced in each of the following neutralization
reactions?
HNO3(aq)+KOH(aq)→H2O(l)+?
HNO3(aq)+Ca(OH)2(aq)→H2O(l)+?
HCl(aq)+Ca(OH)2(aq)→H2O(l)+?
HCl(aq)+KOH(aq)→H2O(l)+?
Drag the appropriate items to their respective
reaction. K2NO3, KNO3, Ca(NO3)2, CaNO3, CaCl, CaCl2,
KCl2, KCl
Reaction A-
Reaction B-
Reaction C-
Reaction D –
Not a product -
Consider the given reaction. MgCO3(s) + 2 HCl(aq) — MgCl2(aq) + H2O(l) + CO2(g) Calculate the atom economy of this reaction to form carbon dioxide assuming that no other reactions are occurring. atom economy = _______ %
Given :
NaOH (aq) + HCl (aq) -> H2O (l) + NaCl (aq)
Mass of 1.00M HCl (diluted in water) : 60.925g
Vol of 1.00M HCl : 60.3mL
Mass of 1.00M NaOH : 50.500g
Vol of 1.00M NaOH : 50.0mL
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1. Find mole of product if: (show calculations)
A. HCl is the limiting reactant: ______
B. NaOH is the limiting reactant: ______
2. FInd the actual limiting reactant: ______
Part E
Write balanced complete ionic equation for
NaOH(aq)+HNO3(aq)→H2O(l)+NaNO3(aq)
Express your answer as a chemical equation. Identify all of the
phases in your answer.
Part F
Write balanced net ionic equation for
NaOH(aq)+HNO3(aq)→H2O(l)+NaNO3(aq)
Express your answer as a chemical equation. Identify all of the
phases in your answer.
Part G
Write balanced complete ionic equation for
Na3PO4(aq)+NiCl2(aq)→Ni3(PO4)2(s)+NaCl(aq)
Express your answer as a chemical equation. Identify all of the
phases in your answer.
Part H
Write balanced net ionic equation for...
Given the following balanced reaction,
O2(g) + 4 H+(aq) + 4 Fe2+(aq) →
2 H2O(l) + 4 Fe3+(aq)
What is the equilibrium constant (K)?
The following information may be useful.
O2(g) + 4 H+(aq) + 4e- → 2
H2O(l) Eº = 1.23 V
Fe3+(aq) + e- → Fe2+(aq) Eº =
0.77 V
Part B What salt is produced in each of the following
neutralization reactions? HNO3(aq)+KOH(aq)→H2O(l)+?
HNO3(aq)+Ca(OH)2(aq)→H2O(l)+? HCl(aq)+Ca(OH)2(aq)→H2O(l)+?
HCl(aq)+KOH(aq)→H2O(l)+? Drag the appropriate items to their
respective bins.
Part C Which substances are always produced in an acid-base
neutralization reaction? Check all that apply. Check all that
apply. a base water an acid a gas a salt
Cars burn gasoline as fuel according to the equation:
C8H18(l)+O2(g)=CO2(g)+H2O(g). (∆Hrxn=-5074KJ). Write a balanced
equation for the reaction. Calculate the Standard enthalpy of
formation for gasoline.
Reaction 1: NaOH(s)--> NaOH (aq)
Reaction 2: NaOH(s) + HCl (aq)--> NaCl(aq)+H2O(l)
Reaction 3: NaOH(aq) +HCl (aq) --> NaCl (aq) + H2O (L)
1) Describe each reaction as endothermic or exothermic and
explain your reasoning.
2) Examine the chemical equations for the three reactions.
Determine their relationship in a way that is consistent with
Hess's Law. (i.e. verify that Hess's Law is upheld. Reaction 3 is
the target equation).
3) Why is heat a stoichiometric quality?
4) Just what IS...