What volume (in mL) of a 0.125 M HNO3 solution is required to
completely react with 39.8 mL of a 0.102 M Na2CO3 solution
according to the following balanced chemical equation?
Na2CO3(aq)+2HNO3(aq)→2NaNO3(aq)+CO2(g)+H2O(l)
Express your answer with the appropriate units.
Homework Text bOOK
Here is the reaction
Cu (s) + 4 HNO3 (aq) >>> Cu(NO3)2 (aq) + 2
NO2 (g) + 2 H2O (l) You are given 1.00 g of copper, how much
concentrated nitric acid (in mL) do you need for this reaction?
Concentrated nitric acid is 15.0 M HNO3. Which is the
correct answer:
4.19
6.29
1.05
8.38
You are given 1.00 g of copper and 5.00 mL of concentrated
nitric acid, how much concentrated nitric acid (in mole)...
Cu(s)+HNo3(aq)- Cu(NO3)2(aq)+NO2(g)+H2O 1. which chemical
species is the limiting reaggent? 2.which chemical spcies is the
non-limiting reagent? 3.Theoretical Volume amount of nitric acid
needed used. 4Experimental Volume amount of nitc acid used.
5.Experimental Volume amount of nitric acid remaining.
When NO2NO2 is bubbled into water, it is completely converted to
HNO3HNO3 and HNO2HNO2:
2NO2(g)+H2O(l)→HNO3(aq)+HNO2(aq)
Part A
Calculate the pHpH in a solution prepared by dissolving 0.0360
molmol of NO2NO2 in 1.45 LL of water. KaKa for HNO2HNO2 is
4.5×10−44.5×10−4.
Express your answer using two decimal places.
Part B
Calculate the concentrations of all species present (H3O+H3O+,
OH−OH−, HNO2HNO2, NO−2NO2− and NO−3NO3−) in a solution prepared by
dissolving 0.0360 molmol of NO2NO2 in 1.45 LL of water.
Enter your answers...
Balance the following chemical equation:
Cu(s)+HNO3(aq)=Cu(NO3)2+NO(g)+H2O(l).
I missed this question on a quiz after trying to balance it both
algebraically and by standard guess and check methods. Several
classmates missed it as well. The answer is all over the internet,
but what I need is a step by step explanation on how this would be
balanced. Thank you!
If 3.35 g Cu(NO3)2 are obtained from allowing 1.46g of Cu to
react with excess HNO3--
How many grams of copper nitrate are formed from 1.46 g
copper?
What is the percent yield of copper nitrate for this
reaction?
1. Calculate the ΔG°rxn using the following
information.
2 HNO3(aq) + NO(g) → 3 NO2(g) +
H2O(l) ΔG°rxn = ?
ΔG°f (kJ/mol) -110.9 87.6 51.3 -237.1
2.Determine the equilibrium constant for the following reaction
at 549 K.
CH2O(g) + 2 H2(g) → CH4(g) +
H2O(g) ΔH° = -94.9 kJ; ΔS°= -224.2 J/K
3.Calculate ΔGrxn at 298 K under the conditions shown
below for the following reaction.
CaCO3(s) → CaO(s) + CO2(g) ΔG° = +131.1
kJ
P(CO2) = 0.033 atm
What volume of 0.075 M Ba(OH)2(aq) is required to completely
neutralize 22.1 mL of 1.48 M HNO3(aq)?
A) 1.7 x 10–3 L B) 0.87 L C) 1.2 x 10–3 L D) 0.22 L E) 4.9 x
10–3 L