Write a balanced equation for the reaction of copper with nitric acxid tp produce nitric oxide (NO). Predict whether this reaction would occur with more, or less concentrated nitric acid than equation (1) : Cu(s) + HNO3(aq) ---> Cu(NO3)2(aq) + NO2(g) +H2O(l)
Write a balanced equation for the reaction of copper with nitric acxid tp produce nitric oxide...
Concentrated nitric acid reacts with solid copper to give nitrogen dioxide gas and dissolved copper ions according to the equation: Cu(s) + 4 H+(aq) + 2 NO3 - (aq) → 2 NO2(g) + Cu2+(aq) + 2 H2O(l) Suppose that 6.80 g of copper is consumed in this reaction and that the NO2 is collected at a pressure of 0.970 atm and a temperature of 45 oC. What volume of NO2 is produced?
(4) (22 pts) Gold metal dissolves in aqua regia, which is a mixture of concentrated hydrochloric and concentrated nitric acids, but gold does not dissolve in either acid separately. (You may write net ionic equations in this problem.) (a) (6 pts) Write a balanced chemical equation for the reaction of gold and nitric acid to produce Au(aq) and nitric oxide. Calculate the standard emf (in V) for this reaction. Is this reaction spontaneous under standard conditions at 25°C? (b) (6...
Consider the following unbalanced equation. Starting with 0.80 g of elemental copper and 20. mL of 15 M nitric acid (18.9 g), _____mole of water would be produced. Cu(s) + HNO3(aq) ---->Cu(NO3)2(aq) + NO2(g) + H2O(l) a. 0.030 b. 0.80 c. 0.0126 d. 0.025 e. 0.0252
(4) (22 pts) Gold metal dissolves in aqua regia, which is a mixture of concentrated hydrochloric and concentrated nitric acids, but gold does not dissolve in either acid separately. (You may write net ionic equations in this problem.) (a) (6 pts) Write a balanced chemical equation for the reaction of gold and nitric acid to produce Aut(aq) and nitric oxide. Calculate the standard emf (in V) for this reaction. Is this reaction spontaneous under standard conditions at 25°C? (b) (6...
Copper reacts with nitric acid via the following equation: 3 Cu(s) + 8 HNO3(aq) → 3 Cu(NO3)2(aq) + 2 NO(g) + 4 H2O(ℓ) What mass of NO(g) can be formed when 20.7 g of Cu reacts with 50.0 g HNO3? g NO
How will you obtain your nitric oxide for this experiment? The nitric oxide will be generated by the reaction of copper with dilute nitric acid according to this equation. 3 Cu(s) +8H(aq) + 2NO3 (aq) ---> 2NO(g) + 3 Cu²+ (aq) + 4H2O(1) The nitric oxide gas will be taken from a storage bottle provided by the TA. The nitric oxide gas will be collected from a gas cylinder. The nitric oxide gas will be prepared by the reaction of...
Write a balanced chemical equation for the reaction of aqueous solutions of potassium sulfide and nitric acid. a) K2S(aq) + 2HNO3(aq) > H2S(g) +2 KNO3(aq) b) K2S(aq) + 2HNO3(aq) > S(s) +H2(g) + 2KNO3(aq c) K2S(aq) + HNO3(aq) > HS(g) + K2NO3(aq) d) K2S(aq) + 2HNO3(aq) > 2K(s) + H2(g) + S(NO3)2(g) e) K2S(aq) + 2HNO3(aq) > 2KH(aq) + S(NO3)2(g)
q10 Choose the correct, balanced chemical equation for the following neutralization reaction: nitric acid reacts with aqueous barium hydroxide to form aqueous barium nitrate and water O HNO3 + BaOH + BaNO3 + H2O • 2 HNO3(aq) + Ba(OH)2(aq) - Ba(NO3)2(aq) + 2 H2O(1) HNO3(aq) + Ba(OH)2(aq) – Ba(NO3)2(aq) + H2O(1)
3. (14%) The metal copper is oxidized in nitric acid according to the equation: 3 Cu + 8 HNO3 → 3 Cu (NO3) 2 + 2 NO + 4 H2O a) Show how you set the oxidation-reduction reaction and get the equation here above (show as many steps in the process) b) You receive 0.3855 g of copper-containing metal together with other dissolved substances easily set up. You find that to dissolve the copper and form copper nitrate Cu (NO3)...
In this laboratory exploration various reactions of copper will illustrate these properties. First, begin with copper metal. When concentrated nitric acid is added, dramatic changes occur and the metal dissolves forming a brightly colored copper ion-containing solution. Cu(s) + 4HNO3(aq) à Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) _____________ equation Cu(s) + 4H+ + 4NO3-(aq) à Cu+2(aq) +2NO3-(aq)+ 2NO2(g) + 2H2O(l) _____________ equation Reaction type_______________ What advantage(s) is/are there to the second version of the reaction equation? However, if diluted...