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
Copper reacts with nitric acid via the following equation: 3 Cu(s) + 8 HNO3(aq) → 3...
please answer Titration Homework 1. Copper reacts with dilute nitric acid according to the equation 3 Cu(s) + 8 HNO, (aq) + 3 Cu(NO3)2 (aq) + 2NO(g) + 4H20 (1) If a copper penny weighs 3.020g is dissolved in a small amount of nitric acid and the resulting solution is diluted to 50.0 mL with water, what is the molarity of the Cu(NO3)?
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)...
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?
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)
1. Balance the three copper reactions: +H20 (1) +NO2 (g) Cu(NO3)2 (aq) i) Cu (s) HNO3 (aq) NANO3 (aq) NaOH (aq) Cu(OH)2 (s) + ii) Cu(NOs)2 (aq) + H2O (1I) CuO (s) iii) Cu(OH)2 (s) 2. In reaction (i), suppose you add 4.0 mL of 6M nitric acid to a sphere of copper metal that weighs 0.65 grams. Which reactant is the limiting reagent? (Show your work)
Copper reacts with nitric acid to produce copper nitrate, nitrogen dioxide gas, and water. Cu(s) + 4 HNO (aq) Cu(NO ) (aq) + 2 NO (g) + 2 H O(l) If you have 0.60 moles of Cu and the reaction goes to completion, how many moles of HNO are needed to produce 1.2 moles of NO ?
1. Balance the three copper reactions: + H20 (1) Cu(NO3)2 (aq) + NO2(g) i) Cu (s) + HNO3 (aq) ii) Cu(NO3)2 (aq) + NaOH(aq) Cu(OH)2 (s) + NaNO3(aq) (aq) - iii) Cu(OH)2 (S) Cuo(s) + H2O (1) 2. In reaction (i), suppose you add 4.0 mL of 6 M nitric acid to a sphere of copper metal that weighs 0.65 grams. Which reactant is the limiting reagent? (Show your work)
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)
What is the product containing copper after the reaction of Cu(NO3)2(aq) + NaOH --> Cu(s) O Cu(NO3)2(aq) Cuo(s) Cu(OH)2(s) CuSO4(aq) none of these The previous problem had you calculate the mass of carbon dioxide produced when a given mass of potassium carbonate reacted with a given volume of nitric acid. In this reaction with the previously given amounts, what is the limiting reactant? K2CO3 (aq) + 2 HNO3 (aq) --> 2KNO3 (aq) + H20 (1) + CO2 (g) O CO2...
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