Molar mass of Cu2O,
MM = 2*MM(Cu) + 1*MM(O)
= 2*63.55 + 1*16.0
= 143.1 g/mol
mass(Cu2O)= 34.36 g
use:
number of mol of Cu2O,
n = mass of Cu2O/molar mass of Cu2O
=(34.36 g)/(1.431*10^2 g/mol)
= 0.2401 mol
Since Δ H is negative, heat is released
when 2 mol of Cu2O reacts, heat released = 292.0 KJ
So,
for 0.2401 mol of Cu2O, heat released = 0.2401*292.0/2 KJ
= 35.06 KJ
Answer: 35.1 KJ
The oxidation of copper(I)oxide, Cu,O(s), to copper(II)oxide, CuO(s), is an exothermic process. 2 Cu,0(s) + O2(g)...
The oxidation of copper(I) oxide, Cu,O(s), to copper(II)oxide, CuO(s), is an exothermic process. 2 Cu, O(s) + O2(g) 4 CuO(s) kJ AH x = -292.0 mol Calculate the energy released as heat when 61.76 g Cu, O(s) undergo oxidation at constant pressure. KJ energy released:
The oxidation of copper(I) oxide, Cu2O(s), to copper(II) oxide, CuO(s), is an exothermic process, 2Cu2O(s) + O2(g) ----> 4CuO(s) Hrxn = -292.0 kj/mol Calculate the energy released as heat when 42.42 g of Cu2O(s) undergo oxidation at constant pressure. The oxidation of copper(l) oxide, CuzO(s), to copper() oxide, CuO(s), is an exothermic process, ann,--292.0 브 mol kJ Calculate the energy released as heat when 42.42 g of Cu20(s) undergo oxidation at constant pressure Number k.J
The oxidation of copper(I) oxide, Cu2O(s), to copper(II) oxide, CuO(s), is an exothermic process. 2Cu2O(s)+O2(g)⟶4CuO(s)ΔH∘rxn=−292.0 kJmol Calculate the energy released as heat when 62.29 g Cu2O(s) undergo oxidation at constant pressure. energy released: kJ
The oxidation of copper(I) oxide, Cu, O(s), to copper(II)oxide, CuO(s), is an exothermic process. 2 Cu,C(s) + 0,(9) — 4 CuO(s) The change in enthalpy upon reaction of 50.70 g Cu, O(s) is -51.73 kJ. Calculate the work, w, and energy change, AUr, when 50.70 g Cu, O(s) is oxidized at a constant pressure of 1.00 bar and a constant temperature of 25 C. Note that A Er is sometimes used as the symbol for energy change instead of AU...
The oxidation of copper(l) oxide, Cu20(s), to copper(ll) oxide, CuO(s), is an exothermic process, kJ A292.0 rxn mol Calculate the energy released as heat when 22.34 g of Cu20(s) undergo oxidation at constant pressure Number kJ If the heat of combustion for a specific compound is -1320.0 kJlmol and its molar mass is 46.27 g/mol, how many grams of this compound must you burn to release 212.20 kJ of heat? Number
Enter your answer in the provided box. Copper(I) oxide can be oxidized to copper(II) oxide: Cu2O(s) + 1/2 O2(g) → 2 CuO(s) ΔH o rxn = −146.0 kJ Given ΔH o f of Cu2O(s) = −168.6 kJ/mol, find ΔH o f of CuO(s). kJ/mol
Copper(I) oxide can be oxidized to copper(II) oxide: Cu_2O(s) + 1/2 O_2(s) rightarrow 2 CuO(s) Delta H_rxn degree = -146.0 kJ Given Delta H degree f of Cu_2O(s) = -168.6 kJ/mol, find Delta H_f degree of CuO(s). kJ/mol
Given the following data: () Cu (s) O2 (g)CuO (s) () N2 (g) + 02 (g)NO2 (g) H'--157 kJ AHo+33 kJ calculate AH for the reaction below using Hess' Law. 4 Cu (s) 2 NO2 (g)4 CuO (s) N2 (g)
Ethylene oxide is produced by the catalytic oxidation of ethylene: C2H4 (g) + 1/2 O2 (g) --> C2H4O (g) An undesired competing reaction is the combustion of ethylene to CO2. The feed to a reactor contains 2 mol C2H4/mol O2. The conversion and yield in the reactor are respectively 25% and 0.70 mol C2H4O produced/mol C2H4 consumed. A multiple-unit process separates the reactor outlet stream components: C2H4 and O2 are recycled to the reactor, C2H4O is sold, and CO2 and...
Copper has been used for thousands of years, either as a pure metal or in alloys. It is frequently used today in the production of wires and cables. Copper can be obtained through smelting or recycling. Determine the energy associated with each of these processes in order to recycle 1.00 mol Cu. The smelting of copper occurs by the balanced chemical equation CuO(s) +CO(g)- Cu(s) +CO, (g) where ?? c o is- 155 kJ mol. Assume the process of recycling...