The oxidation of copper(l) oxide, Cu20(s), to copper(ll) oxide, CuO(s), is an exothermic process, kJ A292.0...

Question

Question

The oxidation of copper(l) oxide, Cu20(s), to copper(ll) oxide, CuO(s), is an exothermic process, kJ A292.0 rxn mol Calculate

Answer 1

Answer #1

1) We calculate the heat released by said amount of Cu2O, with the help of the molar weight and the heat of reaction:

q = 22.34 g * (1 mol / 143.09 g) * (292 kJ / 1 mol) = 45,552 kJ

2) We calculate the mass of the compound, with the molar weight and the heat of reaction:

mass = 212.20 kJ * (1 mol / 1320 kJ) * (46.27 g / 1 mol) = 7.438 g

If you liked the answer, please rate it in a positive way, you would help me a lot, thank you.

Answer 2

Similar Homework Help Questions

The oxidation of copper(I) oxide, Cu2O(s), to copper(II) oxide, CuO(s), is an exothermic process, 2Cu2O(s) +...

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, Cu,O(s), to copper(II)oxide, CuO(s), is an exothermic process. 2 Cu, O(s)...

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)ΔH∘rxn=−292.0 kJmol...

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,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,0(s) + O2(g) — 4 CuO(s) Hixn = -292.0 kJ mol Calculate the energy released as heat when 34.36 g Cu,O(s) undergo oxidation at constant pressure. energy released:
The oxidation of copper(I) oxide, Cu, O(s), to copper(II)oxide, CuO(s), is an exothermic process. 2 Cu,C(s)...

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...
Enter your answer in the provided box. Copper(I) oxide can be oxidized to copper(II) oxide: Cu2O(s)...

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...

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
8) If the heat of combustion for a specific compound is -1140.0 kJ/mol and its molar...

8) If the heat of combustion for a specific compound is -1140.0 kJ/mol and its molar mass is 33.43 g/mol, how many grams of this compound must you burn to release 959.10 kJ of heat?
If the heat of combustion for a specific compound is - 1200.0 kJ/mol and its molar mass is 29.71 g/mol

If the heat of combustion for a specific compound is - 1200.0 kJ/mol and its molar mass is 29.71 g/mol, how many grams of this compound must you burn to release 891.80 kJ of heat? mass: _______ g

If the heat of combustion for a specific compound is -1350.0 kJ / mol and its molar mass is 61.81 g / mol

If the heat of combustion for a specific compound is -1350.0 kJ / mol and its molar mass is 61.81 g / mol, how many grams of this compound must you burn to release 635,10 kJ of heat?