12)
a)
From reaction,
When 1 mol of O2 reacts, ΔH = -1269.8 KJ
So, for 3 moles of O2, ΔH = -3*1269.8 KJ = -3809.4 KJ
Answer: -3809.4 KJ
b)
From reaction,
When 2 mol of Ca reacts, ΔH = -1269.8 KJ
So, for 8 moles of Ca, ΔH = -8*1269.8/4 KJ = -2539.6 KJ
Answer: -2539.6 KJ
c)
From reaction,
When 2 mol of CaO forms, ΔH = -1269.8 KJ
So, for 1 moles of CaO, ΔH = -1269.8/2 KJ = -634.9 KJ
Answer: -634.9 KJ
Only 1 question at a time please
for 12. Using the reaction enthalpy data shown, determine the amount of heat released in each...
13. Butane, C.Ho, is the fuel used in many hand-held lighters (see Figure 8.16). Based on the reaction enthalpy below, how many grams of butane are needed to produce 1,000 kJ of heat by this reaction? 2 C.H. (g) + 13 O, (o) → 8 CO2(g) + 10 HOU AH = -5,755 kJ
Calculate the standard enthalpy of formation of solid calcium carbonate (CaCO3) using the following thermochemical information: Calculate the standard enthalpy of formation of solid calcium carbonate (CaCo3) using the following thermochemical information: 2 Cao(s) 2 Ca(s) O2(g) AH 1270.2 kJ C(s) O2 (g) CO2 (g) AH 393.5 kJ AH 178.3 kJ CaO(s) CO2 (g) CaCO3(s) kJ AH
Calculate the enthalpy of the reaction 2NO(g) + O2(g)2NO2(g) Hess's law states that "the heat released or absorbed in a chemical process is the same whether the process takes place in one or in several steps." It is important to recall the following rules: given the following reactions and enthalpies of formation: 1. ¢ N2(g) + O2(g)+NO2(g), AH; = 33.2 kJ 2. N2(g) + O2(g) NO(g), AHB = 90.2 kJ 1. When two reactions are added, their enthalpy values are...
Given the following heat of formation values, calculate the heat of reaction for the following: C3H8(g) + O2(g) CO2(g) + H2O(1). AfH values in kJ/mol: C3H8(g): -103.8, O2(g): 0, CO2(g): -393.5, H2O(l): -285.8. 3.613 x 102 kJ/mol -2.220 103 kJ/mol 1.413* 102 kJ/mol -5.755 x 102 kJ/mol If a lighter contains 4.0 mL of liquid butane (density of butane = 0.8 g/cm3), how much heat can we get out of it, from the combustion of butane? 2 C4H 10(g) +...
7. Enthalpy of chemical changes: a.For each of the following reaction, the ∆H is the enthalpy change when the number of moles indicated by the stoichiometric coefficients react. Calculate the ∆H when 1.00 g of the italicized substance is consumed or produced: 4Na (s) + O2(g)---------2Na2O (s) ∆H = -828 KJ CaMg(CO3)2(s)---------------CaO (s) +MgO (s) +CO2(g) ∆H = +302 KJ H2(g) + 2CO (g)--------------H2O2(l) + 2C (s) ∆H = +33.3 KJ
Use the information below to determine the enthalpy change that occurs when 15.2 g of Ca(s) reacts with excess oxygen. 2 Ca(s) + O2(g) 2 CaO(s) AH = -1270kJ O-481.6 kJ 481.6 kJ 240.8 kJ 0-240.8 kJ
Using the equations Ca (s)2 O (g) Сао (s) 2 H2 (g) Determine the enthalpy for the reaction Са (s) + 2 H0 () — Са(ОН)2 (s) + H2 (9). CaO (s) AH° = -635 kJ/mol -64 kJ/mol H2O ()Ca(OH)2 (s) AH O2 (g)2 H2O (I) AH° = -572 kJ/mol kJ/mol 1 2 3 4 6 C 5 7 8 9 +/- 0 x 100 LO 11.01 g of MgSO4 is placed into 100.0 mL of water. The water's temperature...
Using Hess's Law, determine the enthalpy change of the following reaction. CS2(1) + 3 O2(g) --> CO2(g) + 2 SO2(g) C(s) + O2(g) --> CO2(g) AH = -393.5 kJ/mol S(s) + O2(g) --> SO2(g) AH = -296.8 kJ/mol C(s) + 25(s) --> CS2(8) AH = +87.9 kJ/mol -899.2 kJ O-778.2 kJ -602.4 kJ - 1075.0 kJ
Calcium carbide (CaC) is manufactured by the reaction of CaO with carbon at a high temperature (calcium carbide is then used to make acetylene): CaO (s)+3C (s) + CaC2 (s)+CO (g) AH =+464.8 kJ mol- Is this reaction endothermic or exothermic? If 10.0 g of CaO is allowed to react with an excess of carbon, how much heat is absorbed or evolved by the reaction?
Question 4 of 4 > The enthalpy changes, AH, for three reactions are given. H, ()0,()H,O) Ca(s) +2H (aq) Ca2 (aq) +H,(g) CaO(s) +2H (aq) - AH=-286 kJ/mol AH= -544 kJ/mol Ca2 (aq) +H,O() AH =-193 kJ/mol Using Hess's law, calculate the heat of formation for CaO(s) using the reaction shown. 0,()Ca) Ca(s) + kJ/mol ΔΗ- TOOLS During an experiment, a student adds 1.81 g CaO to 300.0 mL of 1.000 M HCI. The student observès a temperature increase of...