Which of the following processes is endothermic, given the following: S(s) + O2(g) → SO2(g) ΔH...

Which of the following processes is endothermic, given the following:

S(s) + O₂(g) → SO₂(g) ΔH = –299 kJ/mol

S(s) + 3/2 O₂(g) → SO₃(g) ΔH = –395 kJ/mol

A) 2 S(s) + 2 O₂(g) → 2 SO₂(g)

B) ½ S(s) + ½ O₂(g) →½ SO₂(g)

C) 2 S(s) + 5/2 O₂(g) → SO₂(g) + SO₃(g)

D) SO₃(g) → S(s) + 3/2 O₂(g)

Expert Solution

queen_honey_blossom answered 2 years ago

Consider the following reaction: 2Mg(s)+O2(g)→2MgO(s)ΔH=−1204kJ Part A Is this reaction exothermic or endothermic? exothermic endothermic SubmitMy...

Consider the following reaction: 2Mg(s)+O2(g)→2MgO(s)ΔH=−1204kJ Part A Is this reaction exothermic or endothermic? exothermic endothermic SubmitMy AnswersGive Up Correct Part B Calculate the amount of heat transferred when 3.56 g of Mg(s) reacts at constant pressure. ΔH = kJ SubmitMy AnswersGive Up Part C How many grams of MgO are produced during an enthalpy change of -231 kJ ? m = g SubmitMy AnswersGive Up Part D How many kilojoules of heat are absorbed when 40.7 g of MgO(s) is...

The reaction, 2 SO3(g) 2 SO2(g) + O2(g) is endothermic. Predict what will happen with following...

The reaction, 2 SO3(g) 2 SO2(g) + O2(g) is endothermic. Predict what will happen with following changes. List the shift and state the reason. a. Temperature increased: b. Pressure decreased: c. More O2 was added: d. V olume decreased: e. Catalyst was added:

4 FeS2(s) + 11 O2(g) → 2 Fe2O3(s) + 8 SO2(g) ΔH = -3307.9 kJ 2...

4 FeS2(s) + 11 O2(g) → 2 Fe2O3(s) + 8 SO2(g) ΔH = -3307.9 kJ 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g) ΔH = -1125.2 kJ 4 FeO(s) + O2(g) → 2 Fe2O3(s) ΔH = 578.2 kJ 2 Fe(s) + O2(g) → 2 FeO(s) ΔH = -544 kJ H2(g) + S(s) → H2S(g) ΔH = -20.2 kJ 2 H2(g) + O2(g) → 2 H2O(l) ΔH = 571.7 kJ By combining the above equations calculate the ΔH(formation)...

Which of the following processes are endothermic? Which of the following processes are endothermic? the reaction...

Which of the following processes are endothermic? Which of the following processes are endothermic? the reaction associated with the ionization energy of potassium. the reaction associated with the heat of formation of CaS. the formation of F2 from its elements in their standard states. the reaction associated with the lattice energy of LiCl. None of the above are endothermic.

Given the following thermochemical equations, 2Cu(s) + S(s) right-arrow Cu2S(s) ΔH°= –79.5 kJ S(s) + O2(g)...

Given the following thermochemical equations, 2Cu(s) + S(s) right-arrow Cu2S(s) ΔH°= –79.5 kJ S(s) + O2(g) right-arrow SO2(g) ΔH°= –297 kJ Cu2S(s) + 2O2(g) right-arrow 2CuO(s) + SO2(g) ΔH° = –527.5 kJ calculate the standard enthalpy of formation (in kJ mole–1) of CuO(s). Multiplied by 1/2 Finally, using the thermodynamic values given and knowing how to add all the equations together to get the desire equation, calculate the value of ΔHf° for the final formation reaction.

Given the following thermochemistry equations: C(s) + 1/2 O2(g) -------> CO (g); ΔH = -110.4 kJ/mol...

Given the following thermochemistry equations: C(s) + 1/2 O2(g) -------> CO (g); ΔH = -110.4 kJ/mol H2 (g) + 1/2 O2 (g) ------> H2O (l); ΔH = -285.5 kJ/mol CO(g) + 1/2 O2(g) -------> CO2 (g); ΔH = -283.0 kJ/mol HCOOH (l) + 1/2 O2 (g) ------> H2O (l) + CO2(g); Δ = -259.6 kJ/mol a) Calculate the ΔH for the formation of HCOOH. b) Calculate the ΔH of the reaction if 0.76 mL of HCOOH is obtained. c) If...

Part A) Calculate ΔHrxn for the reaction CaO(s)+CO2(g)→CaCO3(s) given these reactions and their ΔH values: Ca(s)+CO2(g)2Ca(s)++12O2(g)O2(g)→→CaCO3(s),2CaO(s),ΔH=−814.1...

Part A) Calculate ΔHrxn for the reaction CaO(s)+CO2(g)→CaCO3(s) given these reactions and their ΔH values: Ca(s)+CO2(g)2Ca(s)++12O2(g)O2(g)→→CaCO3(s),2CaO(s),ΔH=−814.1 kJΔH=−1269.8 kJ Express the enthalpy in kilojoules to one decimal place. Part B) Calculate Δ Hrxn for the following reaction: CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g) given these reactions and their ΔH values: C(s)C(s)H2(g)+++2H2(g)2Cl2(g)Cl2(g)→→→CH4(g),CCl4(g),2HCl(g),ΔH=−74.6 kJΔH=−95.7 kJΔH=−184.6 kJ Express the enthalpy in kilojoules to one decimal place. Part c) The thermite reaction, in which powdered aluminum reacts with copper oxide, is highly exothermic. 2Al(s)+3CuO(s)→Al2O3(s)+3Cu(s) Use standard enthalpies of formation to...

1.) Given the following data: C2H2(g) + 5/2 O2(g) à2CO2(g) + H2O(l) ΔH= -1300.kJ C(s) +...

1.) Given the following data: C2H2(g) + 5/2 O2(g) à2CO2(g) + H2O(l) ΔH= -1300.kJ C(s) + O2(g) àCO2(g) ΔH= -394kJ H2(g) + O2(g) à H2O(l) ΔH= -286kJ Use Hess’s Law to calculate ΔH for the reaction 2C(s) + H2(g) àC2H2(g) 2.) Calculate ΔH° for each of the following reactions using the data for the enthalpy of formation in the appendix. 2Na(s) + 2H2O(l)à2NaOH(aq) + H2(g

Consider the following system at equilibrium. S(s)+O2(g)<--->SO2(g) 1. How will adding more S(s) shift the equilibrium?...

Consider the following system at equilibrium. S(s)+O2(g)<--->SO2(g) 1. How will adding more S(s) shift the equilibrium? A) to the right B) to the left C) no effect 2. How will removing some SO2(g) shift the equilibrium? A) to the right B) to the left C) no effect 3. How will decreasing the volume of the container shift the equilibrium? A) to the right B) to the left C) no effect

Calculate ΔHrxn for the following reaction: CaO(s)+CO2(g)→CaCO3(s) Use the following reactions and given ΔH′s. Ca(s)+CO2(g)+12O2(g)→CaCO3(s), ΔH=...

Calculate ΔHrxn for the following reaction: CaO(s)+CO2(g)→CaCO3(s) Use the following reactions and given ΔH′s. Ca(s)+CO2(g)+12O2(g)→CaCO3(s), ΔH= -812.8 kJ 2Ca(s)+O2(g)→2CaO(s), ΔH= -1269.8 kJ Express your answer using four significant figures. Please help I keep getting all the wrong answers.

Question