The following thermochemical equation is for the reaction of C(s,graphite) with O2(g) to form CO₂(g). C(s,graphite) + O2(g) → CO₂ (g) AH = -394 kJ How many grams of C(s,graphite) would have to react to produce 90.2 kJ of energy? grams

The following thermochemical equation is for the reaction of CO(g) with O₂ (g) to form CO₂ (g). 2CO(g) + O2 (g) → 2CO2(g) AH : = - 566 kJ How many grams of CO(g) would have to react to produce 84.1 kJ of energy? grams

A particular natural gas consists, in mole percents, of 83.0% CH4 (methane), 11.2% C₂H6 (ethane), and 5.80% C3H8 (propane). A 385-L sample of this gas, measured at 22 °C and 729 mmHg, is burned in an excess of oxygen gas. Part A How much heat, in kilojoules, is evolved in this combustion reaction?

A chemist measures the energy change AH during the following reaction: 2 Fe₂O3(s)→ 4 FeO(s) + O₂(g) Use the information to answer the following questions. This reaction is... Suppose 14.0 g of Fe₂O3 react. Will any heat be released or absorbed? If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Be sure your answer has the correct number of significant digits. ΔΗ= 560. kJ endothermic. exothermic. Yes, absorbed. Yes, released. No. KJ x10 X Ś ? 0: 000 18 Ar

Consider the reaction.   2Fe2O3⟶4Fe+3O2.    Δ?∘rxn=+824.2 kJ   The formation of 12.0 g of O2 results in the release or absorption of what amount of heat? in kJ

Diborane (B2H6(g)) is a highly reactive boron hydride, which was at one time considered as a possible rocket fuel for the US space program. Write a balanced thermochemical equation for the formation of diborane from the elements using the following information:   2 B(s) + 3/2 O2(g) ---> B2O3(s)                                  ΔH = -1273 kJ/rxn B2H6(g) + 3 O2(g) ---> B2O3(s) + 3 H2O(g)                    ΔH = -2035 kJ/rxn H2(g) + 1/2 O2(g) ---> H2O(l)                                     ΔH = -286 kJ/rxn H2O(l) ---> H2O(g)                                                    ΔH =  +44 kJ/rxn

For the reaction below ΔH = -296 kJ per mole of SO2 formed. S(s) + O2(g) → SO2(g) (b) Calculate the quantity of heat released when 0.544 mol of sulfur is burned in air. kJ

For the reaction 4 H(g) + CO(g) → CH(g) + 2 HO(g) H= -165 kJ/mol How many kJ of heat are liberated when 12.9 g of H react with 64.2 g of CO?

The following thermochemical equation is for the reaction of H₂ (g) with Cl₂ (g) to form HCl(g). H₂ (g) + Cl₂ (g) → 2HCl(g) AH = - 185 kJ How many grams of H₂ (g) would have to react to produce 68.5 kJ of energy? grams

A chemist measures the energy change AH during the following reaction: 2 HgO(s) → 2 Hg(1) + O₂(g) Use the information to answer the following questions. This reaction is... Suppose 24.4 g of HgO react. Will any heat be released or absorbed? AH= 182. kJ If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Round your answer to 3 significant digits. O endothermic. O exothermic. O Yes, absorbed. O Yes, released. O No. x10 X