The following thermochemical equation is for the reaction of hydrogen sulfide(g) with water(l) to form hydrogen(g) and sulfur dioxide(g). H,S(g) + 2H,0(g)- →3H2(g) + SO2(g) AH=207 kJ When 7.60 grams of hydrogen sulfide(g) react with excess water(1), |kJ of energy are

The following thermochemical equation is for the reaction of sodium(s) with water(1) to form sodium hydroxide(aq) and hydrogen(g). 2Na(s) + 2H2O(1)- →2NaOH(aq) +H2(g) AH= -369 kJ When 5.86 grams of sodium(s) react with excess water(1), kJ of energy are

A chemist measures the energy change AH during the following reaction: 2 Fe,03(5) → 4 Fe(5)+O,(g) AH=560. kJ Use the information to answer the following question. Suppose 49.9 g of Fe,0, react. Calculate how much heat will be released or absorbed. ? Round your answer to 3 significant digits.

The following thermochemical equation is for the reaction of carbon dioxide(g) with hydrogen(g) to form acetylene(g) (C,H) and water(g). 2C02(g) + 5H2(g)–C,H2(g) + 4H,O(g) AH = 46.5 kJ When 15.3 grams of carbon dioxide(g) react with excess hydrogen(g), kJ of energy are | Hint: An amount of energy is expressed as a positive number. The sign of AH in the thermochemical equation indicates whether the energy is absorbed or evolved.

(Incorrect) Consider the following reaction: 2 PbS (s) + 3 02 (g) → 2 PbO (s) +2 SO₂ (g) AHxn=-827.4 kJ What mass of PbS has reacted if 765 kJ of heat is produced? You answered: 221. The correct answer is: 442.0g A

Ethyl alcohol, C2H5OH, has a specific heat of 2.40 ?? °?. Which of the following statements best describes what this means? a) It takes 1 joule of energy to increase the temperature of 1 gram of ethyl alcohol by 2.40 °C. b) It takes 1 joule of energy to increase the temperature of 2.40 grams of ethyl alcohol by 1 °C. c) It takes 2.40 joules of energy to increase the temperature of 1 gram of ethyl alcohol by 1 °C. d) It takes 2.40 joules of energy to increase the temperature of 2.40 grams of ethyl alcohol by 1 °C

In the following reaction, how many moles of CH3OH are required to give off 3791 kJ of heat? 2 CH,OH (I) + 3 02 (g) → 2 CO, (g) + 4 H,0(g) AH° = -1280. kJ

How much heat (in kilojoules) is evolved when 135 g of aluminum reacts completely in the following reaction? (the molar mass of aluminum is 27.0 g/mol) 2Al + Fe203 2Fe + Al203 AH = -80 kJ -->

A chemist measures the energy change AH during the following reaction: Cl2(9)+ H2(g) →2 HCl (g) AH=-184. kJ Use the information to answer the following question. Suppose 62.9 g of Cl₂ react. Calculate how much heat will be released or absorbed. ? g0 ☐ x10 EX OkJ olo Be sure your answer has the correct number of significant digits. Ar B >

The following thermochemical equation is for the reaction of iron(III) oxide(s) with hydrogen(g) to form iron(s) and water(g).Fe2O3(s) + 3H2(g)2Fe(s) + 3H2O(g)     H = 98.8 kJ When 44.6 grams of iron(III) oxide(s) react with excess hydrogen(g), kJ of energy are   .