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Chapter 1: Q83E. (page 9)
Of the five elements Sn, Si, Sb, O, Te, which has the most endothermic reaction? (E represents an atom.) What
name is given to the energy for the reaction?
\({\bf{E}}(g) \to {{\bf{E}}^ + }(g){\rm{ }} + {\rm{ }}{{\bf{e}}^ - }\)
Oxygen will require the most energy for the reaction.
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A large piece of jewelry has a mass of 132.6g. A graduated cylinder initially contains 48.6 mL water. When the jewellery is submerged in the graduated cylinder, the total volume increases to 61.2 mL.
a) Determine the density of this piece of jewelry.
b) Assuming that the jewellery is made from only one substance, what substance is it likely to be? Explain.
Hydrogen gas, H2, reacts explosively with gaseous chlorine, \({\bf{C}}{{\bf{l}}_{\bf{2}}}\), to form hydrogen chloride, HCl(g). What is the enthalpy change for the reaction of 1 mole of \({{\bf{H}}_{\bf{2}}}\)(g) with 1 mole of \({\bf{C}}{{\bf{l}}_{\bf{2}}}\)(g) if both the reactants and products are at standard state conditions? The standard enthalpy of formation of HCl(g) is 鈭�92.3 kJ/mol.
Visit this PhET density simulation (http://openstaxcollege.org/l/16phetmasvolden) and select Mystery Blocks.(a) Pick one of the Mystery Blocks and determine its mass, volume, density, and its likely identity.(b) Pick a different Mystery Block and determine its mass, volume, density, and its likely identity.(c) Order the Mystery Blocks from least dense to most dense. Explain.
In glycolysis, the reaction of glucose (Glu) to form glucose-6-phosphate (G6P) requires ATP to be present as described by the following equation:
Glu + ATP 鈫� G6P + ADP
螖骋掳298 = -17kJ
In this process, ATP becomes ADP summarized by the following equation:
ATP 鈫� ADP 螖骋掳298 = -30kJ
Determine the standard free energy change for the following reaction, and explain why ATP is necessary to drive this process:
Glu 鈫� G6P螖骋掳298 = ?
Both graphite and diamond burn.
\({\bf{C}}\left( {{\bf{s, diamond}}} \right){\bf{ + }}{{\bf{O}}_{\bf{2}}}\left( {\bf{g}} \right) \to {\bf{C}}{{\bf{O}}_{\bf{2}}}\left( {\bf{g}} \right)\)
For the conversion of graphite to diamond:
\({\bf{C}}\left( {{\bf{s, graphite}}} \right) \to {\bf{C}}\left( {{\bf{s, diamond}}} \right){\bf{ \Delta {\rm H}}}_{{\bf{298}}}^{\bf{^\circ }}{\bf{ = 1}}{\bf{.90 kJ}}\)
Which produces more heat, the combustion of graphite or the combustion of a diamond?
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