Chapter 1: Q1.6CYL (page 41)
What is the density of a liquid with a mass of 31.1415 g and a volume of 30.13 cm³?
Density =1.034 (round four significant figures, Three decimal places)
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How much heat is produced when 100 mL of 0.250 M HCl (density, 1.00 g/mL) and 200 mL of 0.150 M NaOH (density, 1.00 g/mL) are mixed?
\({\bf{HCl(aq) + NaOH(aq)}} \to {\bf{NaCl(aq) + }}{{\bf{H}}_{\bf{2}}}{\bf{O(l) \Delta H}}_{{\bf{298}}}^{\bf{^\circ }}{\bf{ = - 58kJ}}\)
If both solutions are at the same temperature and the heat capacity of the products is 4.19 J/g °C, how much will the temperature increase? What assumption did you make in your calculation?
What are the allowed values for each of the four quantum numbers:n,l,ml, andms?
Identify each of the following statements as being most similar to a hypothesis, a law, or a theory. Explain your reasoning.
(a) Falling barometric pressure precedes the onset of bad weather.
(b) All life on earth has evolved from a common, primitive organism through the process of natural selection.
(c) My truck’s gas mileage has dropped significantly, probably because it’s due for a tune-up
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?
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 −92.3 kJ/mol.
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