Consider the two spheres shown here, one made of silver and the other of aluminum. The spheres are dropped from a height of 1.7 m. Composition - aluminum Density= 2.70 g/cm³ Volume 196 cm³ Composition silver Density 10.49 g/cm³ Volume 196 cm³ What is the kinetic energy of the silver sphere at the moment it hits the ground? (Assume that energy is conserved during the fall and that 100%% of the sphere's initial potential energy is converted to kinetic energy by the time impact occurs.) Express your answer to two significant figures and include the appropriate units. Value Units Ek =

Consider the two spheres shown here, one made of silver and the other of aluminum. The spheres are dropped from a height of 1.7 m. Composition - aluminum Density= 2.70 g/cm³ Volume 196 cm³ Composition silver Density 10.49 g/cm³ Volume 196 cm³ What is the kinetic energy of the silver sphere at the moment it hits the ground? (Assume that energy is conserved during the fall and that 100%% of the sphere's initial potential energy is converted to kinetic energy by the time impact occurs.) Express your answer to two significant figures and include the appropriate units. Value Units Ek =

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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According to the following reaction, how much energy is evolved during the reaction of 53.2 g Fe2O3 and 7.00 g of CO? 3 Fe2O3(g) + CO(g)→→ 2 Fe3O4(g) + CO2(g) ΔHo = -48.5 kJ 16.2 kJ 5.38 kJ 12.1 kJ 17.4 kJ 48.5 kJ
We can use Hess's Law (and some creativity!) to learn about the energetics of reactions that occur in remote environments. Consider the atmospheric reaction, NO + O → NO2 (a) Use the dissociation energy of O2, 498.34 kJ/mol, and the standard heats of formation for NO (+90.25 kJ/mol) and NO2 (+33.18 kJ/mol) to derive the enthalpy change for this reaction.
A student dissolves 11.1 g of sodium hydroxide (NaOH)in 200. g of water in a well-insulated open cup. He then observes the temperature of the water rise from 22.0 °C to 36.9 °C over the course of 5.3 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NaOH(s) Na (aq) + OH(aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to 3 significant digits. → Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy ΔΗ. per mole of NaOH. rxn exothermic…
potential energy diagrams for the following reactions: 2 Ag (s) + Cl2 (g) = 2 AgCl(s) +254 kj
With the information provided below, calculate the enthalpy of reduction, AredHº, for the reaction: Sr2*(aq) → Sr(s), and comment on the sign of the obtained magnitude given the properties of the alkaline-earth elements (i.e.: metallic character, reduction potentials, etc.). (hint: Hess' law should come in handy) Show your work AatH® (kJ/mol) AnyaH® (kJ/mol) IE: (kJ/mol) IE2 (kJ/mol) Element Sr 164 -1456 549.5 1064 AatHº: enthalpy of atomization; AnyaH®: enthalpy of hydration; IE1: first ionization energy; IE2: second ionization energy 2.
Measurements show that the enthalpy of a mixture of gaseous reactants decreases by 323. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that -162. kJ of work is done on the mixture during the reaction. Calculate the change in energy of the gas mixture during the reaction. Round your answer to 3 significant digits. Is the reaction exothermic or endothermic? kJ exothermic O endothermic x10 X 3
A student dissolves 11.6 g of sodium hydroxide (NaOH)in 250. g of water in a well-insulated open cup. He then observes the temperature of the water rise from 23.0 °C to 35.2 °C over the course of 8.9 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NaOH(s) Na+ (aq) + OH (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy ΔΗ per mole of NaOH.…
Consider a hypothetical ionic compound AB (comprised of A+ and B- ions). Given the following enthalpy data and using a Born-Haber cycle calculation, predict ΔHlattice in kJ mol-1. A(s) + B(s) → AB(s) ΔrH = -422 kJ mol-1 A(s) → A(g) ΔrH = 104 kJ mol-1 B(s) → B(g) ΔrH = 92 kJ mol-1 First ionization energy of A(g) = 505 kJ mol-1 Electron affinity enthalpy of B(g) (exothermic) = -316 kJ mol-1
The enthalpy for the formation of 1 mole of NH3(aq)NH3(aq) is -80.29 kJ/molkJ/mol. What is the enthapy for the formation of 3 moles of NH3(aq)NH3(aq)?
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