In a constant-pressure calorimeter, 65.0 ml of 0.330 m ba(oh)2 was added to 65.0 ml of 0.660 m hcl. the reaction caused the temperature of the solution to rise from 23.60 °c to 28.10 °c. if the solution has the same density and specific heat as water (1.00 g/ml and 4.184 j/g·°c, respectively), what is δh for this reaction (per mole of h2o produced)? assume that the total volume is the sum of the individual volumes.

At room temperature what happens to the average kinetic energy of the molecules of a solid, liquid, and a gas

If a simple machine aduces the strength of a force, what must be increased? the speed of the input force the work the simple machine performs the size of the simple machine the distance over which the force is applied

Challenge question: this question is worth 6 points. as you saw in problem 9 we can have species bound to a central metal ion. these species are called ligands. in the past we have assumed all the d orbitals in some species are degenerate; however, they often are not. sometimes the ligands bound to a central metal cation can split the d orbitals. that is, some of the d orbitals will be at a lower energy state than others. ligands that have the ability to cause this splitting are called strong field ligands, cnâ’ is an example of these. if this splitting in the d orbitals is great enough electrons will fill low lying orbitals, pairing with other electrons in a given orbital, before filling higher energy orbitals. in question 7 we had fe2+, furthermore we found that there were a certain number (non-zero) of unpaired electrons. consider now fe(cn)6 4â’: here we also have fe2+, but in this case all the electrons are paired, yielding a diamagnetic species. how can you explain this?