To begin the experiment, 1.65g of methane CH is burned in a bomb calorimeter containing 1000 grams of water. The initial temperature of water is 18.98°C. The
specific heat of water is 4.184 J/g °C. The heat capacity of the calorimeter is 615
J/ °C. After the reaction the final temperature of the water is 36.38°C.
2. Calculate the change in temperature, AT. Show your work. (1pt)

passing a magnet thought the

mixture , because iron gets attracted to magnet .

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.

mark him as !

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.