Use the data given below to construct a born-haber cycle to determine the heat of formation of kcl. δ h°(kj) k(s) → k(g) 89 k(g) → k (g) e- 418 cl2(g) → 2 cl(g) 244 cl(g) e- → cl-(g) -349 kcl(s) → k (g) cl-(g) 717 use the data given below to construct a born-haber cycle to determine the heat of formation of kcl. h°(kj) k(s) → k(g) 89 k(g) → k (g) e- 418 cl2(g) → 2 cl(g) 244 cl(g) e- → cl-(g) -349 kcl(s) → k (g) cl-(g) 717 -437 kj 631 kj -1119 kj 158 kj -997 kj

Which type of reaction always has an element and a compound as reactants

An experimental procedure requires a 10 ml of acid to be dissolved

Since the gas in your graduated cylinder is a mixture of butane and water vapor, you must determine the partial pressure of the butane, pbutane, alone. to do this, consult a reference and record the partial pressure of the water vapor, pwater, at the temperature you recorded. use the following formula to compute the partial pressure of the butane. pbutane = atmosphere - pwater use the following combined gas law formula and compute the volume that the butane sample will occupy at stp. (hint: convert both temperatures to kelvin.) pbutane x voriginal = pstandard x vfinal troom tstandard use the following ratio and proportion formula to determine the mass of butane needed to occupy a volume of 22.4 l at stp. grams of butane you used “x” grams of butane ml of butane corrected to stp = 22,400 ml compute the theoretical molar mass of butane based on its formula and the atomic masses on the periodic table. compare your experimental results from #3 to the theoretical value of #4, computing a percent error of your findings using this formula: % error = measured value - accepted value x 100 accepted value use the following ratio and proportion formula to determine the mass of butane needed to occupy a volume of 22.4 l at stp. need asap