In the following reaction the iodide ion (i-) in hi is oxidized by the permanganate ion ( a 5.0 ml solution of 0.20m hi requires 4.0 ml of kmno4 to completely oxidize all the iodide. what is the molarity of the kmno4 solution?
10 hi + 2 kmno4 + 3 h2so4 → 5 i2 + 2 mnso4 + 8 h2o
1)0.05 m
2)0.16 m
3)0.25 m
4)0.8 m

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