Question 3:
calculate the molarity of the vinegar sample.
convert the volume of ch3cooh used (9.86 ml from last column in data table) from ml to l.
write this answer in box d.
9.86 ml x (1 l /1000 ml) = d. l of ch3cooh used = (1 pt.)
molarity of vinegar = (moles of ch3cooh) / (l of ch3cooh used)
= (box c answer) / (box d answer)
write the molarity of vinegar in box e below.
e. molarity of vinegar = (1 pt.)

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

What will most likely happen when two bromine atoms bond together?

Achemist has dissolved a certain substance in water. the chemist knows that more of the substance could be dissolved into the water before it stops dissolving. therefore