Strawberries contain 20 wt% fruit solids and 80 wt% water. To make strawberry jam, strawberries are fed to a crusher and the crushed strawberries are fed to a mixer and mixed with sugar in a 40:60 crushed strawberry stream : sugar stream ratio by mass, and then the mixture is fed to an evaporator where water is evaporated until the jam product coming from it is only 1/4 water by mass. a) Draw and label a flowchart of this process.
b) Do the degree-of-freedom analysis and show that the system has zero degrees of freedom (i. e., the number of unknown process variables equals the number of equations relating them). If you have too many unknowns, think about what you might have forgotten to do.
c) Calculate how many pounds of strawberries are needed to make a pound of jam.
d) Making a pound of jam is something you could accomplish in your own kitchen (or maybe even a dorm room). However, a typical manufacturing line for jam might produce 1500lbm/h. List technical and economic factors you would have to take into account as you scaled up this process from your kitchen to a commercial operation.

Given that 1 mi = 1760 yd, determine what conver- sion factor is appropriate to convert 1849 yd to miles; to convert 2.781 mi to yards.

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 is the empirical formula of c6h18o3? ch3o c2h5o c2h6o c2h5o5