Part B Refer to the observations of the test tubes from part A. Determine which metal (or hydrogen) in each test tube is more
reactive. Remember that the less reactive metal (or hydrogen) will typically end up in pure form as an element, so no
reaction will occur if the less reactive metal (or hydrogen) is the one that begins in pure form.
B IV x'x, Font Sizes A. A
More Reactive Element
Test Tube
1
2
3
Elements to compare
Iron and copper
copper and hydrogen
zinc and iron
zinc and magnesium
zinc and hydrogen
Iron and hydrogen
4
5
6
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Balance this equation: n2 + h2 > nh3, write the following molar ratios: n2 / n2 / nh3 h2 /

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

The diagram below shows the different phase transitions that occur in matter. which arrow represents the transition in which dew is formed?