1.- Sodium bicarbonate or sodium hydrogen carbonate, NaHCO3, releases carbon dioxide gas when heated at 180 °C, which is responsible for the rising of cookies, donuts, cakes, and bread. a) Write a balanced equation for the decomposition of the compound (one of the products is Na2CO3).
b) Calculate the mass of CO2 produced if 15.5g of NaHCO3 are heated at 185°C during the baking process of chocolate cake.
c) How many grams of NaHCO3 are necessary to produce 23g of CO2 if the % yield of this reaction is 84%?
2 =44.01 3 =72.01

2.- Ammonium nitrate is a White crystalline solid, highly soluble in water and is used in agriculture as a fertilizer. The industrial process of ammonium nitrate entails the acid-base reaction of ammonia with hydroxide and nitric acid:
NH4OH (ac) + HNO3 (ac) NH4NO3 (ac) + H2O (l)

a) Calculate the mass of NH4NO3 produced by the reaction 50 g de NH4OH 90% of purity with 85 g of HNO3 and the % yield is del 83%.
b) What is the limiting reactant?
c) How many grams of the excess reactant remains at the end of the reaction?
4 = 35.05 43 = 80.04 3 = 63.01

Water molecules have a strong attraction to each other because of hydrogen bonding, allowing water to move against gravity up a plant's stem through capillary action. true false

What method(s) do plants use to obtain nitrogen? select all that apply. absorb it from the atmosphere use bacteria to convert nitrogen to usable form obtain usable nitrogen compounds from the soil absorb nitrogen from water taken in at the roots

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