M7L1M1 - Stoichiometry Conversions 1. If 35.2 g of hydrochloric acid react with excess of magnesium, how many grams of hydrogen are produced?Mg(s) + 2 HCl(aq) MgCl2(aq) + H2(aq)2. How many grams of sodium bromide must be reacted with excess flourine if 25.4 g of bromine gas is produced?2 NaBr(aq) + F2(g) 2 NaF(aq) + Br2(l)3. How many grams of gold is produced by 10.4 g of gold (III) nitrate, which is dissolved in water?3 Cu(s) + 2 Au(NO3)3(aq) 3 Cu(NO3)2(aq) + 2 Au(s)4. If excess nitric acid acid reacts with how many grams of lithium bromide, to produce 72 grams of lithium nitrate?HNO3 (aq) + LiBr(aq) LiNO3(aq) + HBr(aq)5. How many moles of sulfur is needed to react with 56.4 grams of aluminum? 16 Al(s) + 3 S8(s) 8 Al2S3(s) NCVPS Honors ChemistryModule 7, Lesson 1 Mastery AssignmentStoichiometry ConversionsHomeworkPage 2 of 2

City a and city b had two different temperatures on a particular day. on that day, four times the temperature of city a was 8â° c more than 3 times the temperature of city b. the temperature of city a minus twice the temperature of city b was â’3â° c. what was the temperature of city a and city b on that day? city a was 5â° c, and city b was 4â° c. city a was 3â° c, and city b was â’1â° c. city a was 8â° c, and city b was â’3â° c. city a was 5â° c, and city b was â’5â° c.

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

How can carbon move from "land" to bodies of water? describe the way human impact has lead to increased levels of co2 in the atmosphere.