Prelab quiz - e9 - quantification of iron started: nov 3 at 2: 35pm quiz instructions prelab quizzes must be completed and submitted no later than before your scheduled lab. a completed and submitted prelab quiz is a requirement to attend lab. the prelab quizzes replace the prelab questions. due date listed only represents the last date the quiz is available to all students; ie, last day of round robin experiments. the quizzes have 10 questions, with 5 multiple choice and 5 true false. there is no time limit on the quizzes, however after you answer a question you may not go back to that question. on question 10 be sure to "submit for grading" (entering save, does not enter the grade into the gradebook). when you enter submit for grading, be sure to enter to hit submit for grading a second time as prompted. question 32 pts the concentration of hcl used for this experiment is a. 6.0 m b. 2.0 m c.1.0 m d. 12.0 m

Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3no2(g)+h2o(l)→2hno3(l)+no(g) part a suppose that 4.2 mol no2 and 0.50 mol h2o combine and react completely. which reactant is in excess? express your answer as a chemical formula. nothing

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

Estimate the molar mass of the gas that effuses at 1.6 times the effusion rate of carbon dioxide.