Chemistry, 04.05.2021 18:50 brandiwingard
A gas originally at 27 °c and 1.00 atm pressure in a 3.9 l flask is cooled at constant pressure until the temperature is 11 °c. the new volume of the gas is
Answers: 2
Chemistry, 22.06.2019 08:30
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
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Chemistry, 22.06.2019 21:20
The organs inside the body and how they function together
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Chemistry, 23.06.2019 10:30
How much mass would a mole of hydrogen molecules contain? recall that hydrogen is diatomic. g/mol
Answers: 3
A gas originally at 27 °c and 1.00 atm pressure in a 3.9 l flask is cooled at constant pressure unti...
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