A scientist is preparing Aluminum Oxide (Al2O3) by reacting solid Aluminum and Oxygen gas together as shown by this chemical equation:4Al + 3O2 → 2Al2O3 The scientist measures the mass of Aluminum before the reaction and finds 107.92 grams. The scientist measures the mass of Aluminum Oxide after the reaction and finds 299.91 grams. The scientist concludes that 95.99 grams of Oxygen gas must have reacted with the Aluminum. Explain the law that the scientist used to predict the amount of Oxygen gas in the reaction and how that law was used to find the amount of Oxygen gas.

Heating it up with cause a quicker reaction time

Answerstudying coal cumbustion as an energy source;

Use the universal gas law formula: pv = nrt now, the key word in this problem is stp, so at stp, temperature will always be 0 degrees celsius and pressure will always be 1.0 atm or 760 torr. given something is at stp, we already know the two variables pressure and temperature. the other thing we can find with the given information is moles. to find moles, just divide grams by molar mass of the element. 16.0g / 2(16.00)g/mol = 0.5 moles plug the values in to the equation pv = nrt (1.0 atm)( x ) = (0.5 )(0+273=273k) the r value is just a constant for when we use atm, liters, moles and kelvin. i'm assuming you want your answer in liters, but if you dont just move the decimal 3 to the right in your final answer. so when plugging these numbers in to your calculator and trying to find x, you get 11.20665 liters using significant figures the answer is 11.2 liters