4. A sample containing 10.0 mL of 0.300 M H2C2O4 is mixed with 5.00 mL 0.0500 M KMnO4. The purple color of the permanganate disappears after 37.5 s. a. Calculate the initial concentrations of KMnO4 and H2C2O4 in the mixture. (Hint: use the dilution equation. What is the final volume of the solution?)

Cause its being chemically applied?

C, small, hard spheres with insignificant volumes

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