Please help me solve for the three red boxes. GAS LAW IDEAL GAS LAW CONSTANT INTRODUCTION LABORATORY SIMULATION Lab Data \table[[Mass of magnesium (g), 0.020], [Moles of magnesium (mo), 0.00082], [Temperature of water (C), 24.0], [Temperature of water (K), 297.15]. [Vapor pressure of water (mmHg), 22.4], [Barometric pressure (mmHg), 781.0])] Observations Once inverted and placed into water beaker the Mg reacts by releasing gas bubbles and doesn't stop until it fully dissolves. \table [Volume of hydrogen gas collected (mL)], [Volume of hydrogen gas collected (L).]. [Pressure of hydrogen gas (mmHg), 758.6],[Pressure of hydrogen gas (atm)].[ Moles of hydrogen gas produced (mol), 0.00082], [Ideal gas constant (Latm*mol" "K"),0.080]] How to calculate ideal gas constant Water Vapor Pressure Table GAS LAW IDEAL GAS LAW CONSTANT INTRODUCTION LABORATORY SIMULATION Lab Data X Mass of magnesium (g) Moles of magnesium (mol) Temperature of water (°C) Temperature of water (K) 0x00 0.00082 21.0 10 297.15 Vapor pressure of water (mmHg) Barometric pressure (mmHg) Observations Once inverted at placed into water beaker the Mg reacts by re gas bubbles and doesn't stop ured in fully dissolves Volume of hydrogen gas collected (mL) Volume of hydrogen gas collected (L) Pressure of hydrogen gas immHg) Presseire of hydrogen gas (at) Moles of hydrogen gas produced (mo) desi gas constant atm-mel-K) 750.6 000082 0.00 20 21 21 MY NOTES

▼ Part B 2NO3(aq) +8H(aq) + 6e 3Fe(s) + 2NO3 (aq) +8H+ (aq) 3Fe(s)→→3Fe²+ (aq) + 6e →>> 2NO(g) + 4H₂0 (1) →3Fe²+ (aq) + 2NO(g) + 4H₂O(1) IVE ΑΣΦ Calculate El using the tabulated standard electrode potentials at 25 °C. cell Express your answer in volts to three significant figures. Eeell= 1.21 SWE Submit Previous Answers Request Answer 2+ X Incorrect; Try Again; 4 attempts remaining ? V stontiol buoubtrooting the electro na

Complete the table of reactants and products below and identify the limiting reactant.

Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. relative pH of 0.1 M aqueous solution species H20 4 H,PO4 HNO, (Choose one) NO2 7 OH (Choose one) HF (Choose one) ▼