Question

When acidic precipitation hits limestone the following reaction occurs Caco, (s) + 2 H,09 - Ca* (aq) + Co, (g) + 3 H,0 (liq) If 15.00 mL of Co, were produced at 0.985 atm and 310 K, how many mg of Caco, (MM - 100.09 g/mol) were consumed? Note that there are 1000 mg in a gram. Select one: 0 0.0581 98.2 5.81 x 10 05.81 x 10 58.1 Check

Answer 1

Reaction, Caloz + 2H30t (5) Ca 2+ + caa) Co. (g) + 3 H₂O (4) It we observe the amount of co2 Jormed is dependent only on CaCO3 concentration, So, I mole of Caloz forms I mole of Coz We we use the ideal gas equation to first find the moles of Caloz... then use the value to calculate mass of Caloz consumed. PV=nRT Where, P = pressure of Coz gas = 0.985 atm Ve volume of gas = 15 ml = (154.001L) = 0.015 L. ha moles of co, gas = ? R = universal gas constant = 0.082057 L-atm molik T= 310k = Temperature

Substituting all these values, we get in' on moles of coz. ha Pau RXT h = 0.985 alm x 0.015 k 0.082057 Yahyn x 310k molik = 0.000581 mol. As. moles of co2 produced is equal to moles of Caloz consumed. ". Moles of ca loz consumed = 0.000581 Now, mass of Calozi Az = Moles & Molar Mass = 0.000581 mol x 100.09g mol Mass of Caloz=0.05819 consumed. Now, lg = 1000 mg

So, 0.0581 g = 0.0581 x 1000 mg = 58.1 mg. Auswer > option [E] 58. 1mg of Caloz is consumed.