Answer Happy

Use the following standards for all your calculations. Temperature Pressure Molar Volume STP 273.15 K 101.325kPa 22.4 L/mol SATP 298.15 K 100.000kPa 24.8 L/mol Univeral Gas Constant R=8.314 (L-kPa)/(K.mol) Question 1 (1 point) (2.14x10^2) mL of 0.175-mol/L Pb(NO3)2 (aq) is mixed with excess KBr (aq). Calculate the mass of the precipitate. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 units Answer

Question 2 (1 point) ✓ Saved 30 g of iron reacts with 10g of oxygen to form rust (Fe2O3). Which reactant is the limiting reactant, and how much excess will there be? Iron is the limiting reactant, there will be an excess of 4.9 x 10^-1 mol of oxygen left Oxygen is the limiting reactant, there will be an excess of 1.3 x 10^-1 mol of iron left Oxygen is the limiting reactant, there will be an excess of 2.2 x 10^-1 mol of iron left Iron is the limiting reactant, there will be an excess of 2.6 x 10^-1 mol of oxygen left

Question 3 (1 point) (8.7000x10^-1) L of methane, CH4(g), is combusted with (5.50x10^-1) L of oxygen gas in STP conditions. Once the reaction is completely finished, how many moles of the excess reagent remains? Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer

Question 4 (1 point) A (1.70x10^1) g piece of copper reacts with (1.040x10^2) g of silver nitrate dissolved in solution. What mass of silver will be formed from this reaction? Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 units Answer

Question 5 (1 point) Approximately (1.29x10^1) g of lead(II) acetate, Pb(CH3COO)2, is weighed out and placed in a (9.5000x10^1) mL solution of 0.150-mol/L sodium hydroxide. Calculate the mass of precipitate produced in this reaction. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 units Answer