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Question 5 5 pts A 77.0-mL sample of a 0.203 M potassium sulfate solution is mixed...
A 77.0-mL sample of a 0.203 M potassium sulfate solution is mixed with 55.0 mL of...
A 77.0-mL sample of a 0.203 M potassium sulfate solution is mixed with 55.0 mL of a 0.226 M lead(II) nitrate solution and this reaction occurs: K2SO4(aq) + Pb(NO3)2 (aq) ⟶ 2 KNO3(aq) + PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 3.71 g. Determine the percent yield. 1 mole PbSO4 = 303.26 g Group of answer choices 98.4% 80.0% 120.% 75.7%
A 77.0-ml sample of a 0.203 M potassium sulfate solution is mixed with 55.0 mL of...
A 77.0-ml sample of a 0.203 M potassium sulfate solution is mixed with 55.0 mL of a 0.226 M lead(II) nitrate solution and this reaction occurs: K2SO4(aq) + Pb(NO3)2 (aq) + 2 KNO3(aq) + PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 3.71 g. Determine the percent yield. 1 mole PbSO4 = 303.26 g Hydrazine, N2H4, is a liquid used as a rocket fuel. It reacts with oxygen to yield nitrogen gas and water....
A 77.0-ml sample of a 0.203 M potassium sulfate solution is mixed with 52.0 mL of...
A 77.0-ml sample of a 0.203 M potassium sulfate solution is mixed with 52.0 mL of a 0.214 Mlead(11) nitrate solution and this reaction occurs: K2SO4(aq) + Pb(NO3)2 (aq) 2 KNO3(aq) + PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 2.43 g. Determine the percent yield. 1 mole PbSO4 = 303.26g 80.1% O 120% o 58.9% o 72.0%
If 1.85 g MgO is combined with enough 1.00 M HCl to make 100.0 mL of...
If 1.85 g MgO is combined with enough 1.00 M HCl to make 100.0 mL of solution in a coffee- cup calorimeter, the temperature of the resulting solution increases from 21.3°C to 35.7 °C. Calculate the enthalpy change for the reaction per mole of Mgo. Assume that the specific heat capacity of the solution is 4.18 J/g.K, and the density of the solution is 1.00 g/mL. - 131 kJ O -613 kJ O-328 kJ 0 -28.3 kJ
The thermochemical equation for the reaction is shown below: 4 Al(s) + 3 O2(g) → 2...
The thermochemical equation for the reaction is shown below: 4 Al(s) + 3 O2(g) → 2 Al2O3(s) AH = -3352 kJ How much heat is released when 12.1 g of Al react with O2(g) at 25 °C and 1 atm? 0 - 104 kJ 0 -3.59 x 105 kJ -1.50 x 103 kJ O-376 kJ A 77.0-mL sample of a 0.203 M potassium sulfate solution is mixed with 55.0 mL of a 0.226 M lead(II) nitrate solution and this reaction...
A 55.5 mL sample of a 0.106 M potassium sulfate solution is mixed with 40.0 mL...
A 55.5 mL sample of a 0.106 M potassium sulfate solution is mixed with 40.0 mL of a 0.106 MM lead(II) acetate solution and the following precipitation reaction occurs: K2SO4(aq)+Pb(C2H3O2)2(aq)→2KC2H3O2(aq)+PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 0.991 g . Part (A) Identify the limiting reactant. 1. PbSO4 2. KC2H3O2 3. Pb(C2H3O2)2 4. K2SO4 Part (B) Determine the theoretical yield. mass of PbSO4 = __________ g Part (C) Determine the percent yield. ____________ %
U Question 30 5 pts If 4.8 g of sulfur react with an excess amount of...
U Question 30 5 pts If 4.8 g of sulfur react with an excess amount of fluorine according to the equation, what mass of the product is formed when the reaction is complete? 1 mole SF6 - 146.05 g S + 3F2-SF o 228 O 9.0 g 328 O 158 D Question 29 5 pts If 1.85 g MgO is combined with enough 1.00 M HCl to make 100.0 mL of solution in a coffee-cup calorimeter, the temperature of the...
65.0 mL sample of a 0.102 M potassium sulfate solution is mixed with 38.5 mL of...
65.0 mL sample of a 0.102 M potassium sulfate solution is mixed with 38.5 mL of a 0.122 M lead(II) acetate solution and the following precipitation reaction occurs: K2SO4(aq)+Pb(C2H3O2)2(aq)→2KC2H3O2(aq)+PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 0.993 g . a. Define the theoretical yield b. Define the percent yield.
If 1.85 g MgO is combined with enough 1.00 M HCl to make 100.0 mL of...
If 1.85 g MgO is combined with enough 1.00 M HCl to make 100.0 mL of solution in a coffee-cup calorimeter, the temperature of the resulting solution increases from 21.3°C to 35.7 °C. Calculate the enthalpy change for the reaction per mole of Mgo. Assume that the specific heat capacity of the solution is 4.18 J/g.K, and the density of the solution is 1.00 g/mL. A 0.704 g of a pure acid, HA, is dissolved in water and an acid-base...
Sodium hydroxide reacts with carbon dioxide as follows: 2 NaOH(s) + CO2(g) Na2CO3(s) + H2O(1) If...
Sodium hydroxide reacts with carbon dioxide as follows: 2 NaOH(s) + CO2(g) Na2CO3(s) + H2O(1) If 3.70 mol NaOH and 2.00 mol CO2 are allowed to react, how many moles of the excess reactant remains? 0.15 mol CO2 O 0.30 mol NaOH O 1.70 NaOH 1.00 mol CO2 How much energy is required to change the temperature of 1.50 L of water from 25.0 °C to 100.0 °C? The specific heat capacity of water is 4.184 J/g.°C; density H2O =...
A 77.0-ml sample of a 0.203 M potassium sulfate solution is mixed with 55.0 mL of a 0.226 M lead(II) nitrate solution and this reaction occurs: K2SO4(aq) + Pb(NO3)2 (aq) + 2 KNO3(aq) + PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 3.71 g. Determine the percent yield. 1 mole PbSO4 = 303.26 g Hydrazine, N2H4, is a liquid used as a rocket fuel. It reacts with oxygen to yield nitrogen gas and water....
A 77.0-ml sample of a 0.203 M potassium sulfate solution is mixed with 52.0 mL of a 0.214 Mlead(11) nitrate solution and this reaction occurs: K2SO4(aq) + Pb(NO3)2 (aq) 2 KNO3(aq) + PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 2.43 g. Determine the percent yield. 1 mole PbSO4 = 303.26g 80.1% O 120% o 58.9% o 72.0%
If 1.85 g MgO is combined with enough 1.00 M HCl to make 100.0 mL of solution in a coffee- cup calorimeter, the temperature of the resulting solution increases from 21.3°C to 35.7 °C. Calculate the enthalpy change for the reaction per mole of Mgo. Assume that the specific heat capacity of the solution is 4.18 J/g.K, and the density of the solution is 1.00 g/mL. - 131 kJ O -613 kJ O-328 kJ 0 -28.3 kJ
The thermochemical equation for the reaction is shown below: 4 Al(s) + 3 O2(g) → 2 Al2O3(s) AH = -3352 kJ How much heat is released when 12.1 g of Al react with O2(g) at 25 °C and 1 atm? 0 - 104 kJ 0 -3.59 x 105 kJ -1.50 x 103 kJ O-376 kJ A 77.0-mL sample of a 0.203 M potassium sulfate solution is mixed with 55.0 mL of a 0.226 M lead(II) nitrate solution and this reaction...
U Question 30 5 pts If 4.8 g of sulfur react with an excess amount of fluorine according to the equation, what mass of the product is formed when the reaction is complete? 1 mole SF6 - 146.05 g S + 3F2-SF o 228 O 9.0 g 328 O 158 D Question 29 5 pts If 1.85 g MgO is combined with enough 1.00 M HCl to make 100.0 mL of solution in a coffee-cup calorimeter, the temperature of the...
If 1.85 g MgO is combined with enough 1.00 M HCl to make 100.0 mL of solution in a coffee-cup calorimeter, the temperature of the resulting solution increases from 21.3°C to 35.7 °C. Calculate the enthalpy change for the reaction per mole of Mgo. Assume that the specific heat capacity of the solution is 4.18 J/g.K, and the density of the solution is 1.00 g/mL. A 0.704 g of a pure acid, HA, is dissolved in water and an acid-base...
Sodium hydroxide reacts with carbon dioxide as follows: 2 NaOH(s) + CO2(g) Na2CO3(s) + H2O(1) If 3.70 mol NaOH and 2.00 mol CO2 are allowed to react, how many moles of the excess reactant remains? 0.15 mol CO2 O 0.30 mol NaOH O 1.70 NaOH 1.00 mol CO2 How much energy is required to change the temperature of 1.50 L of water from 25.0 °C to 100.0 °C? The specific heat capacity of water is 4.184 J/g.°C; density H2O =...
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