A student runs the reaction: LiOH + CO2 → LiHCO3. The reaction consumes 45.0 g LiOH...

A student runs the reaction: LiOH + CO2 → LiHCO3. The reaction consumes 45.0 g LiOH and produces 72.8 g of LiHCO3. Which of the statements concerning this reaction is true?

Select one: a. The theoretical yield of the product is 117.8 g LiHCO3. b. The theoretical yield of the product is 72.8 g LiHCO3. c. The percent yield of the reaction is 61.8%. d. The actual yield of the product is 72.8 g LiHCO3.

Solutions

Expert Solution

LiOH + CO2 → LiHCO3

moles of LiOH = 45.0/24 = 1.875 moles.

From the balanced equation 1 mole of LiOH = 1 mole of LiHCO3

moles of LiHCO3 formed = 1.875 moles.

mass of LiHCO3 formed = 1.875*68 = 127.5 grams

percent yield = (72.8/127.5)*100 = 57.1 %

Answer = d. The actual yield of the product is 72.8 g LiHCO3.

queen_honey_blossom answered 2 years ago

Next > < Previous

Related Solutions

When the following reaction was carried out, the student obtained 5 g of CO2. If the...

When the following reaction was carried out, the student obtained 5 g of CO2. If the student started with 10 g of CH4 and 10 g of O2, what is the % yield of the reaction? CH4 + 2 O2 --> CO2 + 2 H2O

When the following reaction was carried out, the student obtained 5 g of CO2. If the...

When the following reaction was carried out, the student obtained 5 g of CO2. If the student started with 10 g of CH4 and 10 g of O2, what is the % yield of the reaction? CH4 + 2 O2 --> CO2 + 2 H2O

Consider the reaction: NO2 (g) + CO (g) ---> CO2 (g) + NO (g) The equilibrium...

Consider the reaction: NO2 (g) + CO (g) ---> CO2 (g) + NO (g) The equilibrium constant is at 701 K and 895 K are 2.57 and 567 L mol-1 s-1 so, A. Find the reaction order B. Energy of Activation C. Use part b to find the reaction rate constant at 200 C

Consider the following reaction: CO (g) + H2O (g) ⇌ CO2 (g) + H2(g) If you...

Consider the following reaction: CO (g) + H2O (g) ⇌ CO2 (g) + H2(g) If you start with a mixture containing 1.00 mol of CO and 1.00 mol of H2O, calculate the number of moles of each component in the mixture when equilibrium is reached at 1000 °C. The mixture contains 0.43 mol H2? nCO = nH2O = nCO2 = How do I work this out?

Part A - At 100oC, The equilibrium constant for the reaction: CF4(g) + 2H2O(g) ⇌CO2(g) +...

Part A - At 100oC, The equilibrium constant for the reaction: CF4(g) + 2H2O(g) ⇌CO2(g) + 4HF(g) is Kc,1 = 5.9 And the equilibrium constant at 100oC for the reaction: CO(g) + ½ O2(g) ⇌ CO2(g) is Kc,2 = 1.3 Compute the equilibrium constant at 100oC for the reaction (2 sig figs) 2 CF4(g) + 4H2O(g) ⇌2CO(g) + 8HF(g) + O2(g) is Kc,3 = ? Part B - Consider the reaction below (Equilibrium Constant @ 300K = Kp = 0.150)...

CO2(g) + CCl4(g) => 2 COCl2(g) Calculate ∆G for this reaction at 25 oC under these...

CO2(g) + CCl4(g) => 2 COCl2(g) Calculate ∆G for this reaction at 25 oC under these conditions: PCO2 = 0.112 atm PCCl4 = 0.174 atm PCOCl2 = 0.744 atm

The combustion reaction of propane is as follows. C3H8(g) + 5 O2(g) → 3 CO2(g) +...

The combustion reaction of propane is as follows. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. Answer in KJ/mol reaction (1): C(s) + O2(g) → CO2(g) ΔH = −393.5 kJ/mol reaction (2): H2(g) + 1/2 O2(g) → H2O(l) ΔH = −285.8 kJ/mol reaction (3): 3 C(s) + 4 H2(g) → C3H8(g) ΔH = −103.8 kJ/mol

Consider the reaction: CO2(g)+CCl4(g)⇌2COCl2(g). Calculate ΔG for this reaction at 25 ∘C under these conditions. PCO2=...

Consider the reaction: CO2(g)+CCl4(g)⇌2COCl2(g). Calculate ΔG for this reaction at 25 ∘C under these conditions. PCO2= 0.115 atm PCCl4= 0.170 atm PCOCl2= 0.760 atm

What is ΔGrxno (in kJ) at 647 K for the following reaction? PbO(g) + CO2(g) →...

What is ΔGrxno (in kJ) at 647 K for the following reaction? PbO(g) + CO2(g) → PbCO3(s) PbO: ΔHfo = -219.0 kJ/mol and So = 66.5 J/K mol) PbCO3(s): ΔHfo = -699.1 kJ/mol and So = 131.0 J/K mol) CO2: ΔHfo = -393.5 kJ/mol and So = 213.6 J/K mol)

the reaction of 7.26 g of carbon with excess O2 yeilds 8.20 g of CO2. What...

the reaction of 7.26 g of carbon with excess O2 yeilds 8.20 g of CO2. What is the percent yeild of the reaction?

Subjects