In the theoretical reaction
2 B(aq) + 3 D(aq) ---> E(aq) + 4 F(aq)
the concentration of D(aq) is 0.40 mol/L. If 25.0 mL of aqueous B is needed to react completely with 30.0 mL of aqueous D, the concentration of B(aq) is
A-0.48 mol/L
B)
B-0.32 mol/L
C)
C-0.40 mol/L
D)
D-0.72 mol/L
I answered B?
Right. Go to the head of the class.
What is the volume of 26.311g of butane gas (C4H10), at 22.7°C and 125.1 kPa? Round your answer to the nearest thousandth.
I had gotten 0.009?
To determine the concentration of B(aq), you need to use the information given about the reaction and the volumes of the solutions involved.
First, let's calculate the number of moles of D(aq) used in the reaction:
Volume of D(aq) = 30.0 mL = 0.0300 L (converted to liters)
Concentration of D(aq) = 0.40 mol/L
Moles of D(aq) used = Volume × Concentration = 0.0300 L × 0.40 mol/L = 0.0120 mol
According to the balanced equation, the stoichiometric ratio between B(aq) and D(aq) is 2:3. This means that 2 moles of B(aq) react with 3 moles of D(aq). Therefore, the number of moles of B(aq) required can be calculated as:
Moles of B(aq) required = (2/3) × Moles of D(aq) used = (2/3) × 0.0120 mol = 0.00800 mol
Now we need to determine the concentration of B(aq) based on the volume used:
Volume of B(aq) = 25.0 mL = 0.0250 L (converted to liters)
Concentration of B(aq) = Moles of B(aq) used / Volume = 0.00800 mol / 0.0250 L = 0.320 mol/L
Therefore, the concentration of B(aq) is 0.320 mol/L, which corresponds to option B. So your answer is correct.