<u>Answer:</u> The average rate of the reaction is ![7.82\times 10^{-3}M/min](https://tex.z-dn.net/?f=7.82%5Ctimes%2010%5E%7B-3%7DM%2Fmin)
<u>Explanation:</u>
To calculate the molarity of hydrogen gas generated, we use the equation:
![\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}](https://tex.z-dn.net/?f=%5Ctext%7BMolarity%20of%20the%20solution%7D%3D%5Cfrac%7B%5Ctext%7BMoles%20of%20solute%7D%7D%7B%5Ctext%7BVolume%20of%20solution%20%28in%20L%29%7D%7D)
Moles of hydrogen gas = ![3.91\times 10^{-2}mol](https://tex.z-dn.net/?f=3.91%5Ctimes%2010%5E%7B-2%7Dmol)
Volume of solution = 250 mL = 0.250 L (Conversion factor: 1 L = 1000 mL)
Putting values in above equation, we get:
![\text{Molarity of }H_2=\frac{3.91\times 10^{-2}mol}{0.250L}=0.1564M](https://tex.z-dn.net/?f=%5Ctext%7BMolarity%20of%20%7DH_2%3D%5Cfrac%7B3.91%5Ctimes%2010%5E%7B-2%7Dmol%7D%7B0.250L%7D%3D0.1564M)
Average rate of the reaction is defined as the ratio of concentration of hydrogen generated to the time taken.
To calculate the average rate of the reaction, we use the equation:
![\text{Average rate of the reaction}=\frac{\text{Concentration of hydrogen generated}}{\text{Time taken}}](https://tex.z-dn.net/?f=%5Ctext%7BAverage%20rate%20of%20the%20reaction%7D%3D%5Cfrac%7B%5Ctext%7BConcentration%20of%20hydrogen%20generated%7D%7D%7B%5Ctext%7BTime%20taken%7D%7D)
We are given:
Concentration of hydrogen generated = 0.1564 M
Time taken = 20.0 minutes
Putting values in above equation, we get:
![\text{Average rate of the reaction}=\frac{0.1564M}{20.0min}\\\\\text{Average rate of the reaction}=7.82\times 10^{-3}M/min](https://tex.z-dn.net/?f=%5Ctext%7BAverage%20rate%20of%20the%20reaction%7D%3D%5Cfrac%7B0.1564M%7D%7B20.0min%7D%5C%5C%5C%5C%5Ctext%7BAverage%20rate%20of%20the%20reaction%7D%3D7.82%5Ctimes%2010%5E%7B-3%7DM%2Fmin)
Hence, the average rate of the reaction is ![7.82\times 10^{-3}M/min](https://tex.z-dn.net/?f=7.82%5Ctimes%2010%5E%7B-3%7DM%2Fmin)
Answer:
1.200g
Explanation:
At the top it's 0 and that scale goes by 10s
The middle scale is 1 and it goes by 1s
The bottom scale is .2 and it goes by .1s
1+.2= 1.2 the extra zeroes are just place holders
1.200g
Answer:
5.71 g
Explanation:
Step 1: Write the balanced equation
2 K + Cl₂ ⇒ 2 KCl
Step 2: Calculate the moles corresponding to 12.0 g of KCl
The molar mass of KCl is 74.55 g/mol.
12.0 g × 1 mol/74.55 g = 0.161 mol
Step 3: Calculate the moles of Cl₂ needed to produce 0.161 moles of KCl
The molar ratio of Cl₂ to KCl is 1:2. The moles of Cl₂ needed are 1/2 × 0.161 mol = 0.0805 mol
Step 4: Calculate the mass corresponding to 0.0805 moles of Cl₂
The molar mass of Cl₂ is 70.91 g/mol.
0.0805 mol × 70.91 g/mol = 5.71 g
I had the same question, it's most likely B.