Zn+HCl---->ZnCl2+H2
If you measure the total volume of collected gas over water at 65*C to be 728 mL at a total pressure of 845 torr, how many milliliters of 2.6 HCl would be required to produce the correct amount of hydrogen?
Well, it seems you've stumbled into my laboratory! Don't worry, I won't let you get bored with all these chemical equations.
To solve this problem, we need to find out how much HCl you would need to produce the correct amount of hydrogen gas. Let's break it down step by step, shall we?
First, we need to convert the pressure from torr to atm. There are 760 torr in 1 atm, so 845 torr would be 845/760 atm.
Next, we convert the temperature from Celsius to Kelvin. To do this, we add 273.15 to the temperature. So 65°C would be 65 + 273.15 K.
Now that we have the pressure and temperature, we can use the ideal gas law equation: PV = nRT.
We are given the pressure (P), temperature (T), and volume (V), and we need to find the number of moles (n). So now we need to solve for n.
n = PV / RT
Now, to find how many moles of hydrogen gas we need, we use the balanced chemical equation:
Zn + 2HCl -> ZnCl2 + H2
From the equation, we see that 1 mole of Zn reacts with 2 moles of HCl to produce 1 mole of H2.
So, once we find the number of moles of H2, we can work backward to figure out the moles of HCl needed.
Finally, we can use the equation:
moles of HCl = moles of H2 / 2
Now comes the fun part! Once we have the moles of HCl, we can use its molarity (2.6 HCl) to calculate the required volume.
Given all these steps, I'm afraid I've assembled quite a complex experiment for you. But don't worry, I'm here to clown around and make it more enjoyable! Let me crunch the numbers for you:
Using the ideal gas law, we find the number of moles of H2 produced. Then, we divide that by 2 (because we need twice as many moles of HCl) to find the moles of HCl needed. Finally, we can calculate the volume using the molarity.
Remember, safety goggles on, and let's calculate away!
To determine the volume of 2.6 M HCl required to produce the correct amount of hydrogen gas, we need to use the stoichiometry of the balanced equation and the ideal gas law.
First, let's calculate the moles of hydrogen gas produced using the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in L)
n = moles
R = gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
Converting the given values:
Pressure = 845 torr = 845/760 atm (convert to atm)
Total volume of gas = 728 mL = 728/1000 L (convert to L)
Temperature = 65°C = 65 + 273.15 K (convert to Kelvin)
Using the ideal gas law equation, we can calculate the moles of hydrogen gas produced:
n = PV / RT
Substituting the given values:
n = (845/760) * (728/1000) / (0.0821 * (65 + 273.15))
Now, since the stoichiometric ratio of hydrogen gas to HCl is 1:2, we can determine the moles of HCl needed by dividing the moles of hydrogen gas by 2:
moles of HCl = n / 2
Finally, we can calculate the volume of 2.6 M HCl solution corresponding to the moles needed:
volume = (moles of HCl) / concentration
Substituting the values, we can find the volume of 2.6 M HCl required to produce the correct amount of hydrogen gas.