When 0.010 moles of Zn(s) reacts with 30.0 mL of 1.0 M HCl, the H2 gas produced is collected in a 1.0 L flask at a temperature of 270 K. What is the pressure (atm) of H2 gas collected?
Zn(s) + 2HCl(aq) = ZnCl2(aq) + H2(g)
Oh, the good old Zn(s) and HCl(aq) party! Let's calculate the pressure of the H2 gas collected, shall we?
First, let's find out the number of moles of H2 gas produced. According to the balanced equation, the ratio between Zn(s) and H2(g) is 1:1. So, since we have 0.010 moles of Zn(s), we'll have 0.010 moles of H2(g).
Next, we need to use the ideal gas law to find the pressure of the H2 gas. The ideal gas law equation is P * V = n * R * T, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature.
Given:
V (volume) = 1.0 L
n (number of moles) = 0.010 moles
R (ideal gas constant) = 0.0821 L·atm/(mol·K)
T (temperature) = 270 K
Plugging in the values:
P * 1.0 L = 0.010 moles * 0.0821 L·atm/(mol·K) * 270 K
Now, let me grab my calculator and do the math for you.
(Humming elevator music while calculating...)
The pressure of the collected H2 gas is approximately... (drumroll) 0.220065 atm.
So, the pressure of the H2 gas collected is approximately 0.220065 atm. Enjoy your H2 gas party, my friend!
To determine the pressure of the collected H2 gas, we can use the Ideal Gas Law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
1) Convert the given temperature from Kelvin to Celsius:
270 K - 273.15 = -3.15 °C
2) Convert the mL of HCl solution to liters:
30.0 mL = 30.0 mL * (1 L / 1000 mL) = 0.030 L
3) Determine the number of moles of HCl used:
0.030 L * 1.0 M = 0.030 moles HCl
4) According to the balanced equation, the stoichiometric ratio between HCl and H2 is 2:1. Therefore, the number of moles of H2 produced is half the number of moles of HCl used:
0.030 moles HCl * (1/2) = 0.015 moles H2
5) Use the Ideal Gas Law equation to calculate the pressure:
PV = nRT
P * 1.0 L = 0.015 moles * 0.0821 L·atm/(mol·K) * 270 K
P = (0.015 moles * 0.0821 L·atm/(mol·K) * 270 K) / 1.0 L
P = 0.3031 atm
Therefore, the pressure of the collected H2 gas is 0.3031 atm.
To find the pressure of the collected H2 gas, you can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
First, let's determine the number of moles of H2 gas produced. According to the balanced equation, 1 mole of Zn reacts with 2 moles of HCl to produce 1 mole of H2.
Given that 0.010 moles of Zn reacted, we can determine the moles of H2 produced by multiplying the moles of Zn by the mole ratio:
0.010 mol Zn * (1 mol H2 / 1 mol Zn) = 0.010 mol H2
Now, let's convert the volume from milliliters (mL) to liters (L):
30.0 mL = 30.0 mL * (1 L / 1000 mL) = 0.030 L
The temperature is already given in Kelvin as 270 K.
Now, we can substitute these values into the ideal gas law equation:
PV = nRT
P * 1.0 L = 0.010 mol * 0.0821 L*atm/(mol*K) * 270 K
Simplifying the equation:
P = (0.010 mol * 0.0821 L*atm/(mol*K) * 270 K) / 1.0 L
Calculating the pressure:
P = 0.2231 atm
Therefore, the pressure of the collected H2 gas is 0.2231 atm.
This is a limiting reagent (LR) problem.
mols Zn = 0.01
mols HCl = M x L = 0.03 x 1 = 0.03
mols H2 produced from Zn if we had all of the HCl we needed = 0.01 (from the 1 mol Zn gives 1 mol H2.
molsl H2 produced from 0.03 mols HCl if we had all of the Zn we needed = 0.03 x 1/2 = 0.015 mols H2 (from 2 mol HCl produces 1 mol H2).
In LR problems the SMALLER amount of the product produces is the correct answer (0.01 mol) and the reagent producing that value is the LR.
So 0.01 mol H2 produced. Substitute that into PV = nRT and solve for P.