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)

wondering if water vapor will be in the flask?

Sarah, I worked this for you below. It's a waste of our time to answer twice AND you posted under Lauren also. I assumed no water vapor in the flask.

7atm

To find the pressure (atm) of the H2 gas collected, we need to use the ideal gas law equation:

PV = nRT

Where:
P represents the pressure in atm
V represents the volume in liters
n represents the number of moles
R is the ideal gas constant (0.0821 L.atm/mol.K)
T is the temperature in Kelvin

First, we need to determine the number of moles of H2 gas produced. According to the balanced chemical equation, for every 1 mole of Zn reacting with 2 moles of HCl, 1 mole of H2 gas is produced.

Given that 0.010 moles of Zn reacts, this means that 0.010 moles of H2 gas would be produced as well.

Next, we convert the volume of the flask from mL to liters. 30.0 mL is equal to 0.03 L.

Substituting the values into the ideal gas law equation:

PV = nRT
P * 1.0 L = 0.010 mol * 0.0821 L.atm/mol.K * 270 K

Now, we just need to solve for P:

P = (0.010 mol * 0.0821 L.atm/mol.K * 270 K) / 1.0 L

Calculating the value:

P = 2.2331 atm

Therefore, the pressure of the H2 gas collected is 2.2331 atm.