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) à\longrightarrow ZnCl2(aq) + H2(g)

See above under a difference screen name. Sarah, you continue to use difference screen names and I've asked you several times to use the same screen name. It really slows us down in getting the answers out to you AND it serves no useful purpose.

To determine the pressure of the collected H2 gas, we can use the ideal gas law equation, which is given by:

PV = nRT

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

First, let's calculate the number of moles of H2 gas produced. According to the balanced chemical equation, the stoichiometry between Zn and H2 is 1:1. So, if we have 0.010 moles of Zn, we will also have 0.010 moles of H2.

Next, let's convert the temperature from degrees Celsius to Kelvin. We have 270 K.

Now, let's plug the values into the ideal gas law equation:

PV = nRT

P × 1.0 L = 0.010 moles × 0.0821 L·atm/(mol·K) × 270 K

P = (0.010 moles × 0.0821 L·atm/(mol·K) × 270 K) / 1.0 L

Solving this equation will give us the pressure (P) of the H2 gas collected in the 1.0 L flask.