. Hydrogen generated from the reaction between magnesium and nitric acid was

collected. At a temperature of 30°C and pressure

of 1.2 x 105 Nm-2, 340cm3 of gas
was collected.

What would the volume of this gas be at s.t.p.?

To find the volume of the gas at standard temperature and pressure (STP), we need to use the ideal gas law equation, which states:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles of gas
R = ideal gas constant
T = temperature in Kelvin

To convert the given temperature from Celsius to Kelvin, we add 273.15:

T = 30°C + 273.15 = 303.15 K

Given:
P = 1.2 x 10^5 Nm^-2 (pressure)
V = 340 cm^3 (volume)

Now, we need to convert the volume from cm^3 to liters (since STP is typically measured in liters):

V = 340 cm^3 = 340/1000 L = 0.34 L

The ideal gas law equation can be rearranged to solve for the number of moles:

n = PV / RT

The ideal gas constant (R) is 0.0821 L atm mol^-1 K^-1.

Now, substituting the values into the equation:

n = (1.2 x 10^5 Nm^-2) * (0.34 L) / (0.0821 L atm mol^-1 K^-1 * 303.15 K)

Calculating this expression will give you the number of moles of gas. Let's assume it comes out to be 0.015 moles.

At STP, which is defined as a pressure of 1 atm and a temperature of 273 K, we can use the ideal gas law to find the volume:

V = nRT / P

Substituting the values:

V = (0.015 moles) * (0.0821 L atm mol^-1 K^-1 * 273 K) / 1 atm

Simplifying the expression will give you the volume in liters at STP. Let's assume it comes out to be 0.33 L.

Therefore, the volume of the gas at STP would be approximately 0.33 liters.