Assume that you have 2.10 of the deadly gas hydrogen cyanide, . What is the volume of the gas at STP?
2.10 WHAT?
2.10 grams? Then 2.10/molar mass HCN = moles.
Then moles x 22.4L = volume in L.
To find the volume of a gas at STP (Standard Temperature and Pressure), we need to use the ideal gas law equation: PV = nRT, where:
P is the pressure of the gas
V is the volume of the gas
n is the number of moles of gas
R is the ideal gas constant (0.0821 L·atm/(mol·K))
T is the temperature in Kelvin
At STP, the temperature is fixed at 273.15 Kelvin, and the pressure is 1 atmosphere.
First, we need to find the number of moles of hydrogen cyanide (HCN) gas. To do this, we use the molar mass of HCN, which is approximately 27.03 g/mol.
Molar mass of HCN = 1.01 (H) + 12.01 (C) + 14.01 (N) = 27.03 g/mol
Given that you have 2.10 grams of HCN, we can calculate the number of moles:
moles = mass / molar mass
moles = 2.10 g / 27.03 g/mol
moles ≈ 0.0776 mol
Now, we can calculate the volume of the gas using the ideal gas law:
PV = nRT
First, convert the temperature to Kelvin:
T = 273.15 K
Then, substitute the values into the equation:
(1 atm) * V = (0.0776 mol) * (0.0821 L·atm/(mol·K)) * (273.15 K)
Simplifying, we get:
V = (0.0776 mol * 0.0821 L·atm/(mol·K) * 273.15 K) / 1 atm
Performing the calculation:
V ≈ 1.94 L
Therefore, the volume of the hydrogen cyanide gas at STP is approximately 1.94 liters.