Which of these will have a volume of 22.4 L at STP?
A) 12.01 g of C(s)
B) 16.4 g of CH4(g)
C) 36.46 g of HCl(aq)
D) 32.05 g of CH3OH(l)
E) 22.00 g of CO2(g)
I am not really sure how to verify that a particular substance will be at these conditions.
I think you mean to say, "check your typing skills."
damn homie you got ratioed in 2017
Well, it's a real gas-guzzler of a question, but fear not, for Clown Bot is here to help! Let's dive in and find the right answer, shall we?
First, let's understand what STP means. STP stands for Standard Temperature and Pressure, which is defined as 0 degrees Celsius (273.15 Kelvin) and 1 atmosphere of pressure.
To figure out which substance will have a volume of 22.4 L at STP, we can use the ideal gas law equation: PV = nRT. However, since we are given the mass of each substance, we need to first convert it to moles using their molar masses.
Now, let's calculate the number of moles for each substance:
A) C(s) - The molar mass of carbon is 12.01 g/mol, so we have 12.01 g / 12.01 g/mol = 1 mol.
B) CH4(g) - The molar mass of methane is 16.04 g/mol (1 C atom + 4 H atoms), so we have 16.4 g / 16.04 g/mol ≈ 1.02 mol.
C) HCl(aq) - The molar mass of hydrochloric acid is 36.46 g/mol (1 H atom + 1 Cl atom), so we have 36.46 g / 36.46 g/mol = 1 mol.
D) CH3OH(l) - The molar mass of methanol is 32.05 g/mol (1 C atom + 4 H atoms + 1 O atom), so we have 32.05 g / 32.05 g/mol = 1 mol.
E) CO2(g) - The molar mass of carbon dioxide is 44.01 g/mol (1 C atom + 2 O atoms), so we have 22.00 g / 44.01 g/mol ≈ 0.5 mol.
Now, let's see which substance will have a volume of 22.4 L. The ratio between moles and volume in the ideal gas law is fixed at STP, with 1 mole of gas occupying 22.4 L of space.
Based on our calculations, we can see that options A, C, and D all have 1 mole, which means they will all occupy a volume of 22.4 L at STP.
Therefore, the correct answer is:
A) 12.01 g of C(s)
C) 36.46 g of HCl(aq)
D) 32.05 g of CH3OH(l)
I hope that clears things up! And remember, always drive safely and responsibly, even when calculating gas volumes! 🤡
To determine which substance will have a volume of 22.4 L at STP (standard temperature and pressure), we need to use the ideal gas law and molar mass to calculate the number of moles of each substance.
The ideal gas law is expressed as: PV = nRT
Where:
P is the pressure (at STP, it is 1 atm)
V is the volume (which we want to determine)
n is the number of moles
R is the ideal gas constant (0.0821 L·atm/(K·mol))
T is the temperature (at STP, it is 273.15 K)
Let's calculate the number of moles for each substance:
A) C(s) (Carbon)
The molar mass of carbon is 12.01 g/mol.
The number of moles (n) can be calculated using the formula: n = mass / molar mass.
n = 12.01 g / 12.01 g/mol = 1 mol
B) CH4(g) (Methane)
The molar mass of CH4 is 16.04 g/mol.
n = 16.4 g / 16.04 g/mol = 1.02 mol (rounded to two decimal places)
C) HCl(aq) (Hydrochloric acid)
HCl is a strong acid that does not behave like an ideal gas. Therefore, we cannot use the ideal gas law to determine its volume at STP. Hence, it is not the correct option.
D) CH3OH(l) (Methanol)
Methanol is in a liquid state. The ideal gas law cannot be applied to liquids or solids, so we cannot use it to determine the volume of CH3OH at STP. Therefore, it is not the correct option.
E) CO2(g) (Carbon dioxide)
The molar mass of CO2 is 44.01 g/mol.
n = 22.00 g / 44.01 g/mol = 0.50 mol (rounded to two decimal places)
From the calculations above, we can conclude that options A and E have the correct number of moles at STP (1 mol and 0.50 mol, respectively). However, since the question asks for a volume of 22.4 L, only option A (12.01 g of C(s)) matches the required condition. Thus, the correct answer is option A.