How many liters of hydrogen gas are needed to react with CS2 to produce 1.25 L of CH4 at STP?
See example below. 1 mole of gas at STP occupies 22.4 L.
To determine the number of liters of hydrogen gas needed to react with CS2 to produce 1.25 L of CH4 at STP, we need to use the balanced chemical equation and the concept of stoichiometry.
The balanced chemical equation for the reaction between CS2 and H2 to produce CH4 is:
CS2 + 4H2 -> CH4 + 2H2S
From the balanced equation, we can see that 4 moles of H2 are required to produce 1 mole of CH4. We also know that 1 mole of any ideal gas at STP occupies 22.4 L.
To calculate the number of liters of H2 gas needed, we can follow these steps:
Step 1: Calculate the moles of CH4 needed.
Given that the volume of CH4 is 1.25 L at STP, we can convert it to moles using the ideal gas equation:
n = (V * P) / (R * T)
where,
n = moles of CH4
V = volume of CH4 (in liters) = 1.25 L
P = pressure at STP = 1 atm
R = ideal gas constant = 0.0821 L•atm/(mol•K)
T = temperature at STP = 273 K
n = (1.25 * 1) / (0.0821 * 273)
n ≈ 0.0559 moles
Step 2: Calculate the moles of H2 needed.
From the balanced chemical equation, we know that 4 moles of H2 are needed to produce 1 mole of CH4. Therefore, the moles of H2 needed can be calculated as:
moles of H2 = 4 * moles of CH4
moles of H2 = 4 * 0.0559
moles of H2 ≈ 0.2237 moles
Step 3: Convert moles of H2 to liters.
Since 1 mole of any ideal gas at STP occupies 22.4 L, we can calculate the required number of liters of H2 gas as:
liters of H2 = moles of H2 * 22.4
liters of H2 ≈ 0.2237 * 22.4
liters of H2 ≈ 4.99 L
Therefore, approximately 4.99 liters of hydrogen gas are needed to react with CS2 to produce 1.25 liters of CH4 at STP.
To find out how many liters of hydrogen gas are needed to react with CS2 to produce 1.25 L of CH4 at STP, we need to use the balanced chemical equation for the reaction and stoichiometry.
The balanced chemical equation for the reaction between CS2 and H2 to produce CH4 is:
CS2 + 4H2 -> CH4 + 2H2S
From the equation, we can see that for every molecule of CS2, we need 4 molecules of H2 to produce 1 molecule of CH4.
Since we are given the volume in liters, we need to convert the volume of CH4 from liters to molecules. To do this, we can use the conversion factor:
1 mole of any gas at STP = 22.4 L
Therefore, 1.25 L of CH4 is equal to:
1.25 L * (1 mole of CH4 / 22.4 L) = 0.0558 moles of CH4
Now, using the stoichiometry from the balanced equation, we know that for every mole of CH4, we need 4 moles of H2.
So, 0.0558 moles of CH4 is equal to:
0.0558 moles CH4 * (4 moles of H2 / 1 mole of CH4) = 0.223 moles of H2
Finally, we can convert the moles of H2 to liters using the conversion factor:
0.223 moles of H2 * (22.4 L / 1 mole of H2) = 4.9952 L of H2
Therefore, approximately 4.995 L of hydrogen gas (H2) are needed to react with CS2 to produce 1.25 L of CH4 at STP.