What volume of HCl gas is produced by the reaction of 2.4 liters of H2 gas with 1.5 liters of Cl2 gas? (Volumes are at the same T and P.)

1. 3.0 liters
2. 4.8 liters
3. 0.75 liters
4. 2.4 liters
5. 1.5 liters

Well, well, well! It seems we have a reaction on our hands. The reaction between H2 and Cl2 forms HCl gas. Since the reaction is at the same temperature and pressure, we can use the stoichiometry to solve this problem.

The balanced chemical equation is:
H2 + Cl2 → 2HCl

According to the stoichiometry of the equation, one mole of H2 reacts with one mole of Cl2 to produce two moles of HCl. Since we have the volumes, we need to use the ideal gas law to convert them into moles.

Using the ideal gas law: PV = nRT
We know the pressure and temperature are the same, so we can simplify:
P1V1 = n1RT
P2V2 = n2RT

Dividing the two equations gives us:
V1/V2 = n1/n2

Plugging in the values:
V1 = 2.4 L
V2 = 1.5 L

V1/V2 = 2.4/1.5

Therefore, the volume of HCl gas produced is (2.4/1.5) times the volume of Cl2 gas, which is 1.6 times. Multiply this by 1.5 L (the volume of Cl2) to get the answer.

1.6 * 1.5 L = 2.4 L

So, the volume of HCl gas produced is 2.4 liters. Looks like option 4 is the lucky winner!

To determine the volume of HCl gas produced by the reaction, we first need to determine the balanced chemical equation for the reaction between H2 gas and Cl2 gas.

The balanced chemical equation for this reaction is:

H2(g) + Cl2(g) → 2HCl(g)

From the equation, we can see that 1 mole of H2 gas reacts with 1 mole of Cl2 gas to produce 2 moles of HCl gas.

To find the volume of HCl gas produced, we can use the ratios of the coefficients in the balanced equation.

For every mole of H2 gas, we get 2 moles of HCl gas.

Given that the initial volume of H2 gas is 2.4 liters and the initial volume of Cl2 gas is 1.5 liters, we can use the ratio of volumes to determine the volume of HCl gas produced.

The volume ratio is given by:

Volume HCl gas / Volume H2 gas = Coefficient HCl gas / Coefficient H2 gas

Volume HCl gas / 2.4 liters = 2 / 1

Volume HCl gas = 2 x 2.4 liters / 1

Volume HCl gas = 4.8 liters

Therefore, the volume of HCl gas produced by the reaction is 4.8 liters.

The correct answer is option 2.

To determine the volume of HCl gas produced, we need to use the balanced equation for the reaction between hydrogen gas (H2) and chlorine gas (Cl2) to form hydrogen chloride gas (HCl). The balanced equation is as follows:

H2(g) + Cl2(g) → 2HCl(g)

From the balanced equation, we can see that the stoichiometric ratio between H2 and HCl is 1:2. This means that 1 mole of H2 reacts to form 2 moles of HCl. Since we're given the volume of H2 gas (2.4 liters), we need to use the ideal gas law to convert it to moles.

The ideal gas law is represented as PV=nRT, where:
P = pressure of the gas
V = volume of the gas
n = number of moles
R = ideal gas constant
T = temperature of the gas

Since the volume and temperature are constant, we can rewrite the ideal gas law as n = (PV) / RT.

Now, let's calculate the number of moles of H2 gas:
nH2 = (PV) / RT
= (1 atm * 2.4 L) / (0.0821 atm·L/mol·K * T)
= (2.4 L) / (0.0821 L/mol·K * T)

Similarly, we can calculate the number of moles of Cl2 gas using the given volume of Cl2 gas (1.5 liters):
nCl2 = (PV) / RT
= (1 atm * 1.5 L) / (0.0821 atm·L/mol·K * T)
= (1.5 L) / (0.0821 L/mol·K * T)

Since the stoichiometric ratio between H2 and HCl is 1:2, the number of moles of HCl gas produced will be twice the number of moles of H2 gas consumed.

nHCl = 2 * nH2
= 2 * (2.4 L) / (0.0821 L/mol·K * T)
= 4.8 L / (0.0821 L/mol·K * T)
= 4.8 / (0.0821 * T) moles

Finally, we convert the number of moles of HCl gas to volume using the ideal gas law:

VHCl = nHCl * (RT / P)
= (4.8 / (0.0821 * T)) * (0.0821 atm·L/mol·K * T) / 1 atm
= 4.8 L

Therefore, the volume of HCl gas produced by the reaction is 4.8 liters (option 2).

H2 + Cl2 ==> 2HCl

2.4L H2 will produce 2*2.4 = 4.8 L HCl if it has an excess of Cl2.

1.5 L Cl2 will produce 2*1.5 = 3.0 L HCl if it has an excess of H2.

This is a limiting reagent problem; I know that because BOTH reactants are given. Therefore, the amount HCl produced will be the smaller value (3.0L HCl) and Cl2 is the limiting reagent. H2 gas will be in excess. You can calculate, easily, the amount of H2 not reacted.
1.5 L Cl2 x (1 mole H2/1 mole Cl2) = 1.5 moles H2 used. We had 2.4 moles H2 initially; therefore, we have left 2.4-1.5 = ?? L H2 unreacted.