Consider the following chemical reaction:

C (s)+ H2O(g) --> CO(g)+ H2(g)
How many liters of hydrogen gas are formed from the complete reaction of 1.20 mol of C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and temperature of 310 K.

Well, it looks like we have a chemical reaction going on here! Time to do some calculations.

First, we need to find the stoichiometric ratio between C and H2. From the balanced equation, we can see that for every 1 mole of C, we get 1 mole of H2.

Since we have 1.20 mol of C, we can also predict that we'll have 1.20 mol of H2.

Now, let's find the volume of gas using the ideal gas law. The ideal gas law equation is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

Given that the pressure is 1.0 atm, the temperature is 310 K, and the number of moles of H2 is 1.20 mol, we can solve for the volume (V):

V = (nRT) / P
V = (1.20 mol * 0.0821 atm L / (mol K) * 310 K) / 1.0 atm
V = 30.68 L

Therefore, approximately 30.68 liters of hydrogen gas are formed from the complete reaction of 1.20 mol of C.

Well, that's a lot of hydrogen gas! You better make sure to keep it away from any flames. Safety first!

To determine the number of liters of hydrogen gas formed from the complete reaction, we need to use the ideal gas law equation:

PV = nRT

Where:
P = pressure (1.0 atm)
V = volume (which is what we need to find)
n = number of moles of gas (unknown)
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (310 K)

First, we need to find the number of moles of hydrogen gas (H2) produced from 1.20 mol of carbon (C) using the balanced chemical equation:

C (s) + H2O (g) --> CO (g) + H2 (g)

According to the balanced equation, the stoichiometric coefficient for C is 1, and the stoichiometric coefficient for H2 is also 1. This means that for every 1.20 mol of C reacted, 1.20 mol of H2 will be produced.

Now, we can substitute the values into the ideal gas law equation:

PV = nRT

(1.0 atm) (V) = (1.20 mol) (0.0821 L·atm/mol·K) (310 K)

Simplifying the equation:

V = (1.20 mol) (0.0821 L·atm/mol·K) (310 K) / (1.0 atm)

V = 29.7592 L

Therefore, approximately 29.8 liters of hydrogen gas will be formed from the complete reaction of 1.20 mol of C.

To determine the volume of hydrogen gas formed from the reaction, we can use the Ideal Gas Law equation:

PV = nRT

Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)

We are given:
P = 1.0 atm
T = 310 K

First, we need to calculate the number of moles of hydrogen gas produced using the balanced chemical equation. From the equation, we can see that 1 mole of C produces 1 mole of H2.

So, if we have 1.20 mol of C, we will have an equal number of moles of H2.

n(H2) = 1.20 mol

Now we can use the Ideal Gas Law equation to find the volume of hydrogen gas (V).

PV = nRT

V = (nRT) / P

Substituting the given values into the equation:

V = (1.20 mol * 0.0821 L·atm/(mol·K) * 310 K) / 1.0 atm

V = 30.51 L

Therefore, approximately 30.51 liters of hydrogen gas are formed from the complete reaction of 1.20 mol of C.

You will get 1.20 mol of H2.

V= nRT/P