Two more need help figuring out how to do:
How many liters of water vapor can be produced when 8.23 liters of oxygen gas reacts with hydrogen gas (H2g + 02g = H20g.
How many liters of water vapor can be produced if 108 grams of methane gas are conbusted at 312K and 98 atm. CH4 + 202 = C02 + 2H20
In your first qeustion, you need to state what the temperature and pressure of the oxygen is. Your chemical reaction equation is not balanced.
108 g of methane is 108/16 = 6.75 moles. The reaction will produce 13.5 moles of H2O. Convert that to liters using the perfect gas law.
To solve both of these stoichiometry problems, we need to use the balanced chemical equations and the ideal gas law. Let's break down each problem step by step:
1. How many liters of water vapor can be produced when 8.23 liters of oxygen gas reacts with hydrogen gas (H2g + O2g = H2Og)?
Step 1: Write the balanced chemical equation:
2H2g + O2g -> 2H2Og
Step 2: Identify the mole ratio:
From the balanced equation, we see that 2 moles of H2O are produced for every 1 mole of O2 consumed.
Step 3: Convert given liters of oxygen gas (O2) to moles using the ideal gas law:
PV = nRT
Given:
P = pressure (atm) - not given
V = volume (liters) - 8.23 liters
n = moles - unknown
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature (Kelvin) - not given
Since we don't have the pressure or temperature, we cannot directly convert the volume to moles. We need more information to proceed with this specific problem.
2. How many liters of water vapor can be produced if 108 grams of methane gas are combusted at 312K and 98 atm (CH4 + 2O2 = CO2 + 2H2O)?
Step 1: Write the balanced chemical equation:
CH4g + 2O2g -> CO2g + 2H2Og
Step 2: Identify the mole ratio:
From the balanced equation, we see that 2 moles of H2O are produced for every 1 mole of CH4 consumed.
Step 3: Convert given grams of methane gas (CH4) to moles:
molar mass of CH4 = 12.01 g/mol + 4(1.01 g/mol) = 16.05 g/mol
Given:
m = mass (grams) - 108 grams
M = molar mass (grams/mole) - 16.05 g/mol
moles of CH4 = m / M
Step 4: Convert moles of CH4 to moles of H2O:
From the mole ratio in the balanced equation, we know that for every 1 mole of CH4, 2 moles of H2O are produced.
moles of H2O = 2 * moles of CH4
Step 5: Convert moles of H2O to liters using the ideal gas law:
Given:
P = pressure (atm) - 98 atm
V = volume (liters) - unknown
n = moles - calculated in Step 4
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature (Kelvin) - converted from 312K
Using the ideal gas law:
PV = nRT
V = (nRT)/P
Substitute the known values and solve for V to find the volume of water vapor produced in liters.
Please note that for the second problem, we need the temperature in Kelvin to calculate accurately. Ensure you convert any temperature given in Celsius to Kelvin by adding 273.15.