I need to know how to figure this out, step by step... Don't assume I know anything.. Break it down for me like I'm a 5 year old... I'm really horrible at figuring out where to even begin... what steps to use.. etc.. Thank you!!
CO2(g)+4H2(g)→CH4(g)+2H2O(g)
How many moles of methane are produced when 59.6moles of carbon dioxide gas react with excess hydrogen gas?
Express your answer with the appropriate units. For example, write the unit moles as mol.
How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 19.1moles of water vapor?
Sure, I can break it down for you step by step. Let's start with the first question.
Question 1: How many moles of methane are produced when 59.6 moles of carbon dioxide gas react with excess hydrogen gas?
Step 1: Understand the equation
The given equation is CO2(g) + 4H2(g) -> CH4(g) + 2H2O(g). This shows the balanced chemical equation for the reaction.
Step 2: Identify the mole ratio
From the balanced equation, we can see that for every one mole of carbon dioxide (CO2), we produce one mole of methane (CH4). This is because the coefficient in front of CO2 (1) is the same as the coefficient in front of CH4 (1).
Step 3: Use the mole ratio to calculate the answer
Since 59.6 moles of carbon dioxide (CO2) are given, we can use the mole ratio to determine the number of moles of methane (CH4) produced. Since the mole ratio is 1:1, we conclude that 59.6 moles of carbon dioxide will produce 59.6 moles of methane.
Therefore, the answer to the first question is 59.6 moles of methane (CH4).
Now let's move on to the second question.
Question 2: How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 19.1 moles of water vapor?
Step 1: Understand the equation
The equation provided, CO2(g) + 4H2(g) -> CH4(g) + 2H2O(g), is the same as the previous one. We're still looking at the same balanced chemical equation.
Step 2: Identify the mole ratio
Now, we want to find the number of moles of hydrogen gas (H2) needed to produce 19.1 moles of water vapor (H2O). From the equation, we can see that for every two moles of water vapor, we need four moles of hydrogen gas. This is because the coefficient in front of H2O (2) is twice the coefficient in front of H2 (4).
Step 3: Use the mole ratio to calculate the answer
Since the mole ratio is 2:4 (or simplified as 1:2), we can determine the number of moles of hydrogen gas required to produce 19.1 moles of water vapor. By multiplying the number of moles of water vapor by the mole ratio, we get:
19.1 moles H2O * (2 moles H2 / 2 moles H2O) = 19.1 moles H2
Therefore, the answer to the second question is 19.1 moles of hydrogen gas (H2).
I hope this step-by-step breakdown helps you understand how to approach and solve these types of problems. Let me know if you have any further questions!
To solve these problems step-by-step, let's break them down into smaller tasks:
Task 1: Determine the balanced chemical equation
First, we need to make sure the chemical equation is balanced. Let's check if the given equation is balanced:
CO2(g) + 4H2(g) -> CH4(g) + 2H2O(g)
The equation is already balanced, so we can move on to the next task.
Task 2: Identify the given information and what we are asked to find
For the first question, we are given the amount of carbon dioxide (CO2) and asked to find the amount of methane (CH4) produced.
For the second question, we are given the amount of water vapor (H2O) and asked to find the amount of hydrogen gas (H2) needed.
Task 3: Convert the given units to moles
To solve these problems, we need to convert the given amounts to moles. We can use the molar mass of each compound to convert from grams to moles.
Task 4: Use the stoichiometry of the balanced equation
From the balanced equation, we can determine the ratio of moles of reactants and products. This ratio allows us to calculate the number of moles of the compound we are asked to find.
Task 5: Perform the calculations
Now, let's perform the calculations using the given information and the steps outlined above.
For the first question:
Step 1: Convert the amount of carbon dioxide gas (CO2) to moles using its molar mass.
Step 2: Use the stoichiometry of the balanced equation to determine the moles of methane gas (CH4) produced.
For the second question:
Step 1: Convert the amount of water vapor (H2O) to moles using its molar mass.
Step 2: Use the stoichiometry of the balanced equation to determine the moles of hydrogen gas (H2) needed.
I will provide you with the step-by-step calculations for each question separately.
This is no different than those problems we've been doing. You can convert any mole in an equation to any mole of something else in the same equation just by using the coefficients in the balanced equation
CO2(g)+4H2(g)→CH4(g)+2H2O(g)
Step 1. You have the balanced equation.
Step 2. Convert what you have to mols but your problem starts with mols so that's already done.
Step 3. The conversion step using the coefficients in the balanced equation.
59.6 mols CO2 x (1 mol CH4/1 mol CO2) = 59.6 mols x 1/1 = 59.6 mols CH4.
You always take the mols of what you have and multiply by the conversion factor (made up of the coefficients in the balanced equation) to convert mols of what you have to mols of what you want.
19.1 mols H2O x (4 mols H2/2 mols H2O) = 19.1 x 4/2 = 19.1 x 2 = 38.2 mols H2 gas produced.