Good morning. I need help solving 2 problems for chemistry. For #1 I need someone to check my work and tell me if I did it wrong and show me how and where I went wrong. And for #2 I need someone to help me figure out how to solve it and explain.
1. With the balanced equation below:
2Al+3FeO—>3Fe+Al2O3
Calculate the moles of aluminum that are needed to react completely with 13.2 moles of FeO
[My answer/work]
FeO: Al
3:2
13.2 divides by 3 x 2 =8.8
(I’m not sure if I’m correct or not but can someone help me.)
2. Sodium and water react according to the equation if 13.5g of sodium are added to excess water how many liters of hydrogen gas are formed at stp 2na+2h2o—>2naoh+h2
(I mainly need help solving this one. Can someone please help me)
2Al + 3FeO ==> 3Fe + Al2O3
You have 13.2 mol FeO. Use the coefficients in the balanced equation to convert mols of what you want.
13.2 mol Al x (2 mol Al/3 mols FeO) = 13.2 x 2/3 = 8.8 and you answer is correct; however, I don't like the way you got there. If I do your math I see
13.2/3*2 = 13.2/6 = 2.2. Actually, you meant to write [13.2/3]*2 or 13.2 x 2/3.
For equations you need to find the caps key and use it. Technically, your equation means nothing to me. Co is cobalt, CO is carbon monoxide, and co is the abbreviation for company so it makes a difference in what you're trying to say.
2Na + 2H2O ==> 2NaOH + H2
1. Write and balance the equation. You've done that.
2. Convert what you have (13.5 g Na) to mols. mol = grams/atomic mass = ?
3. Using the coefficients (as in the previous problem) to convert mols of what you have (in this case Na) to mols mols of what you wnt (in this case H2).
4. Now convert mols H2 to units you want. In this case you want volume so
a. mols H2 x 22.4 L/mol = ? L H2.
b. Some problems ask for grams. In that case, then mols H2 x molar mass H2 = g H2.
Print this procedure out. It will work ALL of your simple stoichiometry problems. It will not do limiting reagent problems with with a tweak or two it will.
Good morning! I'll be happy to help you with both of your chemistry problems. Let's start with problem #1.
In this problem, you are given a balanced equation and asked to calculate the moles of aluminum needed to react completely with a given amount of FeO. The balanced equation you provided is:
2Al + 3FeO -> 3Fe + Al2O3
To solve this problem, you need to use the stoichiometry of the balanced equation. The stoichiometric coefficients indicate the ratio of moles between the reactants and products. In this case, the coefficient of Al is 2, while the coefficient of FeO is 3.
To find the moles of aluminum needed, you can set up a proportion using the stoichiometric coefficients:
(2 moles Al / 3 moles FeO) = (x moles Al / 13.2 moles FeO)
Cross-multiplying and solving for x, we get:
x = (2 moles Al / 3 moles FeO) * 13.2 moles FeO
x = 8.8 moles Al
So, the correct answer is 8.8 moles of aluminum.
Now let's move on to problem #2.
In this problem, you are given the equation for the reaction between sodium and water, and you need to determine the volume of hydrogen gas produced when 13.5g of sodium reacts with excess water. The balanced equation you provided is:
2Na + 2H2O -> 2NaOH + H2
To solve this problem, we need to use the concept of molar mass and the ideal gas law. Here are the steps to follow:
1. Convert the given mass of sodium (13.5g) to moles. To do this, divide the mass by the molar mass of sodium (22.99 g/mol). This gives you the number of moles of sodium.
2. Use the stoichiometry of the balanced equation to relate the moles of sodium to the moles of hydrogen gas. From the balanced equation, you can see that 2 moles of sodium react to produce 1 mole of hydrogen gas.
3. Apply the ideal gas law, which states that PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/(mol·K)), and T is the temperature in Kelvin. At STP (standard temperature and pressure), T is 273.15K, and the pressure is 1 atm.
4. Since we are given the number of moles of hydrogen gas, we can rearrange the ideal gas law to solve for volume (V). It becomes V = (nRT)/P, where n is the number of moles, R is the gas constant, T is the temperature, and P is the pressure.
By plugging in the values and solving the equation, you will find the volume of hydrogen gas produced at STP.
I hope this explanation helps you understand how to solve these problems. Let me know if you have any other questions or need further clarification!