0
How many moles of oxygen is left over after reaction of 6.33 mol calcium with 4.00 moles oxygen gas?
Piherring
Based on the balanced equation:
2Ca + O2 --> 2CaO
Two moles of calcium will be consumed for every one mole of oxygen used. This means that if 6.33 mol Ca is used, half this, or 3.165 mol O2 will be needed (use a simple proportion or dimensional analysis).
Subtract the amount of O2 used from 4.00.
Wiki User
∙ 12y ago
Add your answer:
Earn +20 pts
Suppose you react 6.33 mol calcium with 4.00 mol oxygen gas What the number of moles of oxygen left over after the reaction is complete?
Suppose we react 6.00 moles calcium with 4.00 mol oxygen gas. Determine the number of moles of oxygen left over after the reaction is complete.
When 10 moles of H2 are mixed with 10 moles of O2 what is the number of moles of water formed?
Write out the equation first: 10H2 + 10O2 --> xH2O Since there are 2 moles of Hydrogen for every mole of Oxygen and equal moles of both are given, the Hydrogen limits the reaction as the limiting reactant. 10 moles of Hydrogen can make 10 moles of H2O with 5 moles of Oxygen left over. Think of it logically: H2 is two hydrogen atoms and water needs two hydrogen atoms, so it is a one-to-one reaction.
Identify the number of moles of excess reagent left over when 4.821 moles of ironIII oxide are reacted with 5.591 moles of aluminum in the thermite reaction?
2.026 mole ironIII oxide
How many liters of oxygen are needed to exactly react with 27.8 g of methane at STP?
1) First find the number of moles of methane in 27.8 g using the molar mass.See the Related Question to the left of this answer "How do you convert from grams to moles and also from moles to grams?" to do that.2) Then write the balanced reaction. Methane (CH4) reacts with oxygen (O2) to form carbon dioxide (CO2) and water (H2O). See the related question "How do you balance a chemical reaction?" to do that.3) That will tell you the ratio of moles of methane to moles of oxygen (it will be 2 to 1). So from Part 1, multiply the number of moles of methane by 2 to get moles of oxygen. Then, use the Ideal Gas Law to find out how many liters that will take up at STP. Use the Related Question link "How do you solve Ideal Gas Law problems?" to do that.
Identify the number of moles of excess reagent left over when 6.258 moles of iron(III) oxide are reacted with 8.359 moles of aluminum in the thermite reaction?
2.079 mole iron(III) oxide
Suppose you react 6.33 mol calcium with 4.00 mol oxygen gas What the number of moles of oxygen left over after the reaction is complete?
Suppose we react 6.00 moles calcium with 4.00 mol oxygen gas. Determine the number of moles of oxygen left over after the reaction is complete.
When 10 moles of H2 are mixed with 10 moles of O2 what is the number of moles of water formed?
Write out the equation first: 10H2 + 10O2 --> xH2O Since there are 2 moles of Hydrogen for every mole of Oxygen and equal moles of both are given, the Hydrogen limits the reaction as the limiting reactant. 10 moles of Hydrogen can make 10 moles of H2O with 5 moles of Oxygen left over. Think of it logically: H2 is two hydrogen atoms and water needs two hydrogen atoms, so it is a one-to-one reaction.
What is the chemical reaction between calcium and hydrochloric acid?
Ca + 2HCl --> CaCl2 + H2O This wrong. There is no oxygen on the left side of this equation. So, Ca + 2HCl -> CaCl2 + H2
Identify the number of moles of excess reagent left over when 4.821 moles of ironIII oxide are reacted with 5.591 moles of aluminum in the thermite reaction?
2.026 mole ironIII oxide
How many liters of oxygen are needed to exactly react with 27.8 g of methane at STP?
1) First find the number of moles of methane in 27.8 g using the molar mass.See the Related Question to the left of this answer "How do you convert from grams to moles and also from moles to grams?" to do that.2) Then write the balanced reaction. Methane (CH4) reacts with oxygen (O2) to form carbon dioxide (CO2) and water (H2O). See the related question "How do you balance a chemical reaction?" to do that.3) That will tell you the ratio of moles of methane to moles of oxygen (it will be 2 to 1). So from Part 1, multiply the number of moles of methane by 2 to get moles of oxygen. Then, use the Ideal Gas Law to find out how many liters that will take up at STP. Use the Related Question link "How do you solve Ideal Gas Law problems?" to do that.
How many grams of oxygen are produced when 11.5 grams NO2 is formed?
You can't answer this question unless you know the the NO2 was formed FROM. You need to write the balanced reaction for the reaction and then use stoichiometry to solve for the amount of oxygen produce.See the Related Questions to the left for how to write a balanced reaction and how to use stoichiometry to solve this type of problem.
Identify the number of moles of excess reagent left over when 8.368 moles of iron III oxide are reacted with 9.825 moles of aluminum in the thermite reaction.?
3.456 mole iron(III) oxide
Identify the number of moles of excess reagent left over when 6.258 moles of iron(III) oxide are reacted with 8.359 moles of aluminum in the thermite reaction?
2.079 mole iron(III) oxide
How does varying the ratio of H2 to O2 affect this chemical reaction?
If the reaction is 2H2 + O2 = 2H20 then varying the ratio doesn't really affect the reaction. Let's throw out a ratio...you've got 20 moles of H2 and 10 moles of O2, which will give you 20 moles of water. If you were to change that to 20 moles of H2 and 15 moles of O2, you're still going to get 20 moles of water...but you'll have five moles of O2 left over that can't react with anything because there's no hydrogen left. Conversely, if you have an overage of hydrogen you will theoretically be left with excess hydrogen...the reality of hydrogen is it's reactive enough it will go out looking for something to do, and you'll get a second compound.
If you have 0.50 mole of Ca how many atoms are present?
What compound? Please copy your homework questions completely. How else can we help you cheat?To find the number of moles of oxygen (or any other element), multiply the number of atoms present on the molecule (in subscript) by the number of molecules present in the reaction (in standard script to the left of the molecule)In this case:2 H2 + O2 --> 2 H2OOn the reactant side (to the left of the arrow), there are 4 moles of hydrogen present because we have inserted 2 moles of diatomic hydrogen (multiply the subscript 2 by the standard script 2 to the left of the molecule). We can calculate that there are 2 moles of oxygen present because we have inserted one mole of diatomic oxygen. On the products side (the right side of the arrow) we produced 2 moles of water (indicated by the standard script 2 to the left of the molecule) Each molecule of water contains 2 molecules (2 moles) of hydrogen and one molecule (one mole) of oxygen. Thus, we have a balanced equation because this gives us 4 moles of hydrogen and 2 moles of oxygen, just like we had on the reactant side.The multipliers in standard script to the left of the molecule gives us the molar ratio. 2 moles of diatomic hydrogen react with 1 mole of diatomic oxygen to produce 2 moles of water. Thus, if we were to burn .5 moles of diatomic hydrogen in excess oxygen, we would produce .5 moles of water. This is because, by looking at our chemical equation, we see that the molar ratio of diatomic hydrogen to water is 2:2 (or 1:1). We would have .25 moles of oxygen because the ratio of hydrogen to oxygen is 4:2 (or 2:1).Were this the question on your homework, the answer would be ".25 moles"
What is a limited reactant?
With any chemical reaction you have reactants and products, for this question I'll use the example of the formation of water from it's parts, Hydrogen and Oxygen. The equation would look like this: 2H2 (g) + O2 (g) -> 2H2O (l) Let's say you start out with 3 moles of Hydrogen and 1 mole of Oxygen. From the reaction you can see that for every mole of O2 that reacts, 2 moles of H2 are reacted. This means that after your mole oxygen reacts, you are still left with a mole of excess Hydrogen. Thus, Hydrogen is considered the excess reactant, and Oxygen is considered the limited reactant. In short, the limited reactant is whichever reactant you will use up in the reaction first.
300 g of ammonia react with 36 moles of sulfuric acid to produce ammonia sulfate how many moles of excess sulfuric acid are left over after the reaction is complete?
26.9 - 27.4
