If 200.0 g of copper(II) sulfate react with an excess of zinc metal, what is the theoretical yield of copper?
Answers
Answer:
The theoretical yield of copper is 79.6281 g
Explanation:
Moles of copper sulfate =
According to reaction 1 mol of copper sulfate gives 1 mol of copper .
Then 1.2530 mol of copper sulfate will gives :
of copper .
Mass of 1.2530 mol of copper :
1.2530 mol × 63.55 g/mol = 79.6281 g
The theoretical yield of copper is 79.6281 g
Related Questions
Describe 3 ways that you could change the rate of the reaction based on principles that effect rates of reactions.
Who was the first to propose the existence of atoms? John Dalton Democritus Joseph Proust Ernest Rutherford
Hanna hypothesizes that granite is denser than sandstone. How can Hanna test her hypothesis?
Yesterday we combined Hydrochloric Acid HCl with Sodium Hydroxide NaOH in a violent reaction that resulted in water H2O and common table salt NaCl. How many grams of hydrochloric acid should we use so we have exactly enough to react with 40g of sodium hydroxide? You'll need to write a chemical reaction, balance it, and then perform your calculation. also how many grams of salt NaCl will be produced and how many grams of water H2O be produced?
Answers
Answer:
355 ml
Explanation:
because a can of soda could't hold more than that measure.
B. 3 billion years
C. 4 billion years
D. 4.5 billion years
Answers
has stopped?
Answers
Answer:
Ammonia is limiting reactant
Amount of oxygen left = 0.035 mol
Explanation:
Given data:
Masa of ammonia = 2.00 g
Mass of oxygen = 4.00 g
Which is limiting reactant = ?
Excess reactant's amount left = ?
Solution:
Balance chemical equation:
4NH₃ + 3O₂ → 2N₂ + 6H₂O
Number of moles of ammonia:
Number of moles = mass/molar mass
Number of moles = 2.00 g/ 17 g/mol
Number of moles = 0.12 mol
Number of moles of oxygen:
Number of moles = mass/molar mass
Number of moles = 4.00 g/ 32 g/mol
Number of moles = 0.125 mol
Now we will compare the moles of ammonia and oxygen with water and nitrogen.
NH₃ : N₂
4 : 2
0.12 : 2/4×0.12 = 0.06
NH₃ : H₂O
4 : 6
0.12 : 6/4×0.12 = 0.18
O₂ : N₂
3 : 2
0.125 : 2/3×0.125 = 0.08
O₂ : H₂O
3 : 6
0.125 : 6/3×0.125 = 0.25
The number of moles of water and nitrogen formed by ammonia are less thus ammonia will be limiting reactant.
Amount of oxygen left:
NH₃ : O₂
4 : 3
0.12 : 3/4×0.12= 0.09
Amount of oxygen react = 0.09 mol
Amount of oxygen left = 0.125 - 0.09 = 0.035 mol
Final answer:
The limiting reactant in the reaction between Ammonia and Oxygen is Ammonia (NH3). All of the Oxygen is used up in the reaction, so no excess reactant remains.
Explanation:
This question involves a concept in chemistry known as limiting reactants and stoichiometry. The balanced chemical reaction between Ammonia (NH3) and Oxygen (O2) is: 4NH3 + 5O2 -> 4NO + 6H2O. This indicates that 4 moles of NH3 react with 5 moles of O2.
To find the limiting reactant, you first need to convert the grams of your reactants to moles. The molar mass of NH3 is approximately 17.0g/mol, and the molar mass of O2 is 32.0g/mol. Therefore, you have 2.00g/17.0g/mol = 0.118 moles of NH3 and 4.00g/32.0g/mol = 0.125 moles of O2.
Since 5 moles of O2 are needed for every 4 moles of NH3, and we have slightly more O2 than NH3, the limiting reactant is NH3. To find the amount of excess reactant, we determine how much O2 actually reacted by multiplying (0.118 moles NH3)*(5 moles O2/4 moles NH3) = 0.1475 moles O2. The original amount of O2 was 0.125 moles, so the amount left over is 0.125 - 0.1475, which is a negative number and thus not possible. This confirms that O2 is the excess reactant, although it entirely reacted. Hence, no excess reactant remains.
Learn more about Limiting Reactant here:
#SPJ3
Answers
Final answer:
Subatomic particles are particles smaller than an atom. Therefore, any element or matter larger than these particles such as molecules, compounds, or cells can be considered as non-examples.
Explanation:
The question asks for non-examples of subatomic particles, that is, elements that do not fall within the category of subatomic particles. Subatomic particles are particles smaller than an atom, such as protons, neutrons, and electrons. Therefore, any element or matter larger than an atom would be a non-example of a subatomic particle.
Examples of non-examples include molecules like water (H2O), oxygen (O2), or carbon dioxide (CO2). These are made up of multiple atoms and thus are larger than individual subatomic particles. Similarly, compounds like salt (NaCl) or sugar (C12H22O11) are also non-examples because they are made of multiple atoms as well. Cells, the basic structural units of living organisms, are much larger than subatomic particles and also represent non-examples.
Learn more about subatomic particles here:
#SPJ6
Answers
Exothermic changes: the system heats the surrounding. the heat absorbed by
the surroundings increase the freedom of motion of the particles which
increases the entropy of the surrounding. therefore qsys < 0 , qsurr > 0
and delt S > 0 .
the explanation:
the exothermic reaction is a chemical reaction which releases heat, and the
heat is one of its products in the reaction. So the system here released heat
and the surroundings will absorb it.
-in the exothermic reaction, the enthalpy in the surroundings will increase,
as ΔSsurr = -ΔH/T and when ΔH in the exothermic reaction has a negative
sign( - ) so, ΔSsurr has to be +Ve ( positive sign) ∴ ΔSsurr > 0 .
-and when the system released the heat and the surroundings absorbed it this affects the freedom of motion of the particles and make it increase and this will affect the entropy and make it increase.
- in exothermic reaction when the system released heat and the surroundings absorbed it will increase the thermal disorder in the surrounding which makes
ΔSsurr >0 and qsys <0 & qsurr >0 as qsurr = - qsys
when ΔSsurr is proportional to the amount of heat transferred
∴ΔSsurr α qsurr and ΔSurr α - q sys
so when ΔSsurr has a positive sign in the exothermic reaction so qsurr >0
and qsys<0.
Answers
Final answer:
The reaction PCl5 + 4H2O -> H3PO4 + 5HCl involves 5 moles of HCl and 4 moles of water. Thus, for every mole of HCl produced, 0.8 moles of water is consumed. Hence, in this scenario, 2.76 moles of water would have been consumed to produce 3.45 moles of HCl.
Explanation:
In the balanced equation, PCl5 + 4H2O -> H3PO4 + 5HCl, you notice that 4 moles of water react with PCl5 to produce 5 moles of HCl. This means for every mole of HCl produced, 0.8 moles of water would have been consumed (4 moles / 5 moles).
So, if the reaction results in 3.45 moles of HCl, we can calculate the number of moles of water that reacted by multiplying the moles of HCl by 0.8. This gives us 2.76 moles of water.
Learn more about Mole Ratio here:
#SPJ12
Final answer:
By creating a proportion based on the balanced chemical equation, it is determined that 2.76 moles of water reacted with PCl5 to produce 3.45 moles of HCl.
Explanation:
To determine how many moles of water reacted if 3.45 moles of HCl are produced, we refer to the balanced chemical equation:
PCl5 + 4H2O → H3PO4 + 5HClAccording to the equation, for every 5 moles of HCl produced, 4 moles of water are needed. Therefore, you can set up a proportion to calculate the moles of water:
- (Moles of HCl produced / Moles of HCl in the equation) = (Moles of H2O reacted / Moles of H2O in the equation)
- (3.45 moles HCl / 5 moles HCl) = (x moles H2O / 4 moles H2O)
Solving for x gives you the number of moles of water that reacted:
x = (3.45 moles HCl × 4 moles H2O) / 5Thus, x = 2.76 moles of H2O.
Learn more about Stoichiometry here:
#SPJ3