Answer:
4. gives the relative number of atoms of each element per formula unit
Explanation:
An empirical formula -
It refers to the formula which determined the simplest whole - number ratio of all the atoms in a given species , is referred to as an empirical formula .
In simple terms ,
It is he smallest formula of the whole number which when multiplied by some whole number gives the actual structure of the compound .
Hence , from the given information of the question ,
The correct option for empirical formula is 4.
Cause their are both have difference s
Answer:
i) The pCa before initiating the titration is 2.6
ii) The pCa is 6.67
Explanation:
please look at the solution in the attached Word file
<u>Answer:</u>
All of the limiting reagent gets used up causes the percent yield of a reaction to be less than 100%
<u>Explanation:</u>
It is rare for a chemical reaction to occur with the right proportion of reactants that reacts together to form resultant products.During this process, one of the reactants gets used up faster resulting in the lower percent yield. Such product that gets used up faster is called limiting reagent. This limiting reagent is responsible for lowering the percentage yield in the chemical reaction.
The limiting reactant can be found easily by calculating the yield of each reactant assuming they are consumed completely. The reactant which has least yield is the limiting reactant of the reaction.
Answer:
2.52 g H₂
Explanation:
To find the mass of hydrogen gas, you need to (1) convert moles H₂O to moles H₂ (via mole-to-mole ratio from reaction coefficient) and then (2) convert moles H₂ to grams H₂ (via molar mass from periodic table values). When multiplying the given value by the mole-to-mole ratio, you need to use the coefficients of the balanced equation. An reaction is balanced once there is an equal amount of each element on both sides.
<u>(Step 1)</u>
The unbalanced equation:
Ca(s) + H₂O(l) ----> Ca(OH)₂(aq) + H₂(g)
<u>Reactants</u>: 1 calcium, 2 hydrogen, 1 oxygen
<u>Products</u>: 1 calcium, 4 hydrogen, 2 oxygen
The balanced equation:
1 Ca(s) + 2 H₂O(l) ----> 1 Ca(OH)₂(aq) + 1 H₂(g)
<u>Reactants</u>: 1 calcium, 4 hydrogen, 2 oxygen
<u>Products</u>: 1 calcium, 4 hydrogen, 2 oxygen
<u>(Step 2)</u>
Molar Mass (H₂): 2(1.008 g/mol)
Molar Mass (H₂): 2.016 g/mol
<u>(Step 3)</u>
2.50 moles H₂O 1 mole H₂ 2.016 g
--------------------------- x ------------------------- x ---------------------- = 2.52 g H₂
2 moles H₂O 1 mole