Answer:
Mg(s) + 2H^+(aq) ----> Mg^2+(aq) + H2(g)
Explanation:
We must first write the molecular equation, then obtain the complete ionic equation and subsequently get the net ionic equation as shown below;
Molecular reaction equation;
Mg(s) + 2HCl(aq) ------> MgCl2(aq) + H2(g)
Complete ionic equation;
Mg(s) + 2H^+(aq) + 2Cl^-(aq) ----> Mg^2+(aq) + 2Cl^-(aq) + H2(g)
Net ionic equation;
Mg(s) + 2H^+(aq) ----> Mg^2+(aq) + H2(g)
36) HCl(aq)+KOH(aq)⇒H₂O(l)+KCl(aq)
37) You can use the equation M₁V₁=M₂V₂
M₁=concentration of acid
V₁=volume of acid in orginal solution
M₂=concentration of base
V₂= the volume of based used to neutralize the acid
M₁=(0.150M KOH x 0.0185L KOH)/0.025L HCl
M₁=0.111M HCl
This equation works since we no based off of the formula in question 36 that 1 mole of KOH will neutralize 1 mole of HCl and <span>M₂V₂ is equal to the moles KOH which means it needs to equal M</span>₁V₁ since that is the number of moles HCl. (if moles HCl did not equal moles KOH the solution would not be neutralized).
Answer:
There is one scientific method
it starts with an
OBSERVATION
then a HYPOTHESIS
which goes to planning, creating an EXPERIMENT
and finally a conclusion for your results
Explanation:
<span> endothermic is the answer
</span>
The empirical formula of the metal iodide is Cr2I.
Mass of Chromium = 23.98
Molar Mass of Chromium = 51.9961
= 0.461 mol
Molar Mass of iodide = 126.9
= 199.6-23.88/126 = 1.394
The ratio between
Chromium and iodinei is1:2.So, the empirical formula is therefore Cr2I
Empirical formula of a chemical compound is the simplest whole number ratio of atoms present in a compound.[1] A simple example of this concept is that the empirical formula of sulfur monoxide, or SO, would simply be SO, as is the empirical formula of disulfur dioxide, S2O2. Thus, sulfur monoxide and disulfur dioxide, both compounds of sulfur and oxygen, have the same empirical formula. However, their molecular formulas, which express the number of atoms in each molecule of a chemical compound, are not the same.
Learn more about Empirical formula here:
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