Balance the following chemical equations and separate the coefficients by commas and a space respectively (put a 1 if the coefficient is assumed 1): Mg(s)+P4(s)→Mg3P2(s) Explanation: Al(s)+N2(s)→AlN(s) Explanation: 5.2.1 Balancing with polyatomic ions We can balance each atom like we did in the previous example but sometimes it becomes very cumbersome especially when we have the same atom in different compounds. Let’s look at the following reaction: YOU CAN DO THIS, BUT IT WILL BE TEDIOUS: Na2SO4(aq) + Mg(NO3)2(aq) → MgSO4(s) + NaNO3(aq) 2 Na atoms 1 S atom 1 Mg atom 2 N atoms 10 O atoms (4 from SO4 and 6 from (NO3)2) 1 Na atom 1 S atom 1 Mg atom 1 N atom 7 O atoms (4 from SO4 and 3 from NO3) This will become …show more content…
very difficult if we balance by oxygen but since SO42- and NO3- remain intact on both sides of the reaction, we can balance for them instead of each atom. This will also alleviate the need to balance for N and S but we will still need to balance for Mg and Na since they are not part of a polyatomic ion. SO DO THIS INSTEAD: Na2SO4(aq) + Mg(NO3)2(aq) → MgSO4(s) + NaNO3(aq) 2 Na atoms 1 SO42– ion 1 Mg atom 2 NO3– ions 1 Na atom 1 SO42– ion 1 Mg atom 1 NO3– ion Since SO4 and Mg are balanced we will start with Na. You could start with NO3 if you want, I just chose Na. Na2SO4(aq) + Mg(NO3)2(aq) → MgSO4(s) + 2 NaNO3(aq) 2 Na atoms 1 SO42– ion 1 Mg atom 2 NO3– ions 2 Na atoms 1 SO42– ion 1 Mg atom 2 NO3– ions By balancing Na, we balanced NO3 too and our equation is balanced.
This will often be the case with ionic reactions but not always. Remember there is no magic trick that works all the time. Let’s take a look at this reaction: (NH4)3PO4(aq) + Ca(ClO4)2(aq) → Ca3(PO4)2(s) + NH4ClO4(aq) 3 NH4+ ions 1 PO43– ion 1 Ca atom 2 ClO4– ions 1 NH4+ ion 2 PO43– ions 3 Ca atoms 1 ClO4– ion Since NH4+ and ClO4– are in a one to one ratio for NH4ClO4 on the products side and there are 3 NH4+ ions and 2 ClO4– ions on the reactants side we can put a 6 in front of NH4ClO4 and then balance to make 6 NH4+ ions and 6 ClO4– ions by putting a 2 in front of (NH4)3PO4 and a 3 in front of Ca(ClO4)2 and see how that works. 2 (NH4)3PO4(aq) + 3 Ca(ClO4)2(aq) → Ca3(PO4)2(s) + 6 NH4ClO4(aq) 6 NH4+ ions 2 PO43– ions 3 Ca atoms 6 ClO4– ions 6 NH4+ ions 2 PO43– ions 3 Ca atoms 6 ClO4– ions By balancing the two polyatomic ions the rest of the ions are balanced as well. Again, this is often the case but not always. Quick Check: 5.2.1.a Balance the following chemical equations and separate the coefficients by commas and a space respectively (put a 1 if the coefficient is assumed 1): …show more content…
Li2CO3(aq)+Fe2(SO4)3(aq)→Fe2(CO3)3(s)+Li2SO4(aq) Explanation: AlCl3(aq)+K3PO4(aq)→AlPO4(s)+KCl(aq) Explanation: Balancing reactions with covalent compounds can be a little tricky because sometimes an atom will appear in more than one compound either on the product or reactants side.
Hydrazine (N2H4) is a flammable liquid used in rocket fuel. Balance the chemical reaction which shows its formation from nitrogen gas and ammonia. NH3(l) + N2(g) → N2H4(l) 3 N atoms 3 H
atoms 2 N atoms 4 H atoms Since N is in two molecules on the reactants side we will balance for H first. In general, when an atom is present in two or more compounds or molecules, you balance it last. We see that hydrogen comes in groups of 3 and 4 in NH3 and N2H4, respectively, so we will place a 4 in front of NH3 and a 3 in front of N2H4. 4 NH3(l) + N2(g) → 3 N2H4(l) 6 N atoms 12 H atoms 6 N atoms 12 H atoms By doing that, N became balanced as well. Propane (C3H8) is used for cooking on a grill outside. It undergoes what is called a combustion reaction to form CO2 and H2O. Balance the chemical reaction: C3H8(g) + O2(g) → CO2(g) + H2O(l) 3 C atoms 8 H atoms 2 O atoms 1 C atom 2 H atoms 3 O atoms Like before since we see that O is in two different places on the products side, we will balance that last. Also since there is only one C in CO2 and 3 Cs and 8 Hs in C3H8 and 2 Hs in H2O we will balance C first by putting a 3 in front of CO2. C3H8(g) + O2(g) → 3 CO2(g) + H2O(l) 3 C atoms 8 H atoms 2 O atoms 3 C atoms 2 H atoms 7 O atoms Now let’s balance H. We see there are 8 Hs on the reactants side and 2 Hs on the products side so we will put a 4 in front of water. C3H8(g) + O2(g) → 3 CO2(g) + 4 H2O(l) 3 C atoms 8 H atoms 2 O atoms 3 C atoms 8 H atoms 10 O atoms Now we have 10 O atoms on the products side so we will put a 5 in front of the O2 to give us a total of 10 O atoms. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l) 3 C atoms 8 H atoms 10 O atoms 3 C atoms 8 H atoms 10 O atoms Carbon monoxide and nitrogen monoxide are toxic gases and are by-products of fuel combustion. The catalytic converter in your car converts them into carbon dioxide and nitrogen which are not toxic. Balance the chemical reaction: NO(g) + CO(g) → N2(g) + CO2(g) 1 N atom 2 O atoms 1 C atom 2 N atoms 2 O atoms 1 C atom Since the only atom not balanced is N we will start with that but we can see that since oxygen is in two of the reagents anything we do to N and C will affect O, so we will worry about O last. 2 NO(g) + CO(g) → N2(g) + CO2(g) 2 N atoms 3 O atoms 1 C atom 2 N atoms 2 O atoms 1 C atom We now have N and C balanced but not O. We need one more O on the product side but can only increase the number of O atoms on the products side in multiple of 2s. So if we put a 2 in front of CO2 and a 2 in front of CO we will have all our atoms balanced. 2 NO(g) + 2 CO(g) → N2(g) + 2 CO2(g) 2 N atoms 4 O atoms 2 C atoms 2 N atoms 4 O atoms 2 C atoms Quick Check: 5.2.1.b
The question I was trying to answer is Which balanced chemical equation best represents the thermal decomposition of sodium bicarbonate. Using that question to guide us we were trying to determine which of the four chemical equations show how atoms are rearranged during thermal decomposition. We concluded it was the second chemical equation, we know that because:
An elements¡¦ reaction to certain substances may be predicted by its placement on the Periodic Table of Elements. Across a period, an element on the left will react with more vigor than one on the right, of the same period. Vertically, as elements are sectioned into groups, the reaction of each element increases as you move down in the same group. With this in mind, the reactions of the substances involved in this experiment may be hypothesized, observed, and validated.
It is important however to note that the NH4 and K ions are still in
I will not add a catalyst to my solution and I will not stir my solution. · I will use 25cm3 of hydrochloric acid. · I will use 1g of calcium carbonate.
If I were to roughly plot a graph for the reaction, it would look like
CaCl2 + H2O + CO2
Reaction 2: H = 50 x 4.18 x -10.3" H = -2152.7 This value is for 1.37g of calcium oxide, not 56.1g, which is its relative molecular mass. Therefore: H =
Na2S203 (aq) + 2HCl (aq) -> 2NaCl (aq) + H20 (l) + SO2 (g) + S (s)
NaOH(aq)Â Â Â Â Â Â Â Â +Â Â Â Â Â Â Â Â Â HCl(aq)Â Â Â Â Â Â Â Â Â Â Â Â Â Ã Â Â Â Â Â Â Â Â Â Â Â Â NaCl(aq) Â Â Â Â Â Â + Â Â Â H2O(l).
In the reaction, potassium peroxodisulphate and potassium iodide will be used to provide the peroxodisulphate ions and iodide ions respectively. The ionic formula for the reaction is as follows:
According to the principle of charge balance, there must be equal number of cationic and anionic (H+ and K+) species in the PBX solution. Fig. 5 show that the concentration of IC was maintained at 0 mg/L during the entire oxidation process, indicating that there is no CO32- and HCO3- in this solution. The ion
Cl- (aq) + Na+ (aq) + OH- (aq) Na+ (aq) + Cl- (aq) +H+ + OH- [IMAGE]The above is an example of a neutralization reaction, involving an acid and an alkali. The result is a salt and water. In every neutralization reaction, the metal in the alkali (Na+ here) takes the place oh the hydrogen in the acid, forming a metal compound called a salt.
0.1M HCl, 10 mL of 0.1N KMnO4, 0.2 g. KI, 5 mL of alcohol, and 5 mL of
The pH of the solution would alter the rate of the reaction if it was
C6H12O6 + 2 ADP + 4 H+ → 2 C2H5OH + 2 CO2 + 2 ATP + 2 H2O