JLH Chem Ch 5 Flashcards
Consider the reaction of hydrogen and oxygen to form water, according to the balanced equation: 2 H2 + O2 –> 2 H2O. Identify the limiting reactant in the molecular art.
Count how many molecules each: 3 O2 4 H2
Consider the reaction of hydrogen and nitrogen to form ammonia, according to the balanced equation:
3 H2 + N2 -→ 2 NH3
Identify the limiting reactant in the molecular art.
H2 is the limiting reactant
Using the balanced equation for the reaction of H2 with O2 to form H2O, determine the limiting reactant with
5.0 mol H2 and 5.0 mol O2
H2 is the limiting reactant
Using the balanced equation for the reaction of H2 with O2 to form H2O, determine the limiting reactant with
8.0 mol H2 and 2.0 mol O2
O2 is the limiting reactant
The amount of A2, the limiting reactant, determines how much AB can form. Because the balanced equation shows that each A2 molecule forms two AB molecules, three A2 molecules form how many AB molecules?
six AB molecules
Using the balanced equation, 3 H2 + N2 -→ 2 NH3
Calculate the number of moles of product formed from 5.0 moles of H2 and 3.0 moles of N2
Identify H2 as the original quantity and use the mole ratio from the balanced equation as a conversion factor to calculate how much N2 is needed for complete reaction.
Using the balanced equation, 3 H2 + N2 -→ 2 NH3, calculate the number of moles of product formed with
1.0 mole H2 and 2.0 mol N2
0.67 mol
Using the balanced equation, N2 + O2 -→ 2 NO,
determine the limiting reactant when 10.0 g of N2 (molar mass 28.02 g/mol) react with 10.0 g of O2 (molar mass 32.00 g/mol)
Using the balanced equation, N2 + O2 -→ 2 NO,
determine the limiting reactant for:
12.5 g N2 and 15.0 g O2
(N2 molar mass 28.02 g/mol; O2 molar mass 32.00 g/mol)
N2
Using the balanced equation, N2 + O2 -→ 2NO,
calculate the number of grams of NO (molar mass 30.01 g/mol) formed when 10.0 g of N2 (molar mass 28.02 g/mol) react with 10.0 g of O2 (molar mass 32.00 g/mol)
1st, determine the limiting reactant (O2)
Using the balanced equation, N2 + O2 -→ 2 NO,
determine the limiting reactant:
12.5 g N2 and 15.0 g O2
(N2 molar mass 28.02 g/mol; O2, molar mass 32.00 g/mol)
N2
Using the balanced equation, N2 + O2 -→ 2 NO,
calculate the number of grams of NO (molar mass 30.01 g/mol) formed when 10.0 g of N2 (molar mass 28.02 g/mol) react with 10.0 g of O2 (molar mass 32.00 g/mol)
1st, determine limiting factor (O2)
How many of each atom is in
C2H6O + 3O2
2 C
6 H
7 O
How many of each atom is in
Mg3 (PO4)2
3 Mg
2 P
8 O
How do we balance this equation?
C3H8 + O2 -> CO2 + H2O
Place coefficient 3 before CO2 on right side
Place coefficient 4 before H2O on right side
Place coefficient 5 before O2 on left side
balance this equation
C6H12O6 + O2 –> CO2 + H2O
C6H12O6 + O2 –> CO2 + H2O
The airbag in an automobile inflates when ionic sodium azide (NaN3) rapidly decomposes to sodium (Na) and gaseous N2.
Write a balanced equation for this reaction.
write a balanced equation for the reaction of ethane (C2H6) with O2 to form CO2 and H2O
balance the equation (card 29)
Ca3 (PO4)2 + H2SO4 –>
CaSO4 + H3PO4
CuCO3 –> CuO + CO2
is this a combination or decomposition?
decomposition
The reaction of zinc with CuCL2 [copper(II) chloride] to form ZnCl2 (zinc chloride) and copper is a single replacement reaction. What element replaces what element in the compound CuCl2?
Zn replaces Cu in the compound CuCl2.
The reaction of BaCl2 (barium chloride) with K2CO3 (potassium carbonate) to form BaCO3 (barium carbonate) and KCl (potassium chloride) is a double replacement reaction. What ions in this reaction exchange parts?
The cations Ba2+ & K+ exchange places to form two new ionic compounds.
(in double replacement, two compounds are reactants & two compounds are products)
is CuO + 2 HCl -> CuCl2 + H2O a single replacement or double replacement?
Double replacement
The Cu2+ (in CuO) and H (in HCl) exchange to form two new compounds.
is Zn + 2 HCl -> ZnCl2 + H2 a single or double replacement reaction?
single replacement
The element Zn replaces the H atom in HCl to form a new compound & new element
The nonmetals O2 and Cl2 readily gain electrons to form 2 O2- and 2 Cl-, respectively; that is, they are
reduced
A positively charged ion like Cu2+ is _______ to Cu by _______ two electrons, whereas two negatively charged Cl- anions are ________ to Cl2 by ______ two electrons.
A positively charged ion like Cu2+ is reduced to Cu by gaining two electrons, whereas two negatively charged Cl- anions are oxidized to Cl2 by losing two electrons.
If Cu2+ gains two electrons to form Cu, it is said to be…
reduced
If Zn loses electrons to Cu2+. Which one is the reducing agent and which one is the oxidizing agent?
Zn is the reducing agent
Cu2+ is the oxidizing agent
The metals sodium (Na) and magnesium (Mg) readily lose electrons to form the cations Na+ and Mg2+, respectively; that is, they are
oxidized
The nonmetals O2 and Cl2 readily gain electrons to form 2 O2- and 2 Cl-, respectively; that is, they are
reduced
A positively charged ion like Cu2+ is _______ to Cu by _______ two electrons, whereas two negatively charged Cl- anions are ________ to Cl2 by ______ two electrons.
A positively charged ion like Cu2+ is reduced to Cu by gaining two electrons, whereas two negatively charged Cl- anions are oxidized to Cl2 by losing two electrons.
Identify what is oxidized and what is reduced in the following reaction
Mg + 2 H+ -> Mg2+ + H2
Zn + 2H+ -> Zn2+ + H2
Identify what is oxidized and what is reduced
write out half equations to show how many electrons are gained or lost by each species
Zn = oxidized
2H+ = reduced
