Cheatography
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Guide to Chapters 1.1, 1.2 and 1.3 in IB Chem DP1
Includes: Finding moles, volume and concentration
Limiting and excess reagents
Titrations and STandard solutions
Ideal Gas Law
This is a draft cheat sheet. It is a work in progress and is not finished yet.
Formulas
No. of molecules = n [no. of moles] x A [Avogadro's Constant] |
No. of moles (n) = Mass (m)/ Molar Mass (Mr) |
No. of Atoms = No. of Molecules [n x A] x Atomicity |
No. of moles (n) = Volume (dm3) / Molar volume (STP or RTP) |
% yield = [Experimental yield/ Theoretical Yield] x 100 |
C [molarity] = no. of moles [n]/ Volume of concentration [v] |
Ideal Gas Law - PV = nRT |
Volume/concentration constant - C1V1 = C2V2 |
Finding Percentage Yield of a Reaction
Note: % yield always applies on PRODUCTS |
1: In any situation, first determine which of the products is the limiting reagent |
2: Using the compound which is limiting, form a ration such that [limiting reactant : product] |
3: Under the ratio, write the coefficient ratio of reactant : product |
4: Add the molar mass OF 1 MOLE |
5: Multiply the Molar mass with the number of moles = mass value |
6: Cross multiply to find the THEORETICAL YIELD |
7: Use the mass of the product given in the question - (EXPERIMENTAL YIELD) |
8: Substitute in the formula: [Experimental Yield/ Theoretical Yield] x 100 to find % yield |
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How to Find the Limiting Reagent
Step 1: Write down the whole equation |
Step 2: Balance the entire equation |
Step 3: Using the balanced equation, determine the coefficient ratio of the reactants |
Step 4: Write down the ratios of the values given in the question |
Step 5: Convert the amounts to moles |
Step 6: divide the values (mole ratio / coefficient ratio) |
Ans: The smallest value is the limiting reagent |
Ideal Gas Law
PV = nRT; where |
P - Pressure (Pa) |
V = Volume (m3) |
T - Temperature (K) *Take celsius value and + 273 |
R - Constant (8.31 JK/mol) |
n - no. of moles (mol) |
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Molar Volume Values
STP - Standard Temperature and Pressure |
RTP - Room Temperature and Pressure |
Temp.: 0 degrees Celsius |
Temp.: 20 degrees Celsius |
Pressure: 1 atm |
Pressure = approx. 1atm |
Volume: 22.7 dm3 |
Volume: 24 dm3 |
Ideal Gas vs. Real Gas
Ideal Gas |
Real Gas |
Obeys all gas laws |
All properties change |
No forces of attraction |
Forces of attraction |
Collide in straight lines |
Collision in random motion |
No mass or volume |
High Temperature |
Low Temperature |
Low Pressure |
High Pressure |
High Volume |
Low Volume |
Steps to Find a Standard Solution
Standard Solution: a solution of accurately known concentration |
Step 1: Weigh a known amount of solute |
Step 2: Dissolve the Solute in a minimal amount of water |
Step 3: Transfer the solution to a volumetric flask without washing |
Step 4: Make the solution fill the flask till the meniscus reaches accurate value |
Step 5: Place stopper and invert into mix solution |
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