molar volume

diff --git a/chem/gas.md b/chem/gas.md
index 1848d3885a4a7490e52e259d177d933c513f2dd2..3020896b239ebfcd342fa4ee1f22f5403939aace 100644 (file)
--- a/chem/gas.md
+++ b/chem/gas.md
@@ -8,10 +8,11 @@ $${P_1 V_1 \over T_1} = {P_2 V_2 \over T_2}$$
 
 $$PV=nRT$$
 
-where $R =$ universal gas constant $= 8.31 \text{J} \text{K}^{-1} \text{mol}^{-1}$  
-$P$ is measured in kPa
-$V$ is measured in L
-$T$ is measured in K
+where  
+$R =$ universal gas constant $= 8.31 \text{ J K}^{-1} \text{mol}^{-1}$  
+$P$ is measured in kPa  
+$V$ is measured in L  
+$T$ is measured in K  
 $n$ is no of mol of gas
 
 
@@ -22,7 +23,7 @@ $n$ is no of mol of gas
 
 > Equal volumes of all gases measured at the same temperature and pressure contain the same number of gas particles
 
-$\therefore$ 1 mole of any gas at SLC occupies 24.8L - **molar gas voluem**
+$\therefore$ 1 mole of any gas at SLC occupies 24.8L - **molar gas volume**
 
 $$n={V \over V_M}$$
 
@@ -31,3 +32,9 @@ $V$ = actual volume (in litres)
 $V_m$ = molar volume of gas
 
 $$\therefore n_{SLC} = {V \over 24.8}$$
+
+## Molar volume
+
+Volume of a mole of a gas - depends on pressure & temperature  
+Molar gas volume = $V_M = 24.8 \text{ L mol}^{-1}$ at SLC  
+Use $n = {V \over V_m}$ like $n={m \over M}$
\ No newline at end of file