From b86be11153644ad5522ff836091f7659b47c35e7 Mon Sep 17 00:00:00 2001
From: Andrew Lorimer <andrew@lorimer.id.au>
Date: Mon, 4 Feb 2019 11:21:19 +1100
Subject: [PATCH 1/1] standard conditions for gases

---
 chem/gas.md | 24 +++++++++++++++++++++++-
 1 file changed, 23 insertions(+), 1 deletion(-)

diff --git a/chem/gas.md b/chem/gas.md
index 6b7580e..4cd5689 100644
--- a/chem/gas.md
+++ b/chem/gas.md
@@ -4,4 +4,26 @@
 
 $$PV=nRT$$
 
-where $R =$ universal gas constant $= 8.31 \text{J} \text{K}^{-1} \text{mol}^{-1}$
\ No newline at end of file
+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
+$n$ is no of mol of gas
+
+
+- **Standard temperature and pressure (STP)** - standard temperature is 0 $^\circ$ C or 273 K. Standar dpressure is 100.0 kPa
+- **Standard laboratory conditions (SLC)** - temperature 25 $^\circ$ C (298K), pressure 100.0 kPa
+
+## Molar gas volume
+
+> 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**
+
+$$n={V \over V_M}$$
+
+where $n$ = number of mol  
+$V$ = actual volume (in litres)  
+$V_m$ = molar volume of gas
+
+$$\therefore n_{SLC} = {V \over 24.8}$$
-- 
2.47.1