How do you balance a chemical equation
1 answer:
There should be mass balance and the charge balance between the reactants and the products
Mass balance : total no of individual atoms of each type should be balanced before and after the reaction
Charge balance : Overall charge of the reactants should be balanced with the overall charge of the products
You can balance,
1)by just looking at it
2)by Algebraic method given above or
3)by the redox method
You need to know how to get the oxidation numbers in order to use the oxidation method
Mass balance : total no of individual atoms of each type should be balanced before and after the reaction
Charge balance : Overall charge of the reactants should be balanced with the overall charge of the products
You can balance,
1)by just looking at it
2)by Algebraic method given above or
3)by the redox method
You need to know how to get the oxidation numbers in order to use the oxidation method
You might be interested in
Explanation:
We will balance equation which describes the reaction between sulfuric acid and sodium bicarbonate: as follows.
Next we will calculate how many moles of are present in 85.00 mL of 1.500 M sulfuric acid.
As, Molarity =
1.500 M =
n = 0.1275 mol
Now set up and solve a stoichiometric conversion from moles of to grams of
. As, the molar mass of
is 84.01 g/mol.
= 21.42 g
So unfortunately, 15.00 grams of sodium bicarbonate will "not" be sufficient to completely neutralize the acid. You would need an additional 6.42 grams to complete the task.
Answer:
Explanation:
Hello there!
In this case, according to the described chemical reaction, it is possible to compute the theoretical mass of silver as mass via the 1:2 mole ratio of copper to silver and their atomic mass in the periodic table, in order to perform the following stoichiometric setup:
Next, given the actual yield of 120 g, we compute the percent yield via:
Regards!
Answer:
Mole fraction SF₄: 0,121
Mole fraction CO₂: 0,879
Partial pressure SF₄: 0,134 atm
Partial pressure CO₂: 0,968 atm
Total pressure: 1,102 atm
Explanation:
The moles of sulfur tetrafluoride gas and carbon dioxide gas are:
5,29g SF₄×= <em>0,0489 moles SF₄</em>
15,6 CO₂×= <em>0,354 moles CO₂</em>
Mole fraction SF₄:
= <em>0,121</em>
Mole fraction CO₂:
= <em>0,879</em>
It is possible to obtain partial pressure of both gases with moles of each gas using:
P = nRT/V
Where n are respective moles, R is gas constant (<em>0,082atmL/molK</em>), T is teemperature (27°C=<em>300,15K</em>), V is volume (<em>9,0000L)</em>
Replacing:
Partial pressure SF₄: <em>0,134atm</em>
Partial pressure CO₂: <em>0,968atm</em>
Now, the sum of the partial pressures is the total pressure in the tank, that means:
Total pressure: 0,134atm + 0,968atm = <em>1,102atm</em>
<em></em>
I hope it helps!