First, determine the molar mass of the empirical formula given for the substance. This can be solved by adding the products of the number of moles and the molar mass of each of the atom as shown below,
M = (3 mols C)(12 g C/1 mol C) + (2 mols H)(1 g H/1 mol H) + (1 mol N)(14 g N/1 mol N)
M = 52 g/mol
Then, divide the given molar mass above by the calculated value.
n = 208.19 g/mol / 52 g/mol = 4
Then, multiply the value of n to the coefficients of the atoms giving us the answer.
<em> ANSWER: C₁₂H₈N₄</em>
The stoichiometry of the reaction gives the molar ratio in which the reactants react with each other and the ratio in which products are formed.
The coefficients of the reactants in the reaction follow the stoichiometry
the balanced chemical equation for the reaction is as follows;
2C₃H₆(g) + 9O₂(g) ---> 6CO₂(g) + 6H₂O(l)
Answer:
55.18 L
Explanation:
First we convert 113.4 g of NO₂ into moles, using its molar mass:
- 113.4 g ÷ 46 g/mol = 2.465 mol
Then we<u> use the PV=nRT formula</u>, where:
- P = 1atm & T = 273K (This means STP)
- R = 0.082 atm·L·mol⁻¹·K⁻¹
Input the data:
- 1 atm * V = 2.465 mol * 0.082atm·L·mol⁻¹·K⁻¹ * 273 K
And <u>solve for V</u>:
