The total mass is the sum of the masses.
It is
5543 + 23.45 + 697.4 mg = 6263.85 mg
Answer: 6263.85 mg
Answer:
0.5 moles OF CARBON WILL BE BURNT SHOULD 196.5 kJ OF HEAT IS LIBERATED IN THE REACTION.
Explanation:
The standard heat of combustion of a substance is the heat evolved when one mole of the substance is burned completely in oxygen under standard conditions.
From the reaction, -393kJ of heat is required to burn 1 mole of Carbon completely in oxygen.
C(s) + O2 (g) -----> CO2(g) -393 kJ mol^-1
Should 196.5 kJ of heat was evolved by the reaction, the number of moles of carbon to be produced will be x moles;
-393 kJmol^-1 of heat was required to burn 1 mole of Carbon
196.5 kJ/mol of heat will burn x moles of carbon.
x = ( 196.5 * 1 / -393)
x = -0.5 moles
0.5 moles of carbon will be burnt when 196.5 kJ of heat is liberated
<u>Answer:</u> The molecular formula of compound is
<u>Explanation:</u>
We are given:
Empirical formula of compound = CHO
For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.
The equation used to calculate the valency is :
We are given:
Mass of molecular formula = 180 g/mol
Mass of empirical formula = 29 g/mol
Putting values in above equation, we get:
Multiplying this valency by the subscript of every element of empirical formula, we get:
Hence, the molecular formula of compound is
Answer:
0.1334
Explanation:
The number of atoms per unit (n) is given by:
The atomic packing factor (APF) is:
Answer:
2:1
1.2 × 10² g
Explanation:
Step 1: Write the balanced combustion equation
CH₄ + 2 O₂ ⇒ CO₂ + 2 H₂O
Step 2: Establish the appropriate molar ratio
According to the balanced equation, the molar ratio of O₂ to CH₄ is 2:1.
Step 3: Calculate the moles of CH₄ required to react with 15 moles of O₂
We will use the previously established molar ratio.
15 mol O₂ 1 mol CH₄/2 mol O₂ = 7.5 mol CH₄
Step 4: Calculate the mass corresponding to 7.5 moles of CH₄
The molar mass of CH₄ is 16.04 g/mol.
7.5 mol × 16.04 g/mol = 1.2 × 10² g