A stoichiometric mixture is a mixture of fuel and oxygen for which the masses of these two components are exactly those needed for complete combustion.
A stoichiometric mixture is a balanced mixture of fuel and oxygen.
The fuel and the oxygen react completely without the excesses of either.
The opposite of a stoichiometric mixture is called feeding an excess, when minimum one reactant is an excess amount.
Balanced chemical equation for reaction of combustion one type of a fuel: C₈H₁₈ + 25/2O₂ → 8CO₂ + 9H₂O
Stoichiometric mixture for this example is when fuel (C₈H₁₈) and oxygen(O₂) react in proportion 1 : 12.5.
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Answer: Object B will heat up more.
Explanation:
The formula for specific heat is as follows.
Q = 
Where,
Q = heat provided
m = mass
C = specific heat
= change in temperature
Now, both the objects have same mass and equal amount of heat is applied.
According to the formula, the equation will be as follows.
= 
= 
Cancel m from both sides, as mass is same. Therefore,
= 
Cancel out the initial temperature and put the values of specific heat, then the equation will be as follows.
= 
Therefore, from the above equation it can be concluded that the object with low specific heat will heat up more as its specific heat will be inversely proportional to its final temperature.
Hence, object B will heat up more.
Answer:
Molar mass = 0.09 × 10⁴ g/mol
Explanation:
Given data:
Mass = 0.582 g
Volume = 21.3 mL
Temperature = 100°C
Pressure = 754 mmHg
Molar mass = ?
Solution:
(21.3 /1000 = 0.0213 L)
(100+273= 373 K)
(754/760 = 0.99 atm)
PV = nRT
n = PV/RT
n = 0.99 atm × 0.0213 L / 0.0821 atm. L. mol⁻¹. k⁻¹ × 373 K
n =0.02 mol/ 30.6
n = 6.5 × 10⁻⁴ mol
Molar mass = Mass/ number of moles
Molar mass = 0.582 g / 6.5 × 10⁻⁴ mol
Molar mass = 0.09 × 10⁴ g/mol