According to Avogadro's law, the two gases will have equal number of molecules.
<h3>Avogadro's law </h3>
From the question, we are to determine how the two gases would compare according to Avogadro's law
First, we will state the Avogadro's law
<em>Avogadro's law</em> states that "equal volume of all gases at the <u>same temperature and pressure</u> contain the same number of molecules"
Now, from the given information
We have 2 liters of hydrogen gas and 2 liters of oxygen gas at the <u>same temperature and pressure</u>
According to Avogadro's law, gases that are equal in volume and are at the same temperature and pressure will have equal number of molecules.
Hence, according to Avogadro's law, the two gases will have equal number of molecules.
Learn more on Avogadro's law here: brainly.com/question/26174006
<span>Energy = Mass * heat capacity * temperature change so,
</span>The energy added is 435 J and the temperature has to increase since the energy is added.
<span>435 J = 10.0 g * 0.89 J/gC * temperature change </span>
<span>Temperature change = 48.9 C </span>
<span>The initial temperature is 25.0 C, the final temperature is 25.0 C + 48.9 C = 73.9 C.</span>
Answer:
atomic mass of X is 48.0 amu
Explanation:
Let y be the atomic mass of X
Molar mass of O_2 is = 2×16 = 32 g / mol
X + O2 -----> XO_2
According to the equation ,
y g of X reacts with 32 g of O_2
24 g of X reacts with Z g of O_2
Z = ( 32×24) / y
But given that 24.0 g of X exactly reacts with 16.0 g of O_2
So Z = 16.0
⇒ (32×24) / y = 16.0
⇒ y = (32×24) / 16
y= 48.0
So atomic mass of X is 48.0 amu
2.03 kg = 2030 grams
2030g C6H8O7 (1 mol/ 192.124g) = 10.6 mol C6H8O7
