Answer:
The limiting reactant is the 6.279 g of
Explanation:
We have to start with the <u>reaction</u> between sodium carbonate () and the Nickel (II) Chloride (), so:
We will have a <u>double replacement reaction</u>. Now we have to <u>balance</u> the reaction, so:
The next step is the <u>calculation of the moles for each reactive</u>. For we have use the <u>molarity equation</u>:
For the calculation of moles of we have to use the <u>molar mass</u> of the compound (129.59 g/mol):
The next step is the division of each mole value by the <u>coefficient of each reactive</u> of the balance reaction. In this case <u>we have "1" for each reactive</u>, so:
The final step is to <u>choose the smallest value</u>. In this case is the value that correspond to . Therefore is the limiting reactive.
It should be rounded to 1 so I'm guessing true
The ideal gas behavior gets deviated because of the real gases. The particles in the gas occupy finite space and exert interactive forces between themselves.
Explanation:
An ideal gas behavior is at low temperature and at high pressure. According to kinetic theory, the ideal gases "do not occupy space" and there is "no interaction" among the gas molecules. But practically while applying the gas laws this is not the actual case.
<u>Ideal gas equation:
</u>
PV = nRT
Answer: 1.77 kg of manganese (IV) oxide reacts to produce 1.12kg of manganese metal.
Explanation:
The balanced chemical equation is:
To calculate the moles, we use the equation:
moles of manganese =
According to stoichiometry :
3 moles of is produced by = 3 moles of
Thus 20.4 moles of is produced by = of
Mass of (1kg=1000g)
Thus 1.77 kg of manganese (IV) oxide reacts to produce 1.12kg of manganese metal.
Answer:
Specific heat capacity of aluminium is 0.869J/g°C
Explanation:
Values: 51.1g of Al, 150.0g of water, Aluminium sample: 92.1°C; Water: 18.0°C, final temperature: 22.9°C.
The heat absorbed for the water is the same relased for the aluminium, the formula is:
Where m is mass, dT is change in temperature and C is specific heat of each compound (4.18J/g°C for water)
Replacing:
150.0g×(22.9°C-18.0°C)×4.18J/g°C = -51.1g×(22.9°C-92.1°C)×C(Al)
3072.3J = 3536.12g°C×C(Al)
0.869J/g°C = C(Al)
<em>Specific heat capacity of aluminium is 0.869J/g°C</em>