Answer:
1.42 moles
Explanation:
25.58 g of H₂O .
Molecular weight of water = 2 x 1 + 16 = 18
1 mole of water = 18 g of water
18 g of water = 1 mole
25.58 g of water = 25.58 / 18 mole
= 1.42 moles .
Answer: 14.3%Explanation: In order to find the mass percent of hydrogen in this compound, you must determine how many grams of hydrogen you'd get in 100 g of compound.
In your case, you know that an unknown mass of hydrogen reacts with 0.771 g of carbon to form 0.90 g of hydrocarbon, which is a compound that contains only carbon and hydrogen.
Use the total mass of the hydrocarbon to determine how many grams of hydrogen reacted with the carbon.
Now, if 0.90 g of this compound contain 0.129 g of hydrogen, it follows that 100 g of this compound will contain.
So, if 100 g of this compound contain 14.33 g of hydrogen, it follows that the mass percent of hydrogen is 14.3%
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Answer:
Ni + Sn^2+ —> Sn + Ni^2+
Explanation:
First let us generate an elemental equation for the reaction. This is illustrated below:
Ni + Sn(NO3)2 —> Sn + Ni(NO3)2
From the equation above, a solid metal Sn is formed.
Now we can generate a net ionic equation as follows:
Ni + Sn^2+ —> Sn + Ni^2+
