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The balanced chemical equation for the production of chromium metal from the reaction of chromium(ll) nitrate reacts with a strip of zinc is:
3 Zn + 2 Cr(NO₃)₃ → 2 Cr + 3 Zn(NO₃)₂
This is a redox reaction, which <u>is a chemical reaction in which one or more electrons are transferred between the reagents</u>, causing a change in their oxidation states. In the proposed reaction, Cr oxidation state goes from +3 to 0, becoming metallic chromium, while Zn goes from being Zn⁰ to Zn²⁺.
<u>The mass of chromium metal produced in the above reaction will be,</u>
425.0 mL x x
x
x
= 5.52 g
So, the mass of chromium metal produced when 425.0mL of 0.25M chromium(ll) nitrate reacts with a strip of zinc that remains in excess is 5.52 g of Cr.
<u>Answer:</u> The maximum amount of water that could be produced by the chemical reaction is 20.16 grams
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
.....(1)
- <u>For butane:</u>
Given mass of butane = 13 g
Molar mass of butane = 58.12 g/mol
Putting values in equation 1, we get:
- <u>For oxygen gas:</u>
Given mass of oxygen gas = 70.9 g
Molar mass of oxygen gas = 32 g/mol
Putting values in equation 1, we get:
The chemical equation for the reaction of butane and oxygen gas follows:
By Stoichiometry of the reaction:
2 moles of butane reacts with 13 moles of oxygen gas
So, 0.224 moles of butane will react with = of oxygen gas
As, given amount of oxygen gas is more than the required amount. So, it is considered as an excess reagent.
Thus, butane is considered as a limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
2 moles of butane produces 10 moles of water
So, 0.224 moles of butane will produce = of water
Now, calculating the mass of water from equation 1, we get:
Molar mass of water = 18 g/mol
Moles of water = 1.12 moles
Putting values in equation 1, we get:
Hence, the maximum amount of water that could be produced by the chemical reaction is 20.16 grams