40.1g of nitrogen gas is produced.
The equation given is
2 NH₃ + 3 CuO →3 Cu + N₂ + 3 H₂O
This equation is already balanced.
When 3 moles of CuO are consumed, 1 mole of nitrogen gas is produced.
We get 1 mole of nitrogen from 3 moles of copper oxide.
We need to find the number of moles of nitrogen gas produced when 4.3 moles of copper oxide are consumed.
4.3/3 x 1 = 1.433 mols
- 1.433 mols of nitrogen gas are produced
- The molar mass of nitrogen gas is 14+14 = 28g
- The amount of nitrogen gas produced in grams is 28x1.433 = 40.1g
40.1g of nitrogen gas can be made when 4.3 moles of CuO are consumed.
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Answer: 1.87 atm
Explanation:
Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.
The combined gas equation is,
where,
= initial pressure of gas = 2.50 atm
= final pressure of gas = ?
= initial volume of gas = 26.4 ml
= final volume of gas = 36.2 ml
= initial temperature of gas = 
= final temperature of gas = 
Now put all the given values in the above equation, we get:
The new pressure is 1.87 atm by using combined gas law.
Answer: 25.8 g of 
will be produced from the decomposition of 73.4 g of 
Explanation:
To calculate the moles :
The balanced chemical reaction is:
According to stoichiometry :
2 moles of produce = 3 moles of
Thus 0.242 moles of will produce= 
of
Mass of = 
Thus 25.8 g of will be produced from the decomposition of 73.4 g of
Answer:
I'd say the correct answer is A
Explanation:
hope this helps:)
sorry if its wrong:(
