Answer : 51.8 g of nitrogen are needed to produce 100 grams of ammonia gas.
Solution : Given,
Mass of 
= 100 g
Molar mass of = 27 g/mole
Molar mass of 
= 28 g/mole
First we have to calculate moles of .
The given balanced chemical reaction is,
From the given reaction, we conclude that
2 moles of produced from 1 mole of
3.7 moles of produced from 
of
Now we have to calculate the mass of .
Mass of = Moles of × Molar mass of
Mass of = 1.85 mole × 28 g/mole = 51.8 g
Therefore, 51.8 g of nitrogen are needed to produce 100 grams of ammonia gas.
Answer:
the answer is C
Explanation:
6.7 to 13.2 then look at the numbers they go up but not a lot each time
It’s B
Because that is the smallest way scientists divide plants your welcome
Answer:
A. observing
Explanation:
There are various steps that are involved in a scientific investigation. Observation is the first step of the scientific investigation. In this step, a close examination is laid on the investigation. Observation is collected with the senses and the information is gathered.
In the given excerpt, Clive missed the observation part of the scientific investigation. All the other three steps were followed by Clive. He was not able to observe the situation and so was not able to provide the answers to the questions asked by his classmates.
Answer:
HF is the limiting reactant
Explanation:
The balanced equation for the reaction is given below:
SiO₂ + 4HF —> SiF₄ + 2H₂O
From the balanced equation above,
1 mole of SiO₂ reacted with 4 moles of HF.
Finally, we shall determine the limiting reactant. This can be obtained as illustrated below:
From the balanced equation above,
1 mole of SiO₂ reacted with 4 moles of HF.
Therefore, 7.5 moles of SiO₂ will react with = 7.5 × 4 = 30 moles of HF.
From the calculation made above, we can see clearly that it will take a higher amount (i.e 30 moles) of HF than what was given from the question (i.e 5 moles) to react completely with 7.5 moles of SiO₂.
Therefore, HF is the limiting reactant and SiO₂ is the excess reactant.
