Answer:
72.0 mL of steam is formed.
Explanation:
The reaction is :
You can treat coefficient of compounds as amount of volume used.
Therefore for 4 mL of ammonia 5 mL of oxygen is used to form 4 mL of nitric oxide gas and 6 mL of steam.
For 1 mL of ammonia 
(=1.25) mL of oxygen is used to form 
(=1) mL of nitric oxide gas and 
(=1.5) mL of steam.
OR
Just transform the chemical equation by dividing the whole equation by 4 so that the coefficient of 
become one like this
We don't know which one will be completely exhausted and which one will be left so we have to consider two cases :
<em>1. </em><em>Assume ammonia to be completely exhausted</em>
For 50 mL of ammonia 
(= 62.5) mL of oxygen is needed. But we have just 60 mL of oxygen so this assumption is false.
2. <em>Assume oxygen to be completely exhausted</em>
For 60 mL of oxygen only 
(=48) mL of ammonia is needed. In this case we have sufficient amount of ammonia. So this case is true.
Now we know that during complete reaction 48 mL of ammonia and 60 mL of oxygen is used which will form (= 48) mL of nitic oxide gas and 
(= 72) mL of steam.
Therefore <em>72 mL of steam </em>is formed.
Hi lovely,
The answer you're looking for would be Plasma.
Answer:
How many moles of oxygen gas are required to make 8.33 moles of carbon dioxide? ... be used to produce 1.99 grams of water. 1.99 mg H2O X. 1mol H2O. 18.0g X ... c. If the reaction produces 5.3 mg of carbon dioxide how many grams of water ... X. 25mol O2. 2mol C8H18. X. 32.0g O2. 1mol O2. = 4.80 x 103g O2. Answer ...
Explanation:
Ans: Elements in the same period have the same number of electron shells.
Answer:
Explanation:
Hello there!
In this case, sine the solution of this problem require the application of the Raoult's law, assuming heptane is a nonvolatile solute, so we can write:
Thus, we first calculate the mole fraction of chloroform, by using the given masses and molar masses as shown below:
Therefore, the partial pressure of chloroform turns out to be:
Regards!
