Answer: If a reaction produces a gas such as oxygen or carbon dioxide, there are two ways to measure the reaction rate: using a gas syringe to measure the gas produced, or calculating the reduction in the mass of the reaction solution.
Explanation:
https://courses.lumenlearning.com/introchem/chapter/measuring-reaction-rates/#:~:text=If%20a%20reaction%20produces%20a,mass%20of%20the%20reaction%20solution.
This is the site I got it from. I hope this helps.
The balanced equation :
2HCl + Zn ⇒ ZnCl₂ + H₂
<h3>Further explanation</h3>
Given
Reaction(unbalanced)
HCl + Zn ⇒ ZnCl₂ + H₂
Required
Balanced equation
Solution
Give a cofficient(the most complex compound=1)
aHCl + bZn ⇒ ZnCl₂ + cH₂
Make an equation
Zn, left = b, right = 1⇒b=1
Cl, left = a, right = 2⇒a=2
H, left = a, right = 2c⇒2c=a⇒2c=2⇒c=1
The equation becomes :
<em>2HCl + Zn ⇒ ZnCl₂ + H₂</em>
Answer:
A rock is a naturally occurring solid mixture of one or more minerals or organic matter.
Explanation:
A mineral is naturally formed, inorganic, solid, with a fixed chemical composition, and crystalline structure. A rock at the surface of the Earth would need to be weathered down into sediments.
<u>HOPE THIS WILL GIVE YOU SOME IDEAS !!!!!</u>
The balanced chemical reaction would be:
16Al + 3S8 = 8Al2S3
We need to determine which reactants are the limiting and the excess. To determine this, we use the initial amounts of the reactants given above. We need to convert them into units of moles and use the balanced reaction to relate the substances calculating the amount needed to react all of the reactants. We do as follows:
63.8 g Al ( 1 mol Al / 26.98 g Al ) ( 3 mol S8 / 16 mol Al ) (256.48 g S / 1 mol S )= 113.72 g S8 needed to completely react
72.3 g S8 ( 1 mol S8 / 256.48 g S8) ( 16 mol Al / 3 mol S8 ) ( 26.98 g / mol ) = 40.56 g Al needed to completely react
Therefore, the excess would be Al and the limiting would be sulfur. The amount excess would be 63.8 g Al - 40.56 g Al = 23.24 g Al
<h3><u>Answer;</u></h3>
- <u>0.433 g N2 </u>
- <u>0.293 g O2 </u>
- <u>0.0367 g He</u>
<h3><em>Explanation and solution;</em></h3>
- We can start by getting the total pressure; which will be the sum of the partial pressure of each gas.
221 torr + 131 torr + 131 torr
P (total) = 483 torr total
n = PV / RT, we can determine the total number of moles of the mixture
= (483 torr) x (1.30 L) / ((62.36367 L Torr/K mol) x (25.0 + 273.15 K))
= 0.033769 mol gases total
-
Therefore; we can determine the mass of each gas;
- <u>Nitrogen gas </u>
<em>N2 = 28.01 g/mol</em>
<em>= (0.033769 mol) x ( 221 torr N2/ 483 torr) x (28.01 g N2/mol) </em>
<u>= 0.433 g N2 </u>
<em>
O2 = 32 g/ mol </em>
<em> =(0.033769 mol) x (131 torr O2/ 483 torr) x (32 g O2/mol)</em>
<em> </em><em><u>= 0.293 g O2 </u></em>
- <em><u>Helium gas </u></em>
<em><u>
</u></em><em>He = 4 g/mol</em>
<em>= (0.033769 mol) x (131 torr He/ 483 torr) x (4.00 g He/mol) </em>
<em><u>= 0.0367 g He</u></em>