The Law of conservation of mass states that option C: matter is neither created nor destroyed.
<h3>What is the law of conservation of matter?</h3>
Physical and chemical changes can cause matter to transform into different forms, but no matter what happens, matter is always conserved. There is no creation or destruction of matter; the amount of matter is the same before and after the transformation.
The principle of matter conservation. argues that matter cannot be generated or destroyed during a chemical reaction. The same number of atoms exist before and after the alterations even though the matter may shift from one form to another. reactant.
Therefore, According to the principle of mass conservation, neither chemical processes nor physical changes can create or destroy mass in an isolated system. The mass of the products and reactants of a chemical reaction must be equal, in accordance with the law of conservation of mass.
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1. Multiple-choice
Q.
Conservation of matter article questions
Law of conservation of mass states that
answer choices
matter is created
matter is destroyed
matter is neither created nor destroyed
matter does not change
Answer:
![V_{NH_3}=39.6L](https://tex.z-dn.net/?f=V_%7BNH_3%7D%3D39.6L)
Explanation:
Hello,
By assuming STP conditions (0°C and 1atm), we first compute the reacting moles of both hydrogen and nitrogen as shown below via the ideal gas equation:
![n_{N_2}=\frac{PV}{RT}=\frac{1atm*36.7L}{0.082 \frac{atm*L}{mol*K}*273.15K} =1.64molN_2\\n_{H_2}=\frac{PV}{RT}=\frac{1atm*59.4L}{0.082 \frac{atm*L}{mol*K}*273.15K} =2.65molH_2](https://tex.z-dn.net/?f=n_%7BN_2%7D%3D%5Cfrac%7BPV%7D%7BRT%7D%3D%5Cfrac%7B1atm%2A36.7L%7D%7B0.082%20%5Cfrac%7Batm%2AL%7D%7Bmol%2AK%7D%2A273.15K%7D%20%3D1.64molN_2%5C%5Cn_%7BH_2%7D%3D%5Cfrac%7BPV%7D%7BRT%7D%3D%5Cfrac%7B1atm%2A59.4L%7D%7B0.082%20%5Cfrac%7Batm%2AL%7D%7Bmol%2AK%7D%2A273.15K%7D%20%3D2.65molH_2)
Next, one identifies the limiting reagent by computing the moles of hydrogen that completely react with 1.64mol of nitrogen as follows:
![n_{H_2}^{reacting}=1.64molN_2*\frac{3molH_2}{1molN_2}=4.92molH_2](https://tex.z-dn.net/?f=n_%7BH_2%7D%5E%7Breacting%7D%3D1.64molN_2%2A%5Cfrac%7B3molH_2%7D%7B1molN_2%7D%3D4.92molH_2)
In such a way, as there are just 2.65 available moles of hydrogen one states that we have spare nitrogen and the hydrogen is the limiting reagent, thus, the yielded moles of ammonia are computed as:
![n_{NH_3}=2.65molH_2*\frac{2molNH_3}{3molH_2}=1.767molNH_3](https://tex.z-dn.net/?f=n_%7BNH_3%7D%3D2.65molH_2%2A%5Cfrac%7B2molNH_3%7D%7B3molH_2%7D%3D1.767molNH_3)
Finally, one computes the required volume in liters as:
![V_{NH_3}=\frac{nRT}{P}=\frac{1.767mol*0.082 \frac{atm*L}{mol*K} *273.15K}{1atm}\\V_{NH_3}=39.6L](https://tex.z-dn.net/?f=V_%7BNH_3%7D%3D%5Cfrac%7BnRT%7D%7BP%7D%3D%5Cfrac%7B1.767mol%2A0.082%20%5Cfrac%7Batm%2AL%7D%7Bmol%2AK%7D%20%2A273.15K%7D%7B1atm%7D%5C%5CV_%7BNH_3%7D%3D39.6L)
Best regards.
Answer:
b is the best in my opion
Explanation:
Answer:
you would need to multiply 50 times 2 wich is 100 so i beleive its 100
Explanation: