Answer:
Explanation:
The pressure is constant, so, to calculate the volume, we can use Charles' Law:
\dfrac{V_{1}}{T_{1}} = \dfrac{V_{2}}{T_{2}}
Data:
V₁ = ?; T₁ = 450 K
V₂ = 103.4 L; T₂ = 284.9 K
Calculation:
When 189.6 g of ethylene (C2H4) burns in oxygen to give carbon dioxide and water, how many grams of CO2 are formed? C2H4(g) + O2
1 answer:
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Answer: The reaction is not at equilibrium and will proceed to make more products to reach equilibrium.
Explanation:
Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as
K is the constant of a certain reaction when it is in equilibrium, while Q is the reaction quotient of activities of products and reactants at any stage other than equilibrium of a reaction.
For the given chemical reaction:
The expression for is written as:
Given : = 54.8
Thus as , the reaction will shift towards the right i.e. towards the product side.
Answer:
In 12.6g of there are 0.29 moles of
and
molecules of
Explanation:
First you should find the molar mass of the :
Then you should write the conversion factor using the molar mass:
So, there are 0.29 moles of in 12.6g of
.
Finally to find the number of molecules, you should use the Avogadro´s number:
There are moles of
in 12.6g of
Answer:
Explanation:
Hello,
Based on the given chemical reaction, as 31.2 mL of hydrogen are yielded, one computes its moles via the ideal gas equation under the stated conditions as shown below:
Now, since the relationship between hydrogen and magnesium is 1 to 1, one computes its milligrams by following the shown below proportional factor development:
Best regards.