4X + 3O₂ = 2X₂O₃
n(X₂O₃)=0.02225 mol
m(X)=4.000 g
x - the molar mass of metal
m(X)/4x=n(X₂O₃)/2
x=m(X)/{2n(X₂O₃)}
x=4.000/{2*0.02225)=89.89 g/mol
X=Y (yttrium)
B.2C2H6 + 5O2 >2CO2 +3H2O
Answer:
Hope this helps :)
Explanation:
In the chemical industry, acids react in neutralization reactions to produce salts. For example, nitric acid reacts with ammonia to produce ammonium nitrate, a fertilizer. Additionally, carboxylic acids can be esterified with alcohols, to produce esters.
Acids are used to remove mineral deposits, rust stains, and hard water deposits. They can remove discoloration from some metals, such as aluminum, brass, bronze, and copper. Some acids are effective both in cleaning and disinfecting surfaces.
Answer:
Okay, Left top= waning gibbous
left second= new moon
left third= third quarter
left fourth= waxing crescent
right top= Waning crescent
right second= first quarter
right third= full moon
right fourth= Waxing gibbous
hope you do good :)
Answer:
See detailed explanation.
Explanation:
Hello!
In this case, for the reaction:
It is known that the equilibrium constant tends to be greater than 1; therefore, it is a reaction that tends to go rightwards towards the formation of hydrogen iodide.
a) Here, since the reaction tends to form the product, it is clear that the initial concentration of iodine and hydrogen will decrease as the reaction reaches equilibrium in order to increase the concentration of hydrogen iodide.
b) Yes, it stops at the point in which the following expression:
![\frac{[HI]^2}{[I_2][H_2]}](https://tex.z-dn.net/?f=%5Cfrac%7B%5BHI%5D%5E2%7D%7B%5BI_2%5D%5BH_2%5D%7D)
Equals the equilibrium constant.
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