Answer:
0.171 grams of oxygen combined with the metal.
Explanation:
Mass of magnesium oxide produced = 0.421 g
Mass of magnesium metal used = 0.250 g
Suppose reaction completely converts the magnesium into magnesium oxide.
Mass of oxygen combined with magnesium = m
0.421 g = 0.250 g + m
m = 0.421 g - 0.250 g = 0.171 g
0.171 grams of oxygen combined with the metal.
A net ionic equation which tends to show the ions that underwent a change in the reaction
<h3>What is a reaction equation?</h3>
The term reaction equation is the term that can be used to describe the instance where reactants combine together. If this occurs in solution we can say that the reaction is an aqueous phase reaction because the reactants wee all dissolved in solution.
It is possible for ionic substances in solution to react. When this occurs, it is possible for us to put down a net ionic equation which tends to show the ions that underwent a change in the reaction and the product of this reaction may be a liquid, a gas or a solid.
In this case, the complete molecular equation can be written as;
Ba(NO3)2(aq) + Na2SO4(aq) -----> BaSO4(s) + 2NaNO3(aq)
The complete ionic equation can be written as;
Ba^2+(aq) + 2NO3^-(aq) + 2Na^+(aq) + SO4^2-aq) -----> BaSO4(s) + 2NO3^-(aq) + 2Na^+(aq)
Net ionic equation is;
Ba^2+(aq) + + SO4^2-aq) -----> BaSO4(s)
Learn more about balanced reaction equation:brainly.com/question/22064431
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Answer:
40 g
Explanation:
Find the line labeled KClO3 (which might take you a min, theres a lot of lines here)
Notice that when the line creates a direct point, you can measure the exact temperature needed to dissolve a certain amount (like how they gave 30 degrees and it lined up perfectly with the 10 g line. )
Since its asking for the amount at 80 degrees, all you need to do is trace the line to the 80 degree point, and look at the grams. (notice it made a direct point, so there definitely should be any decimals or guesswork)
By reading the graph, you can tell that at 80 degrees, it dissolves 40 grams, and that is your answer.
Hope this helps :)
Answer:
NH2.
Explanation:
The mass of hydrogen in the sample = 1.525 - 1.333 = 0.192g.
Dividing the 2 masses by the relative atomic mass of hydrogen and nitrogen:
H: 0.192 / 1.008 = 0.1905
N: 1.333 / 14.007 = 0.09517
The ratio of N to H = 0.09517 : 0.1905
= 1 : 2.
So the empirical formula is NH2.
Answer: 0.4 g
Explanation:
1) Balanced chemical equation:
2) 2C2H2 + 5 O2 → 4CO2 + 2 H2O
3) mole ratios:
2 mol C2h2 : 5 mol O2
4) Convert 0.13 g C2H2 into number of moles
n = mass in grams / molar mass
molar mass C2H2 = 2 *12g/mol + 2*1 g/mol = 26 g/mol
n = 0.13 g / 26 g/mol = 0.005 mol
5) Set the proportion with the unknown
5 mol O2 x
----------------- = ---------------
2 mol C2H2 0.005 mol C2H2
x = 0.005 mol C2H2 * 5 mol O2 / 2 mol C2H2 = 0.0125 mol O2
6) Convert 0.0125 mol O2 to grams
mass = number of moles * molar mass
molar mass of O2 = 32 g/mol
mass = 0.0125 mol * 32 g/mol = 0.4 g
Answer: 0.4 g
