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Triss [41]
3 years ago
15

So3+H2o→H2 So4 use the oxidation numbers to identify the nature of this reaction redox or not​

Chemistry
1 answer:
makvit [3.9K]3 years ago
4 0

This is not an redox reaction because the oxidation number of Oxygen atom is not changing.

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In the synthesis reaction, the white powder produced is magnesium oxide (mgo, mm = 40.3 g/mol). how many moles of magnesium oxid
gulaghasi [49]
Number of moles = mass of product / molecular mass
=mass of product (MgO) / 40.3

Since the mass of MgO is not given in the question, the correct answer choice cannot be given.  However, proceeding witht eh above formula will enable you to find the correct number of moles given the mass of MgO.
3 0
3 years ago
6. If 4 mole of the rocket fuel ammonium perchlorate, NH4C/04 (s) is
Bond [772]

Answer:

144g of H₂O

Explanation:

3NH₄ClO₄(s) + 3Al → Al₂O₃(s) + AlCl₃(s) + 3NO(g) + 6H₂O(g)

From the equation:

3 moles of NH₄ClO₄ produced 6 moles of H₂O

4 moles of NH₄ClO₄ produced ? moles of H₂O

(4 ₓ 6)/3 = \frac{24}{3} = 8 moles of H₂O

1 mole of H₂O = (1 × 2) + 16 = 18g (The Relative Molecular mass of H₂O)

8 moles of H₂O = ?

Therefore 8 × 18 = 144g

=144g of H₂O

3 0
3 years ago
A mineral consisted of 29.4% calcium, 23.5% sulfur and 47.1% oxygen. What is the empirical formula?
inessss [21]
Step  one  calculate  the  moles  of  each  element
that  is  moles= %  composition/molar  mass
molar  mass  of    Ca  =  40g/mol,     S=  32  g/mol ,   O=  16 g/mol

moles  of      Ca = 29.4 /40g/mol=0.735 moles,      S= 23.5/32  =0.734 moles,  O= 47.1/16= 2.94   moles

calculate  the mole  ratio  by  dividing   each  mole with  smallest  mole   that   is  0.734
Ca=  0.735/0.734= 1,      S=  0.734/0.734 =1,   O  = 2.94/  0.734= 4
therefore  the  emipical  formula  =  CaSO4
5 0
3 years ago
What is an example of a telescope?
lianna [129]
Is there choices? Cuz if there is i Need them


4 0
3 years ago
How much heat in kj is released by burning 9.5 grams of methane?
tatyana61 [14]
Methane is the compound CH4, and burning it uses the reaction:

CH4 + O2 -> CO2 + H2O, which is rather exothermic. To find the heat released by burning a certain amount of the substance, you should look at the bond enthalpy of each compound, and then compare the values before and after the reaction. In methane, there are 4 C-H bonds, which have bond energy of 416 kj/mol, resulting in a total bond energy of 1664 kj/mol. O2 is 494 kj/mol. Therefore we have a total of 2080 kj/mol on the left side. On the right side we have CO2, which has 2 C=O bonds, each at 799 kj/mol each, resulting in 1598 kj/mol, and H2O has 2 O-H bonds, at 459kj/mol each, resulting in a total of 2516 kj/mol on the right hand side. Now, this may be confusing because the left hand side seems to have less heat than the right, but you just need to remember: making minus breaking, which results in a total change of 436kj/mol heat evolved.

Now it is a simple matter of find the mols of CH4 reacted, using n=m/mr.

n = 9.5/16.042 = 0.592195 mol

Therefore, if we reacted 0.592195 mol, and we produced 436 kj for one mol, the total amount of energy evolved was 436*<span>0.592195 kj, or 258.197 kj.</span>
7 0
4 years ago
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