Determine ΔT if T1 = 5oC and T2 = 123oC

To accomplish this, we must first understand the rules of significant figures.
<span>Rule #1: All digits other than zero are considered significant. (1234)
 Rule #2: Leading zeros do not count as significant. (0.093)
 Rule #3: Zeros situated between non-zero digits are significant. (78309)
 Rule #4: Trailing zeros are significant only if there is a decimal point. (0.05470)

Therefore, considering these rules, 56.0g contains three significant figures due to the decimal point.
0.0004m has just one significant figure per Rule #2.
1003ml contains 4 significant figures because the zeros are between two significant digits.
Lastly, 0.0350s has 3 significant figures because digits following a decimal point are counted.

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2C3H6 (g) + 2NH3 (g) + 3O2 (G) -> 2C3H3N (g) + 6H2O (g)

To begin, this isn't really a chemistry forum, but anyway.

This represents a limiting reagent scenario.

Set it up as a Dimensional Analysis issue.

Begin with your desired outcome.

Your goal is to find the mass of acrylonitrile (C3H3N)

so you should initiate with that (I'll abbreviate Acrylonitrile as ACL for convenience)

(g) = (53 g of ACL/1mol ACL) (2 mols ACL/2 mol C3H6)/ (1mol C3H6/42 grams) (15.0 grams)

If you calculate that, you will find that 15 grams of C3H6 yields 18.9 grams of acrylonitrile produced.

Utilize the same approach for the remaining two reactants.

So, I figured it out, and for

oxygen, I calculated 11.04 grams

and for ammonia, I calculated 15.29 grams

This means that the maximum possible production is 11.04 grams, since to create any additional amount, more O2 would be necessary, but with only 10 grams available, that's the upper limit for this reaction.

The other two reactants are in excess.

Please rate as brainliest!

The accurate answer is 33.8 g.

The chemical equation can be expressed as:

2H2 + O2 = 2H2O

Given the amounts of the reactants, we need to identify the limiting reactant before calculating the amount of product generated.

4.0 g H2 ( 1 mol / 2.02 g ) = 1.98 mol H2
5.0 g O2 ( 1 mol / 32 g ) = 0.1563 mol O2

The limiting reactant is O2, as it will be fully consumed in the reaction.

0.1563 mol O2 ( 2 mol H2O / 1 mol O2 ) ( 18.02 g / mol ) = 5.6 g H2O will be produced

Answer: The correct choice is (b).

Explanation:

We have the mass of Magnesium at 97.22 g, and the molar mass of Magnesium is 24.305 g/mol.

Therefore, the calculation for the number of moles is as follows.

          Number of moles =

                                 =  

                                 = 4 mol

Additionally, it is known that one mole contains atoms/mol. Thus, we calculate the total number of atoms in 4 moles as follows.

               

               = atoms

or,            = atoms

Hence, we conclude that in 97.22 grams of Magnesium, there are atoms.