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Sav [38]
3 years ago
12

I need help with this! 1-4 please!

Chemistry
1 answer:
PolarNik [594]3 years ago
4 0

Answer:

1 =   1.203 L.

2 = 1.291 dg.

3 = 843.062 - 638.1848 = 204.8772

The answer consist of seven significant figures.

4= 123.0 × 8.43 = 1036.89

answer consist of six significant figures.

Explanation:

Q 1 = part 1

Convert the 1202.57120 mL into L

Both milliliter and litters are the unit of volume. Liter is larger unit while milliliter is the smaller unit. One liter is equal to the thousand milliliter. In order to convert the milliliter into liter we will divide the given value by thousand.

1202.57120  / 1000 = 1.2025712 L

By rounding the answer into four significant figures  1.203 L.

Q 1 = Part 2

Convert the 0.1290743 g into dg.

The gram and decigram are both the unit of mass. gram is larger unit decigram is smaller unit. one gram is equal to 10 dg. In order to convert the gram unto dg we will multiply the value with 10.

 0.1290743 × 10 =  1.290743 dg

By rounding the answer into four significant figures  1.291 dg.

Q 1 = part 3

843.062 - 638.1848 = 204.8772

The answer consist of seven significant figures. The zero between the 2 and 4 is also a significant. If we have to round the answer in four significant figures the answer will be 204. 9.

Q 1 = part 4

123.0 × 8.43 = 1036.89

answer consist of six significant figures. if we round the answer into four significant figures then answer will be 1037.

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The equation for the combustion of CH4 (the main component of natural gas) is
Lera25 [3.4K]

Heat produced =  -13588.956 kJ

<h3>Further explanation</h3>

Given

The reaction of combustion of Methane

CH4(g)+2O2(g)→CO2(g)+2H2O(g) ΔH∘rxn=−802.3kJ

271 g of CH4

Required

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Solution

mol of 271 g CH₄ (MW=16 g/mol0

mol = mass : MW

mol = 271 : 16

mol = 16.9375

So Heat produced :

= mol x ΔH°rxn

= 16.9375 mol x −802.3kJ/mol = -13588.956 kJ

6 0
3 years ago
Please review the attachment
astra-53 [7]

Answer: The correct answer is -297 kJ.

Explanation:

To solve this problem, we want to modify each of the equations given to get the equation at the bottom of the photo. To do this, we realize that we need SO2 on the right side of the equation (as a product). This lets us know that we must reverse the first equation. This gives us:

2SO3 —> O2 + 2SO2 (196 kJ)

Remember that we take the opposite of the enthalpy change (reverse the sign) when we reverse the equation.

Now, both equations have double the coefficients that we would like (for example, there is 2S in the second equation when we need only S). This means we should multiply each equation (and their enthalpy changes) by 1/2. This gives us:

SO3 —>1/2O2 + SO2 (98 kJ)

S + 3/2O2 —> SO3 (-395 kJ)

Now, we add the two equations together. Notice that the SO3 in the reactants in the first equation and the SO3 in the products of the second equation cancel. Also note that O2 is present on both sides of the equation, so we must subtract 3/2 - 1/2, giving us a net 1O2 on the left side of the equation.

S + O2 —> SO2

Now, we must add the enthalpies together to get our final answer.

-395 kJ + 98 kJ = -297 kJ

Hope this helps!

8 0
3 years ago
Read 2 more answers
Stoichiometry: Calculate the moles of H2 produced by .042 g Mg in the equation Mg + 2HCl &gt; MgCl2 + H2
Evgesh-ka [11]

Answer:

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I think this is the correct answer I not a 100% sure if it is correct.

Explanation:

Guessing

6 0
3 years ago
Calculate the missing variables in each experiment below using Avogadro’s law.
blagie [28]

Answer:

The answer to your question is: letter c

Explanation:

Data

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V2 = 123 ml    n2 = ?

Formula

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5 0
3 years ago
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cricket20 [7]
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2.boiling
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4.<span>The base donates a hydrogen ion.
5.That causes the oxidation of another element
6.</span>MnO2
7.When a substance is reduced, electrons are lost.
8.True I think
9.False
10.True

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3 0
4 years ago
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