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Jet001 [13]
3 years ago
7

50 points - I need this really soon! plz help

Chemistry
1 answer:
kirill115 [55]3 years ago
7 0

Answer:

C.

Explanation:

Butane (C4H10) has 3 C-C bonds in the carbon chain and 10 C-H bonds

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How many grams of HF are needed to react with 3.0 moles of Sn? *
Lostsunrise [7]

Answer:

120g

Explanation:

We'll begin by writing the balanced equation for the reaction. This is given below:

Sn + 2HF —> SnF2 + H2

Next, we shall determine the number of mole of HF needed to react with 3 moles of Sn.

From the balanced equation above, 1 mole of Sn reacted with 2 moles of HF.

Therefore, 3 moles of Sn will react with = 3 x 2 = 6 moles of HF.

Finally, we shall convert 6moles of HF to grams

This is illustrated below:

Number of mole of HF = 6moles

Molar Mass of HF = 1 + 19 = 20g/mol

Mass of HF =..?

Mass = number of mole x molar Mass

Mass of HF = 6 x 20

Mass of HF = 120g

Therefore, 120g of HF is needed to react with 3 moles of Sn

6 0
3 years ago
A sample of a compound is decomposed in the laboratory and produces 330 g carbon, 69.5 g hydrogen, and 220.2 g oxygen. Calculate
Zarrin [17]

Answer: Empirical formula is C_2H_5O

Explanation: We are given the masses of elements present in a sample of compound. To evaluate empirical formula, we will be following some steps.

<u>Step 1 :</u> Converting each of the given masses into their moles by dividing them by Molar masses.

Moles=\frac{\text{Given mass}}{\text{Molar mass}}

Molar mass of Carbon = 12.0 g/mol

Molar mass of Hydrogen = 1.0 g/mol

Molar mass of Oxygen = 16.0 g/mol

Moles of Carbon = \frac{330g}{12g/mol}=27.5moles

Moles of Hydrogen = \frac{69.5g}{1g/mol}=69.5moles

Moles of Oxygen = \frac{220.2g}{16g/mol}=13.76moles

<u>Step 2: </u>Dividing each mole value by the smallest number of moles calculated above and rounding it off to the nearest whole number value

Smallest number of moles = 13.76 moles

\text{Mole ratio of Carbon}=\frac{27.5moles}{13.76moles}=1.99\approx 2

\text{Mole ratio of Hydrogen}=\frac{69.5moles}{13.76moles}=5.05\approx 5

\text{Mole ratio of Oxygen}=\frac{13.76moles}{13.76moles}=1

<u>Step 3:</u> Now, the moles ratio of the elements are represented by the subscripts in the empirical formula

Empirical formula becomes = C_2H_5O

7 0
3 years ago
BRAINLIESTTT ASAP! PLEASE HELP ME :)
Iteru [2.4K]

Answer:

The mass of the products left in the test tube will be less than that of the original reactants.

Explanation

The equation for the reaction is

Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)

 1.0          3.0              3.9             0.1

Assume you started with 1.0 g of Mg.

It will react with 3.0 g of HCl to form 3.9 g of MgCl2 and 0.1 g of H2

.

Mass of reactants = mass of products

        1.0 g + 3.0 g = 3.9 g + 0.1 g

                    4.0 g = 4.0 g

The Law of Conservation of Mass is obeyed.

However, your test tube and its contents will weigh 0.1 g less than it did before the reaction.

Does that contradict the Law of Conservation of Mass? It does not.

One of the products was the gas, hydrogen, and it escaped from the test tube. You weren't measuring all the products, so test tube and its contents weighed less than before.

7 0
3 years ago
11. What is the concentration (in M) of an ammonia (NH3) solution if 12.23 grams of ammonia are
photoshop1234 [79]

Answer:  1.284M NH3

Explanation:  (12.23 grams)/(17.0 gramms/mole) = 0.7191 moles

Dissolved in 560.0 ml (=0.5600L)

(0.7191 moles)/(0.560L) = 1.284M  (4 sig figs)

5 0
2 years ago
Temperature and silica content determine the _______ of magma. A. color B. elasticity C. viscosity D. texture
Rudik [331]
Hello.

The answer is 

<span> C. viscosity.

</span>Temperature and silica content determine the viscosity of magma. 

The viscosity of amagma<span> is largely controlled by the </span>temperature.
<span>
Have a nice day.</span>
3 0
3 years ago
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