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2 years ago

How many moles are in 12.9 grams of Fe?

Chemistry

2 answers:

amid [387]2 years ago

6 0

Answer:

0.1677 is the answer

Explanation:

xeze [42]2 years ago

5 0

0.1677 is the answer

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Write the symbol for every chemical element that has atomic number greater than 55 and less than 140.8 u

patriot [66]

Answer on the picture

8 0

2 years ago

Predict the boiling point of water at a pressure of 1.5 atm.

Lina20 [59]

Answer:

100.8 °C

Explanation:

The Clausius-clapeyron equation is:

$ln\frac{P_{1} }{P_{2}} =$ -Δ $\frac{H_{vap}}{r} (\frac{1}{T_{2}}-\frac{1}{T_{1}} )$

Where 'ΔHvap' is the enthalpy of vaporization; 'R' is the molar gas constant (8.314 j/mol); 'T1' is the temperature at the pressure 'P1' and 'T2' is the temperature at the pressure 'P2'

Isolating for T2 gives:

$T_{2}=(\frac{1}{T_{1}} -\frac{Rln\frac{P_{2}}{P_{1}} }{Delta H_{vap}}$

(sorry for 'deltaHvap' I can not input symbols into equations)

thus T2=100.8 °C

7 0

2 years ago

What is the electron configuration of an element with atomic number 20?

Vedmedyk [2.9K]

[Ar]4s^2
hope it helps

8 0

3 years ago

Read 2 more answers

Which of the following statements about balanced chemical equations is true?

miv72 [106K]

Answer:

The correct answer is They provide the molar ratio of reactant and products in a chemical reaction.

Explanation:

Balanced chemical equation helps us to calculate the number of moles of both reactant and product.For example

2H2+O2=2H2O

From the above balanced equation it can be stated that 2 molecules of hydrogen(H2) reacts with 1 molecule of oxygen(O2) to form 2 molecules of water.

3 0

3 years ago

Read 2 more answers

How many grams of N2 can be produced when 6.50 g of O2<br> reacts?

Olenka [21]

Answer:

3.79 g of N2.

Explanation:

We'll begin by writing the balanced equation for the reaction.

This is given below:

4NH3 + 3O2 → 2N2 + 6H2O

Next, we shall determine the mass of O2 that reacted and the mass of N2 produced from the balanced equation.

This is illustrated below:

Molar mass of O2 = 16x2 = 32 g/mol

Mass of O2 from the balanced equation = 3 x 32 = 96 g

Molar mass of N2 = 2x14 = 28 g/mol

Mass of N2 from the balanced equation = 2 x 28 = 56 g

Summary:

From the balanced equation above,

96 g of O2 reacted to produce 56 g of N2.

Finally, we shall determine the mass of N2 produced by reacting 6.50 g of O2.

This can be obtained as follow:

From the balanced equation above,

96 g of O2 reacted to produce 56 g of N2.

Therefore, 6.50 g of O2 will react to produce = (6.50 x 56)/96 = 3.79 g of N2.

Therefore, 3.79 g of N2 were obtained from the reaction..

4 0

2 years ago