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2 years ago

What is the atomic mass of one mole of H? g/mole

2 answers:

7 0

For one mole of hydrogen, H, the atomic mass is 1 g per mole. Hydrogen contains 1 proton and zero neuton. A neutral atom of hydrigen also contains 1 electron.

DENIUS [597]2 years ago

6 0

Answer:

1.008 is correct

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The electronic arrangement of an atom shows how electrons are distributed across the different energy levels. Which of the follo

bazaltina [42]

Answer:

The answer is D which is Selenium

5 0

3 years ago

One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4NH3 (g) 5O2 (g

madreJ [45]

Answer:

O2 is the limiting reactant.

Explanation:

Step 1: Data given

Mass of NH3 = 2.00 grams

Mass of O2 = 2.50 grams

Molar mass NH3 = 17.03 g/mol

Molar mass O2 = 32 g/mol

Step 2: The balanced equation

4NH3(g) + 5O2 (g) → 4NO(g) + 6H2O (g)

Step 3: calculate moles NH3

Moles NH3 = mass NH3 / molar mass NH3

Moles NH3 = 2.00 grams / 17.03 g/mol

Moles NH3 = 0.117 moles

Step 4: Calculate moles O2

Moles O2 = mass / molar mass O2

Moles O2 = 2.50 grams / 32 g/mol

Moles O2 = 0.0781 moles

Step 5: Calculate the limiting reactant

For 4 moles NH3 we need 5 moles O2 to produce 4 moles NO and 6 moles H2O

O2 is the limiting reactant. It will completely be consumed. (0.0781 moles). NH3 is in excess. There will react 4/5 * 0.0781 moles = 0.0625 moles

There will remain 0.117 - 0.0625 = 0.0545 moles NH3

O2 is the limiting reactant.

8 0

3 years ago

If 5.0 liters H2 (g) at STP is heated to a temperature of 985, pressure remaining constant, the new volume of the gas will be?

vlada-n [284]

Answer:

$V_2=18 \ L \ H_2$

General Formulas and Concepts:

Chemistry - Gas Laws

STP (Standard Conditions for Temperature and Pressure) = 22.4 L per mole at 1 atm, 273 K
Charles' Law: $\frac{V_1}{T_1} =\frac{V_2}{T_2}$

Explanation:

Step 1: Define

Initial Volume: 5.0 L H₂ gas

Initial Temp: 273 K

Final Temp: 985 K

Final Volume: ?

Step 2: Solve for new volume

Substitute: $\frac{5 \ L \ H_2}{273 \ K} =\frac{x \ L \ H_2}{985 \ K}$
Cross-multiply: $(5 \ L \ H_2)(985 \ K) = (x \ L \ H_2)(273 \ K)$
Multiply: $4925 \ L \ H_2 \cdot K = 273x \ L \ H_2 \cdot K$
Isolate x: $18.0403 \ L \ H_2 = x$
Rewrite: $x=18.0403 \ L \ H_2$

Step 3: Check

We are given 2 sig figs as the smallest. Follow sig fig rules and round.

$18.0403 \ L \ H_2 \approx 18 \ L \ H_2$

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3 years ago

What is the quire drought of hotdog water and why does it taste wired

Liula [17]

Answer:

Oil trout

Explanation:

Hotdog water with toes

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2 years ago

In what situations are van der waals forces the most significant

viktelen [127]

Its most significant when all other forces are absent

7 0

3 years ago