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____ [38]
3 years ago
9

Perform the following operation

Chemistry
1 answer:
Gekata [30.6K]3 years ago
4 0

Explanation:

Perform the following operation

and express the answer in

scientific notation.

5.4x103 x 1.2x107

You might be interested in
how many molecule of carbon dioxide are needed to react with excess iron oxide to produce 11.6 g of iron
lesya692 [45]

Answer:

0.16 moles of Carbon

Explanation:

The balanced reaction equation:

2Fe_{2}O_{3} + 3C → 4Fe + 3CO_{2}↑

The mole ratio of Carbon to Iron is 3 : 4 (since Fe2O3 is in excess)

i.e 3 moles of C produces 4 moles of Fe.

If 1 mole of Fe - 55.8g of Fe

? moles - 11.6g of Fe

= \frac{11.6}{55.8} = 0.208 moles

But 3 moles of C - 4 moles of Fe

? moles of C - 0.208 moles of Fe

= \frac{3 *0.208}{4} = 0.16 moles of carbon.

I hope this explanation was clear and useful.

5 0
3 years ago
A particle with 10 protons, 11 neutrons, and 12 electrons has a mass number of:
garik1379 [7]

For any given element the mass number can be found by adding the protons and the neutrons.

In this case its 10 protons plus 11 neutrons which gives us 21 as the mass number.

7 0
2 years ago
What is the balanced chemical symbol equation for silicon + water?
Paladinen [302]

Answer: not 100% sure.

Explanation:

7 0
3 years ago
I need help with this question for homework
solong [7]
Octane is the resistance of the burning of gasoline

3 0
3 years ago
Consider the following reaction at constant P. Use the information here to determine the value of ΔSsurr at 355 K. Predict wheth
Elena-2011 [213]

Answer:

\Delta S_{surr} = + 0.32113\: kJ/K

Explanation:

Given: Entropy of surrounding: ΔSsurr = ?

Temperature: T= 355 K

The change in enthalpy of reaction: ΔH = -114 kJ

Pressure: P = constant

As we know, ΔH = -114 kJ ⇒ negative

Therefore, the given reaction is an exothermic reaction

Therefore, Entropy of surrounding at <em>constant pressure</em> is given by,

\Delta S_{surr} = \frac{-\Delta H}{T}

\therefore \Delta S_{surr} = -\left (\frac{-114 kJ}{355 K}  \right ) = + 0.32113\: kJ/K > 0

<u><em>In the given reaction:</em></u>

2NO(g) + O₂(g) → 2NO₂(g)

As, the number of moles of gaseous products is less than the number of moles of gaseous reactants.

\therefore \Delta S_{system} <  0

As we know, <em>for a spontaneous process, that the total entropy should be positive.</em>

\Delta S_{total} = \Delta S_{surr} + \Delta S_{system} > 0  

<u>Therefore, at the given temperature,</u>

  • if \Delta S_{surr} > \Delta S_{system} \Rightarrow \Delta S_{total} > 0 then the given reaction is spontaneous
  • if \Delta S_{surr} < \Delta S_{system} \Rightarrow \Delta S_{total} < 0 then the given reaction is non-spontaneous
6 0
3 years ago
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